Examiner's comment
The correct answer was B. Most candidates chose the correct answer but a few selected C or D as they were unsuccessful in assigning oxidation numbers or coordination numbers to the given complex ion. Section B overview The section contained questions from all aspects of modules 1, 2, 3 and 5 of the specification. Candidates found many of the questions, including those with an extended response nature, relatively straightforward and the majority managed to cope with the mathematical content. As a rule, candidates should aim to use unrounded calculator values in their intermediate calculations to avoid rounding errors in their final answer. Candidates should be reminded to present their numerical working clearly. They should also be advised to avoid leaving two different solution approaches without crossing one of them out. If they need to restart an answer, they would be well advised to make use of additional space as necessary rather than trying to write their answers in the margins with the order of steps difficult to follow. In more complicated calculations, where multiple different chemical species and quantities are involved, using appropriate symbols and subscripts/descriptors in brackets, as well as units, helps appropriately identify numbers provided as amounts in moles/concentrations/masses. Some candidates were less confident and knowledgeable of content shared with the AS specification and traditionally taught earlier on in the course. These were specifically: structure and bonding, reaction rates and redox reactions of the halogens. Candidates wrote far more than was necessary in some responses. Candidates should avoid repeating sentences which often introduce contradictions at the end of the response when expanding on written answers. Where candidates make use of additional space, it would be worth reminding them to write down the full question part: in many cases where questions had a number, part and subpart, the part or subpart was missing (or incorrect).
![1 The burette readings from a titration are shown below.
Initial reading / cm3 4.95
Final reading / cm3 23.10
The burette used has an uncertainty of 0.05 cm3 for each reading.
What is the percentage uncertainty of the resulting titre?
A 0.22%
B 0.28%
C 0.44%
D 0.55%
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_01.webp)
![2 How many p electrons does an atom of chlorine have?
A 5
B 7
C 11
D 17
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_02.webp)
![3 What is the number of hydrogen atoms in 6.8 g NH3?
A 2.408 × 1023
B 3.612 × 1023
C 7.224 × 1023
D 1.806 × 1024
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_03.webp)
![4 Which reaction to extract iron (Fe) has the highest atom economy?
A 2Al + Fe2O3 2Fe + Al 2O3
B FeO + CO Fe + CO2
C Fe2O3 + 3CO 2Fe + 3CO2
D 2Fe2O3 + 3C 4Fe + 3CO2
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_04.webp)
![5 Phosphorus is burnt in oxygen to produce a mixture of oxides.
Which oxide has the closest to 50% by mass of phosphorus?
A PO2
B P2O3
C P2O5
D P4O9
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_05.webp)
![6 What is the oxidation number of S in Na2S2O3?
A –4
B –2
C +2
D +4
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_06.webp)
![7 Which of the following is not a redox reaction?
A CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
B NaOH(aq) + HCl (aq) NaCl (aq) + H2O(l)
C 2KCl O3(s) 2KCl (s) + 3O2(g)
D Fe(s) + H2SO4(aq) FeSO4(aq) + H2(g)
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_07.webp)
![8 Which compound has molecules with a trigonal planar shape?
A BeCl 2
B BCl 3
C NCl 3
D PCl 3
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_08.webp)
![9 Which equation describes the second ionisation energy of magnesium?
A Mg(g) Mg2+(g) + 2e–
B Mg(s) Mg2+(g) + 2e–
C Mg+(g) Mg2+(g) + e–
D Mg2+(g) + e– Mg+(g)
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_09.webp)
![10 Which molecule is polar?
A H2S
B CO2
C CCl4
D C2F4
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_10.webp)
![11 The equation for the complete combustion of methanol, CH3OH, is shown below.
CH3OH(l) + 11
2O2(g) CO2(g) + 2H2O(l)
The table shows standard enthalpy changes of formation, Δf Ho, in kJ mol–1.
Substance CH3OH(l) O2(g) CO2(g) H2O(l)
ΔfH o / kJ mol–1 –239 0 –393 –286
What is the enthalpy change of combustion of CH3OH(l), in kJ mol–1?
A +726
B +440
C – 440
D –726
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_11.webp)
![12 Hydrogen and iodine react in the reaction below.
H2(g) + I2(g) 2HI(g)
Which row is correct when pressure is increased?
Rate of reaction Equilibrium yield of HI
A Increases Increases
B Increases No effect
C Increases Decreases
D Decreases No effect
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_12.webp)
![13 Which statement is not a sustainability benefit of an industrial process using a catalyst?
A Lower temperatures can be used.
B The position of equilibrium moves towards the products.
C The reaction takes place in less time.
D There is reduced energy demand.
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_13.webp)
![14 The skeletal formulae of four alcohols, W, X, Y, Z, are shown below.
OH
W
OH
X
OH
Y
Z OH
Which pair of alcohols are structural isomers of each other?
A W and X
B W and Y
C W and Z
D X and Y
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_14.webp)
![15 A compound is shown below.
What is the systematic name of this compound?
F CH3
C C
CH3CH2 H
A E-3-fluoropent-2-ene
B E-3-fluoropent-3-ene
C Z-3-fluoropent-2-ene
D Z-2-fluoropent-3-ene
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_15.webp)
![16 Which equation is a propagation step in the catalytic breakdown of ozone?
A C2F2Cl 2 C2F2Cl • + Cl •
B O3 + O 2O2
C Cl • + Cl • Cl 2
D Cl O• + O Cl • + O2
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_16.webp)
![17 How many structural isomers of C5H12O are secondary alcohols?
A 1
B 2
C 3
D 4
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_17.webp)
![18 The hydrolysis of 1-iodopropane by aqueous potassium hydroxide takes place at a faster rate
than 1-bromopropane.
Which statement explains the different rates of reaction?
A Iodine is less reactive than bromine.
B The C–I bond enthalpy is less than the C–Br bond enthalpy.
C The C–I bond is less polar than a C–Br bond.
D The C–I bond length is shorter than the C–Br bond length.
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_18.webp)
![19 In a mass spectrum, which alkene is likely to have a fragment ion at m / z = 29?
A H2C=CHCH=CH2
B H2C=C(CH3)2
C H3CCH=CHCH3
D H3CCH=CHCH2CH3
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_19.webp)
![20 The IR spectrum of a compound is shown below.
100
80
60
transmittance
(%)
40
20
0
4000 3000 2000 1500 1000 400
wavenumber / cm–1
Which compound could have produced the IR spectrum?
A CH3CH=CH2
B CH3CH2CHO
C CH3CH2CH2OH
D CH3CH2COOH
Your answer [1]](/img/JUN25_H0321/JUN25_H0321_20.webp)
![1 The table shows the number of protons and neutrons in four different atoms.
Atom Number of protons Number of neutrons
W 17 18
X 18 18
Y 19 18
Z 18 19
Which two atoms are isotopes of the same element?
A W and X
B X and Y
C X and Z
D Y and Z
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_01.webp)
![2 11.895 g of hydrated cobalt(II) chloride, CoCl 2•xH2O, is heated to remove the water of
crystallisation.
After heating to constant mass, the mass of the anhydrous salt was 6.495 g.
What is the value of x?
A 3
B 5
C 6
D 7
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_02.webp)
![3 The diagram shows the Born-Haber cycle for sodium oxide, Na2O.
2Na+(g) + O2–(g)
2Na+(g) + O(g) + 2e–
2Na+(g) + O–(g) + e–
2Na(g) + O(g)
2Na(g) + ½O2(g)
2Na(s) + ½O2(g)
Na2O(s)
Why is the value for the second electron affinity of oxygen positive?
A An electron is added to a high energy orbital.
B An electron is added to a negative ion.
C An electron is removed from a gaseous atom.
D An electron is removed from a positive ion.
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_03.webp)
![4 What volume, in cm3, of 0.250 mol dm–3 barium hydroxide solution is required to exactly
neutralise 25.0 cm3 of 0.115 mol dm–3 hydrochloric acid?
Ba(OH)2(aq) + 2HCl (aq) BaCl 2(aq) + 2H2O(l)
A 5.75
B 11.50
C 23.00
D 54.35
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_04.webp)
![5 The graph shows the volume of hydrogen released over time in a chemical reaction.
100
90
80
70
60
Volume of
hydrogen 50
/ cm3
40
30
20
10
0
0 20 40 60 80 100
Time / s
What is the rate of reaction, in cm3 s–1, at 30 seconds?
A 0.8
B 1.2
C 2.1
D 2.4
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_05.webp)
![6 Methane reacts with oxygen as shown in the equation:
CH4(g) + 2O2(g) CO2(g) + 2H2O(g) ΔrH = –730 kJ mol–1
The table shows some bond enthalpies.
Bond O–H O=O C=O
Bond enthalpy / kJ mol–1 +464 +498 +805
What is the bond enthalpy, in kJ mol–1, of the C–H bond in methane?
A +109
B +367
C +435
D +568
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_06.webp)
![7 The table below shows the boiling points of some hydrogen halides.
Hydrogen halide Boiling point / K
HCl 188
HBr 206
HI 238
What is the best explanation for the trend in boiling points from HCl to HI?
A The strength of the covalent bonds increases.
B The strength of the hydrogen bonds increases.
C The strength of the induced dipole–dipole interactions (London forces) increases.
D The strength of the permanent dipole–dipole interactions increases.
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_07.webp)
![8 The burette readings from an experiment are shown:
Final reading / cm3 29.35
Initial reading / cm3 2.60
The burette has an uncertainty of ±0.05 cm3.
What is the percentage uncertainty of the titre?
A 0.17%
B 0.19%
C 0.34%
D 0.37%
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_08.webp)
![9 Hydrogen reacts with iodine monochloride, ICl , as shown in the equation:
H2 + 2ICl 2HCl + I2
The mechanism for the reaction is:
H2 + ICl HCl + HI slow step
HI + ICl HCl + I2 fast step
What is the rate equation for the reaction between H2 and ICl ?
A rate = k [HI] [ICl ]
B rate = k [H2] [ICl ]
C rate = k [H2] [ICl ]2
D rate = k [H2] [HI] [ICl ]2
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_09.webp)
![10 The overall equation for a hydrogen–oxygen fuel cell is:
H2(g) + 1 2O2(g) H2O(l)
The half-equation at the negative electrode is:
H2(g) + 2OH–(aq) 2H2O(l) + 2e–
What is the half-equation at the positive electrode?
A 1 2O2(g) + H2(g) 2H2O(l) + 2e–
B 1 2O2(g) + H2O(l) 2OH–(aq) + 2e–
C 1 2O2(g) + H2O(l) + 2e– 2OH–(aq)
D O2(g) + 2OH–(aq) + H2(g) + 2e– 2H2O(l)
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_10.webp)
![11 Two redox systems are shown below.
Mg2+(aq) + 2e– Mg(s) E ɵ= – 2.37 V
Pb2+(aq) + 2e– Pb(s) E ɵ = – 0.13 V
Which species is the strongest reducing agent?
A Mg2+(aq)
B Mg(s)
C Pb2+(aq)
D Pb(s)
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_11.webp)
![12 The rate constant, k, for a first order reaction is 6.19 × 10–3 s–1.
What is the half-life, in s, for the reaction?
A 4.29 × 10–3
B 49
C 112
D 323
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_12.webp)
![13 A mixture of ethanoic acid and ethanol is left to reach equilibrium.
A student determines the amount of ethanoic acid remaining in the equilibrium mixture by titrating
the mixture with a solution of sodium hydroxide.
Which row of the table shows a suitable indicator for the titration?
pH range of the indicator
A 1.2 – 2.8
B 4.8 – 6.0
C 9.4 –10.6
D 12.0 –13.4
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_13.webp)
![14 Barium is in Group 2 of the periodic table.
Which statement(s) about barium is / are correct?
1 Its outer shell electrons are in an s-orbital.
2 It reacts more vigorously with water than magnesium.
3 It has a higher first ionisation energy than magnesium.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_14.webp)
![15 Chromium forms the complex ions [Cr(NH3)6]3+ and [Cr(OH)6]3–.
Which statement(s) about the complexes is / are correct?
1 Chromium is in the same oxidation state in each complex ion.
2 The complex ions are different colours.
3 The complex ions have different coordination numbers.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN25_H4321/JUN25_H4321_15.webp)
![1 Which compound is alicyclic and unsaturated?
A
B
C
D
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_01.webp)
![2 0.0200 mol of the compound below reacts with Br2(aq) to make a saturated compound.
How many grams of Br2 are needed for this reaction?
Cl
A 3.20
B 6.39
C 7.99
D 12.80
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_02.webp)
![3 The skeletal structure of a medicinal drug is shown below.
How many hydrogen atoms are in its molecular formula?
H
N
Cl
Cl
A 14
B 15
C 17
D 19
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_03.webp)
![4 Which diagram shows the correct way to set up apparatus for converting ethanol to ethanoic
acid?
water out water in
A B
water in water out
water out water in
water in water out
C D
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_04.webp)
![5 0.200 mol of HOOCCH2CH2COOH is reacted with 0.300 mol NaOH.
How many water molecules are formed?
A 1.204 × 1023
B 1.806 × 1023
C 2.408 × 1023
D 3.612 × 1023
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_05.webp)
![6 Propene can be prepared using the reactions shown.
Which reaction has the lowest atom economy?
A C3H7Br C3H6 + HBr
B C12H26 2C3H6 + C6H14
C C8H18 C3H6 + C5H12
D C3H7OH C3H6 + H2O
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_06.webp)
![7 What are the organic products of the acid hydrolysis of CH3CH2CONHCH3?
A CH3CH2COO– + CH3NH3 +
B CH3CH2COOH + CH3NH3 +
C CH3CH2COOH + CH3NH2
D CH3CH2COO– + CH3NH2
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_07.webp)
![8 Ethene can be reacted with hydrogen bromide.
Which statement about this reaction is correct?
A H– acts as a nucleophile.
B Br+ acts as an electrophile.
C Hδ+ — Br δ– acts as an electrophile.
D Hδ+ — Br δ– acts as a nucleophile.
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_08.webp)
![9 Which reagents could a student use to prepare the ester shown?
O
CH3CH2 C O
O
A
CH3CH2 C OH + HO
B CH3CH2 OH + HOOC
C CH3CH2CH2 OH + HOOC
O
D
CH3CH2 C Cl + HO
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_09.webp)
![10 How many stereoisomers does the compound CH3CH(Br)CH=CHCH(Cl )CH3 have?
A 2
B 4
C 6
D 8
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_10.webp)
![11 Which molecule does not produce a mass spectrum containing a peak at m/z = 29?
OH
A
O
B
O
C
O
O
D
O OH
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_11.webp)
![12 Which process does not involve infrared radiation?
A Catalytic ozone depletion
B Monitoring toxic gases in the air
C Measuring ethanol in breathalyser tests
D Global warming
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_12.webp)
![13 Which molecule(s) would form a ketone group when oxidised?
OH
1
HO OH
O
2
HO OH
3
OH
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_13.webp)
![14 The structure of vitamin C is shown.
HO OH
OH
O
O
OH
Which reagent(s) will react with vitamin C?
1 Aqueous bromine water
2 Acidified potassium dichromate(VI)
3 Aqueous silver nitrate in ethanol
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_14.webp)
![15 Which compound(s) has/have three peaks in their 13C NMR spectrum?
OH
1
OH
OH
2
HO
HO OH
3
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN25_H4322/JUN25_H4322_15.webp)
![1 Which diagram shows a p‑orbital?
A
B
C
D
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_01.webp)
![2 Which row shows the atomic structure of 25Mg2+?
Protons Neutrons Electrons
A 10 12 13
B 10 15 12
C 12 13 10
D 12 13 14
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_02.webp)
![3 A nitrogen oxide contains 36.84% of nitrogen by mass.
What is the empirical formula of the nitrogen oxide?
A NO
B NO2
C N2O
D N2O3
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_03.webp)
![4 Carbon monoxide reacts with oxygen to form carbon dioxide:
2CO(g) + O2(g) 2CO2(g)
Which volumes of CO(g) and O2(g) produce the largest volume of CO2(g)?
All gas volumes are measured at RTP.
A 1.00 dm3 CO and 4.00 dm3 O2
B 2.00 dm3 CO and 3.00 dm3 O2
C 3.00 dm3 CO and 2.00 dm3 O2
D 4.00 dm3 CO and 1.00 dm3 O2
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_04.webp)
![5 Which reaction produces a product with linear molecules?
A 2B + 3F2
B C + O2
C 2H2 + O2
D N2 + 3H2
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_05.webp)
![6 Which statement about the periodic table is not correct?
A Elements in the same group have similar chemical properties.
B The elements are ordered by increasing atomic mass.
C The elements are ordered by increasing atomic number.
D There is a repeating trend of physical and chemical properties across the periods.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_06.webp)
![7 Group 2 compounds can be used in agriculture to neutralise acid soils and in medicine to treat
indigestion.
Which Group 2 compound is not suitable for either use?
A Mg(OH)2
B MgSO4
C CaCO3
D CaO
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_07.webp)
![8 In the UK, water companies typically treat drinking water with chlorine gas at a concentration of
0.500 mg dm–3 or less.
Which statement about UK drinking water is correct?
A Chlorine in drinking water can catalyse the breakdown of ozone.
B Chlorine may form toxic chlorinated hydrocarbons.
C Drinking water with a chlorine gas concentration of 0.500 mg dm–3 contains 2.12 × 1018
chlorine molecules in each dm3.
D In hot weather, chlorine can vaporise from drinking water to cause global warming.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_08.webp)
![9 Which reaction does not show disproportionation of chlorine?
A MnO2 + 4HCl MnCl 2 + Cl 2 + 2H2O
B Cl 2 + H2O HCl + HCl O
C 2Cl O2 + 2NaOH NaCl O2 + NaCl O3 + H2O
D 2NaOH + Cl 2 NaCl + NaCl O + H2O
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_09.webp)
![10 An unknown compound is tested to identify whether it contains sulfate, carbonate or halide ions.
What is the correct sequence of tests required?
A carbonate, halide, sulfate
B carbonate, sulfate, halide
C halide, carbonate, sulfate
D sulfate, carbonate, halide
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_10.webp)
![11 An enthalpy cycle is shown below.
ΔrH
C(s) + ½O2(g) CO(g)
+ ½O2(g) + ½O2(g)
ΔcH = –393 kJ mol–1 ΔcH = –283 kJ mol–1
CO2(g)
What is ΔrH, in kJ mol–1, shown in the enthalpy cycle?
A +676
B +110
C –110
D –676
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_11.webp)
![12 A mixture of gases is heated in a closed container. The reaction rate increases.
Which statement explains why the rate increases?
A More molecules have an energy greater than the activation energy.
B The activation energy decreases.
C The activation energy increases.
D The concentration of the gases increases.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_12.webp)
![13 The reversible reaction below is at equilibrium.
2SO2(g) + O2(g) 2SO3(g)
What is the expression for Kc?
[SO2(g)]2 [O2(g)]
A
[SO3(g)]2
[SO3(g)]2
B
[SO2(g)]2 [O2(g)]
2[SO2(g)] + [O2(g)]
C
2[SO3(g)]
2[SO3(g)]
D
2[SO2(g)] + [O2(g)]
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_13.webp)
![14 What is the name of the compound below?
Cl OH
A 1‑chloro‑1,2‑dimethylpropan‑3‑ol
B 2‑chloro‑3‑methylbutan‑4‑ol
C 3‑chloro‑2‑methylbutan‑1‑ol
D 3‑chloro‑2,3‑dimethylpropan‑1‑ol
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_14.webp)
![15 The structure of a hydrocarbon is shown below.
Which terms describe this hydrocarbon?
A Alicyclic and saturated
B Aliphatic and alicyclic
C Aliphatic and aromatic
D Aromatic and unsaturated
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_15.webp)
![16 Which property explains the low reactivity of alkanes?
A Low C–C bond enthalpy.
B Low bond enthalpy of π‑bonds.
C Low polarity of σ‑bonds.
D Low reactivity of carbon and hydrogen.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_16.webp)
![17 The repeat unit of an addition polymer is shown below.
CH3 Cl
C C
H H
Which statement about this addition polymer is correct?
A Combustion produces toxic alkaline fumes.
B The addition polymer is biodegradable.
C The monomer is H3CCH=CHCl.
D The repeat unit above is shown as a displayed formula.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_17.webp)
![18 Which functional groups are present in the compound below?
O
O
OH
A Alcohol and aldehyde.
B Alcohol and ketone.
C Carboxylic acid and aldehyde.
D Carboxylic acid and ketone.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_18.webp)
![19 Which statement about infrared radiation (IR) is not correct?
A Absorption of IR by molecules such as CO2, H2O and CH4 has been linked to global
warming.
B IR causes CFC molecules to produce chlorine radicals that initiate ozone breakdown in the
upper atmosphere.
C IR causes some covalent bonds to vibrate more and absorb energy.
D IR is used in modern breathalysers to detect ethanol.
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_19.webp)
![20 An alcohol CH3CH2CH(CH3)OH produces a mass spectrum.
The mass spectrum contains a large fragment ion at m/z = 45.
What is the possible identity of this fragment ion?
A CH2CHOH+
B CH2CH2OH+
C CH3CHOH+
D CH3CH2CH+
Your answer [1]](/img/JUN24_H0321/JUN24_H0321_20.webp)
![1 Oxygen has the electron configuration 1s22s22p4.
How are the electrons in an atom of oxygen arranged in the p-orbitals?
A
↑↑ ↑↑
B
↑↓ ↑↓
C
↑↑ ↑ ↑
D
↑↓ ↑ ↑
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_01.webp)
![2 Water has the anomalous properties below.
• Water has relatively high melting and boiling points.
• Ice is less dense than water.
Which statement explains these anomalous properties?
A The covalent bonding within water molecules.
B The hydrogen bonding between water molecules.
C The induced dipole–dipole interactions (London forces) between water molecules.
D The ionic bonding between water molecules.
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_02.webp)
![3 Which chemical process is the most sustainable in terms of the atom economy of the iron
produced?
A Fe2O3 + 3CO 2Fe + 3CO2
B Fe2O3 + 3H2 2Fe + 3H2O
C 2Fe2O3 4Fe + 3O2
D 2Fe2O3 + 3C 4Fe + 3CO2
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_03.webp)
![4 Which compounds of magnesium can be used as ‘antacids’?
A Chlorides
B Hydroxides
C Nitrates
D Sulfates
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_04.webp)
![5 Which statement explains the trend in boiling points down the halogens group?
A The bond enthalpy of the covalent bonds increases.
B The halogens become less electronegative.
C The induced dipole–dipole interactions (London forces) become stronger.
D The reactivity of the halogens decreases.
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_05.webp)
![6 Which equation does not represent a disproportionation reaction?
A Cl 2 + H2O HCl O + HCl
B Cl 2 + 2NaOH NaCl O + NaCl + H2O
C 4KCl O3 KCl + 3KCl O4
D 4HCl + MnO2 MnCl 2 + Cl 2 + 2H2O
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_06.webp)
![7 The equation for the reaction of sulfuric acid with potassium hydroxide is shown below.
H2SO4(aq) + 2KOH(aq) K2SO4(aq) + 2H2O(l)
25 cm3 of 1.00 mol dm–3 H2SO4 is reacted with excess KOH.
The energy given out is 2.8 kJ.
What is the enthalpy change of neutralisation, in kJ mol–1?
A –56
B –70
C –112
D –224
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_07.webp)
![8 Which row in the table explains how a catalyst affects the activation energy (Ea) and the
proportion of molecules with energy > Ea?
How the activation Proportion of molecules
energy changes with energy > Ea
A decreases decreases
B decreases increases
C increases decreases
D increases increases
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_08.webp)
![9 A graph of ln(k) is plotted against 1 / T for a reaction.
(k = rate constant, T = temperature in K.)
The gradient has the numerical value of –16 000.
What is the activation energy, in kJ mol–1, for this reaction?
A +1.92
B +133
C +1920
D +133 000
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_09.webp)
![10 A reaction is zero order with respect to a reactant.
Which rate–concentration graph for the reactant is the correct shape?
A
B
C
D
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_10.webp)
![11 The reversible reaction between hydrogen and iodine to form hydrogen iodide is
H2(g) + I2(g) 2HI(g)
The graph shows how the concentrations of the reactants and product change as the reaction
reaches a dynamic equilibrium.
At which point on the graph is the equilibrium reached?
A B C D
concentration
product
reactants
time
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_11.webp)
![12 Which solution can be added to CH3COOH(aq) to make a buffer solution?
A CH3COONa(aq)
B HCOOH(aq)
C HCl (aq)
D NaCl (aq)
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_12.webp)
![13 A student analyses a solution of a salt.
The results are shown below.
Test Observation
Reaction with NaOH(aq) Green precipitate
Reaction with Ba(NO3)2(aq) White precipitate
What is the formula of the salt?
A CuCl 2
B CuSO4
C FeCl 2
D FeSO4
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_13.webp)
![14 Chlorine has the electron configuration [Ne]3s23p5.
Which statement(s) about chlorine is/are correct when it reacts in redox reactions?
1 It can gain one electron to form 1– ions.
2 It can lose its 3s2 electrons to form 2+ ions.
3 It can lose its 3p5 electrons to form 5+ ions.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_14.webp)
![15 Which statement(s) about elements in the periodic table is/are correct?
1 The position of an element is determined by its relative atomic mass.
2 The elements in a group have similar chemical properties.
3 Transition elements are used as catalysts in the manufacture of chemicals.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN24_H4321/JUN24_H4321_15.webp)
![1 All organic compounds have covalent bonds.
What is the electrostatic attraction in a covalent bond between?
A A shared pair of electrons and the nuclei of the bonded atoms
B Cations and delocalised electrons
C Oppositely charged ions
D Two molecules
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_01.webp)
![2 Hydrogen reacts much more readily with alkenes than with alkanes.
Why is this?
A Alkenes are polar molecules whereas alkanes are not.
B All atoms in an alkane have a full outer shell of electrons.
C The bond enthalpy of C–C σ bonds is higher than that of π bonds.
D The bond enthalpy of C–C σ bonds is lower than that of π bonds.
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_02.webp)
![3 A student investigates the rate of hydrolysis of different iodoalkanes using aqueous silver nitrate
in ethanol.
What colour of precipitate is seen?
A Brown
B Cream
C White
D Yellow
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_03.webp)
![4 The structure of but-1-ene is shown below.
x
y
Which row has the correct shape around carbon atoms labelled x and y?
x y
A Tetrahedral Pyramidal
B Trigonal planar Tetrahedral
C Trigonal planar Pyramidal
D Pyramidal Tetrahedral
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_04.webp)
![5 Geraniol, shown below, is a component in many natural oils.
OH
Geraniol
Which pair of reagents identifies both functional groups in geraniol?
A Acidified dichromate(VI) and 2,4-dinitrophenylhydrazine.
B Bromine water and 2,4-dinitrophenylhydrazine.
C Bromine water and acidified dichromate(VI).
D Tollens’ reagent and aqueous silver nitrate in ethanol.
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_05.webp)
![6 4.30 g of the alcohol C5H9OH, (Mr = 86.0), is burned in oxygen.
C5H9OH(l) + 7O2(g) 5CO2(g) + 5H2O(l)
Which volume of oxygen gas is needed, in dm3, for this complete combustion of C5H9OH,
at RTP?
A 1.2
B 2.4
C 5.8
D 8.4
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_06.webp)
![7 Which statement gives a valid scientific reason for global warming?
A Infrared radiation causes bonds in CH4 molecules to vibrate more.
B Infrared radiation causes O2 molecules to vibrate more.
C Ultraviolet radiation causes bonds in CO2 to vibrate more.
D Ultraviolet radiation causes bonds in CFC molecules to break.
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_07.webp)
![8 The CFC CCl 2F2 can cause the breakdown of ozone in the upper atmosphere.
Which initiation step could occur with ultraviolet radiation to catalyse this breakdown?
A CCl 2F2 ●C + ●Cl 2F2
B CCl 2F2 ●F + ●CCl 2F
C CCl 2F2 ●Cl + ●CCl F2
D CCl 2F2 ●Cl 2 + ●CF2
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_08.webp)
![9 Which compound is a secondary amide?
N
A
OH O
N C
B H
O
O
C
N
H
OH
NH2
D HO C
O
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_09.webp)
![10 1.35 g of ethylamine gas, CH3CH2NH2 (Mr = 45.0), is reacted with 20 cm3 of 2.0 mol dm–3
hydrochloric acid forming a solution of ethylammonium chloride.
CH3CH2NH2(g) + HCl (aq) CH3CH2NH3 +(aq) + Cl –(aq)
What is the concentration of ethylammonium chloride in mol dm–3?
A 0.03
B 0.67
C 1.50
D 2.00
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_10.webp)
![11 Which compound could have produced the IR spectrum shown below?
100
Transmittance
(%) 50
0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1
A HOCH2CHO
B CH3CH2COOH
C CH3CH2COOCH3
D (CH3)2C(OH)COOH
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_11.webp)
![12 1,6-Diaminohexane, H2N(CH2)6NH2, reacts with hexanedioyl dichloride, Cl OC(CH2)4COCl to
form a polyamide and one other product.
What is the other product formed in this reaction?
A HCl
B H2O
C CO
D NH3
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_12.webp)
![13 A sample containing a mixture of 3 components, X, Y and Z, is analysed using gas
chromatography.
The gas chromatogram below is obtained.
The relative peak areas of X, Y and Z are included.
Z
Relative peak areas
X = 1.0
1000 Y
Y = 3.5
Z = 5.5
X
Recorder response
500
0
0 5 10 15
Time / min
Which statement(s) is/are true?
1 The peak for component X shows the mass of one mole.
2 Component Y stays in the column for longer than component X.
3 Component Z consists of more than half of the sample.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_13.webp)
![14 The structures of 3 compounds, 1, 2 and 3, are shown below.
Which compound(s) would produce a carbon-13 NMR spectrum with 2 peaks?
HO
OH
1 2 3
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_14.webp)
![15 Polymers, such as poly(chloroethene), shown below, are difficult to dispose of.
H Cl
C C
H H
Poly(chloroethene)
Which statement(s) is/are true about poly(chloroethene)?
1 It is a photodegradable or biodegradable polymer.
2 When incinerated, it produces toxic waste products which need to be removed.
3 It can be recycled and processed for use as an organic feedstock.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN24_H4322/JUN24_H4322_15.webp)
![1 Which statement explains the trend in boiling points down the halogens group?
A Covalent bonds become stronger.
B Induced dipole–dipole interactions (London forces) become stronger.
C Ionic bonds become stronger.
D Permanent dipole–dipole interactions become stronger.
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_01.webp)
![2 A hydrocarbon contains 85.71% carbon by mass.
What is the empirical formula of the hydrocarbon?
A CH
B CH2
C CH4
D C2H4
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_02.webp)
![3 Hydrogen can be prepared industrially by the reaction of methane with steam.
The equation is shown below.
CH4(g) + 2H2O(g) 4H2(g) + CO2(g)
What is the atom economy of hydrogen for this process?
A 3.8%
B 4.3%
C 15.4%
D 17.4%
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_03.webp)
![4 How many p-orbitals are occupied by electrons in a sulfur atom?
A 2
B 4
C 6
D 10
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_04.webp)
![5 Which substance has the lowest oxidation number for sulfur?
A Na2SO4
B S8
C SF2
D SO2
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_05.webp)
![6 Successive ionisation energies, in kJ mol–1, of an element in Period 3 of the periodic table are
shown below.
1st 2nd 3rd 4th 5th 6th 7th 8th 9th
578 1817 2745 11578 14831 18378 23296 27460 31862
What is the formula of the oxide of the Period 3 element?
A Na2O
B MgO
C Al 2O3
D SiO2
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_06.webp)
![7 How many oxygen atoms are in 120.2 g of SiO2?
A 3.01 × 1023
B 1.20 × 1024
C 2.41 × 1024
D 3.61 × 1024
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_07.webp)
![8 Magnesium nitrate, Mg(NO3)2, decomposes when heated:
Mg(NO3)2(s) MgO(s) + 2NO2(g) + ½O2(g)
0.00250 mol of Mg(NO3)2 is decomposed.
What is the volume of gas produced, measured at RTP?
A 30 cm3
B 60 cm3
C 120 cm3
D 150 cm3
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_08.webp)
![9 Zinc reacts with aqueous silver nitrate, as shown in the equation:
Zn(s) + 2AgNO3(aq) 2Ag(s) + Zn(NO3)2(aq)
0.10 g of zinc is added to 15 cm3 of 0.25 mol dm–3 aqueous silver nitrate.
What is the mass of silver metal that would be formed?
A 0.16 g
B 0.20 g
C 0.33 g
D 0.40 g
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_09.webp)
![10 15.00 cm3 of 18.0 mol dm–3 concentrated hydrochloric acid is diluted with water to prepare
250 cm3 of dilute hydrochloric acid.
What is the concentration, in mol dm–3, of the dilute hydrochloric acid?
A 0.0675
B 0.270
C 0.300
D 1.08
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_10.webp)
![11 The standard enthalpy change of formation of water is –286 kJ mol–1.
Which statement or equation is correct?
A H2(g) + ½O2(g) H2O(l) ΔH o = –143 kJ mol–1
B 2H2(g) + O2(g) 2H2O(l) ΔH o = –286 kJ mol–1
C The O–H bond enthalpy is –143 kJ mol–1.
D The standard enthalpy change of combustion of hydrogen is –286 kJ mol–1.
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_11.webp)
![12 Which statement about energy changes is correct?
A Combustion of an alkane is endothermic.
B In an exothermic reaction, more energy is needed to break bonds than is given out when
bonds are made.
C The activation energy is a negative value.
D The enthalpy change for the condensation of a gas to a liquid is a negative value.
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_12.webp)
![13 The Boltzmann distribution showing the activation energy, Ea, for an uncatalysed reaction is
shown below.
number of
molecules
Ea
energy
What is the difference for the catalysed reaction?
A The activation energy shifts to the left.
B The activation energy shifts to the right.
C The curve flattens.
D The curve shifts to the right.
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_13.webp)
![14 A student measures how the OH– concentration changes over time for a reaction.
The student plots the graph below.
0.20
0.15
[OH–(aq)]
0.10
/ mol dm–3
0.05
0.00
0 100 200 300 400 500 600
time / s
What is the rate of reaction, in mol dm–3 s–1, at 200 s?
A 2.2 × 10–4
B 2.8 × 10–4
C 1.8 × 10–3
D 4.4 × 10–2
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_14.webp)
![15 Which formula does not represent 3-methylbut-1-ene?
A CH3CHCH3CHCH2
B CH2CHCH(CH3)2
C
D
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_15.webp)
![16 How many structural isomers have the molecular formula C4H9Cl ?
A 2
B 3
C 4
D 5
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_16.webp)
![17 3-Methylcyclohexanol is reacted with NaBr and H2SO4.
What is the organic product?
Br
A
Br
B
C
D
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_17.webp)
![18 A student has planned the two-stage synthesis shown below.
H OH OH
H3C
C C Intermediate H3C C C H
H3C H CH3 H
Which compound could be the intermediate for this synthesis?
H H
A H3C C C H
CH3 H
Br H
B H3C C C H
CH3 H
OH H
C H3C C C H
CH3 H
Br Br
D H3C C C H
CH3 H
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_18.webp)
![19 An organic compound produces the infrared spectrum below.
100
transmittance
50
(%)
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
Which compound could have produced this IR spectrum?
A CH3CH2CH=CH2
B CH3CHOHCH2CH3
C CH3CH2COCH3
D (CH3)2CHCOOH
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_19.webp)
![20 Pentan-2-ol and pentan-3-ol are structural isomers with the molecular formula C5H12O and
Mr = 88.
The isomers can be distinguished from the fragment ions in their mass spectra.
Which fragment ion would you expect to be present in only one of these isomers?
A m/z = 29
B m/z = 45
C m/z = 59
D m/z = 73
Your answer [1]](/img/JUN23_H0321/JUN23_H0321_20.webp)
![1 Which sample contains the greatest number of molecules?
A 35.0 g of C2H2
B 45.0 g of C2H6
C 60.0 g of C4H10
D 100.0 g of C6H6
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_01.webp)
![2 0.688 g of an oxide of manganese is reduced by hydrogen gas to form manganese metal and
0.235 g of water.
What is the formula of the oxide of manganese?
A MnO
B MnO2
C Mn2O3
D Mn3O4
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_02.webp)
![3 How many hydrogen atoms are in 2.50 g of pharmacolite, CaHAsO4•2H2O
(Mr = 216.0)?
A 6.97 × 1021
B 2.09 × 1022
C 2.79 × 1022
D 3.48 × 1022
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_03.webp)
![4 40.0 cm3 of 0.200 mol dm–3 HCl is added to 60.0 cm3 of 0.100 mol dm–3 NaOH.
What is the concentration of the resulting solution?
A 0.0200 mol dm–3 HCl and 0.0200 mol dm–3 NaCl
B 0.0200 mol dm–3 HCl and 0.0400 mol dm–3 NaCl
C 0.0200 mol dm–3 HCl and 0.0600 mol dm–3 NaCl
D 0.0600 mol dm–3 HCl and 0.0200 mol dm–3 NaCl
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_04.webp)
![5 Which compound has polar molecules?
A HCN
B BCl3
C CO2
D C2F4
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_05.webp)
![6 Which element has the largest third ionisation energy?
A Li
B F
C Ne
D Na
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_06.webp)
![7 The reaction below is first order with respect to reactant X.
X(aq) products
When the initial concentration of X is 1.0 mol dm–3, the half-life is 16 minutes.
What is the half-life when the initial concentration of X is 2.0 mol dm–3?
A 2 minutes
B 4 minutes
C 8 minutes
D 16 minutes
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_07.webp)
![8 Which compound requires the most energy to convert one mole into its gaseous ions?
A NaF
B Na2O
C MgF2
D MgO
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_08.webp)
![9 The table below shows standard entropies, Sө.
Substance SO2(g) O2(g) SO3(l)
Sө/J K–1 mol–1 248 204 96
What is the standard entropy change, ∆Sө, in J K mol–1, for the formation of 1 mol of SO3(l) from
SO2(g) and O2(g)?
A –508
B –254
C +254
D +508
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_09.webp)
![10 What is the percentage dissociation of a 0.015 mol dm–3 solution of methanoic acid, HCOOH
(Ka = 1.60 × 10–4 mol dm–3)?
A 0.016%
B 1.1%
C 1.82%
D 10.3%
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_10.webp)
![11 A student adds aqueous potassium carbonate to one test tube and aqueous silver nitrate to a
second test tube.
The student adds dilute hydrochloric acid to each test tube.
Which row has the correct observations?
Aqueous potassium carbonate Aqueous silver nitrate
A no change precipitate
B no change no change
C effervescence no change
D effervescence precipitate
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_11.webp)
![12 The equations show the electrode potentials of the half-cells used in a lithium-ion cell.
E ө / V
Li+ + e– Li –3.04
Li+ + CoO2 + e– LiCoO2 +1.16
Which statement is correct in a lithium-ion cell?
A The cell potential is 2.88 V.
B The reaction at the positive electrode is: LiCoO2 Li+ + CoO2 + e–
C The overall cell reaction is: Li + CoO2 LiCoO2
D The oxidation number of Co changes from +2 to +1.
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_12.webp)
![13 Which substance(s) has/have induced dipole–dipole interactions (London forces) in the solid
state?
1 C2H6
2 H2O
3 Si
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_13.webp)
![14 Which statement(s) is/are correct for the anti-cancer complex Pt(NH3)2Cl 2?
1 It has bond angles of 90º.
2 The oxidation number of Pt is +4.
3 It forms both optical and cis-trans isomers.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_14.webp)
![15 Chlorine trifluoride can be decomposed into its elements forming the equilibrium mixture below.
2Cl F3(g) Cl 2(g) + 3F2(g) ∆H = +318 kJ mol–1
colourless green yellow
gas gas gas
Which statement(s) is/are correct?
1 The decomposition is a redox reaction.
2 When the equilibrium mixture is cooled, the colour fades.
3 The decomposition has a negative entropy change.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN23_H4321/JUN23_H4321_15.webp)
![1 Which compound is used for proton exchange in NMR spectroscopy?
A CCl4
B CDCl3
C D2O
D Si(CH3)4
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_01.webp)
![2 Which compound reacts with 2,4-dinitrophenylhydrazine but does not react with Tollens’
reagent?
A C6H5COCOOH
B C6H5CH(OH)CHO
C CH3COCHO
D CH3CH2CH(OH)CH3
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_02.webp)
![3 Propyne, CH3C≡CH, is a member of the alkynes homologous series with the C≡C functional group.
What is the general formula of the alkynes?
A CnH2n–4
B CnH2n–2
C CnH2n
D CnH2n+2
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_03.webp)
![4 The structure of the painkiller paracetamol is shown below.
OH
O
N
H
Paracetamol
Which functional groups are present in paracetamol?
A alcohol, amide
B alcohol, arene, ketone, amine
C phenol, amide
D phenol, ketone, amine
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_04.webp)
![5 Oxymetazoline, shown below, is used as a decongestant in the treatment of colds.
HO N
HN
Oxymetazoline
How many H atoms are in one molecule of oxymetazoline?
A 23
B 24
C 25
D 26
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_05.webp)
![6 Which statement supports the delocalised model of benzene and not the Kekulé model?
A Sigma bonds overlap to form a π-system.
B The carbon-carbon bond lengths are all the same.
C The enthalpy change of hydrogenation is more exothermic than expected.
D Benzene is more reactive than alkenes with bromine.
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_06.webp)
![7 What is the systematic name for the compound below?
A 3,5-dimethylocta-1,3,6-triene
B 3,5-dimethylocta-2,5,7-triene
C 4,6-dimethylocta-1,3,6-triene
D 4,6-dimethylocta-2,5,7-triene
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_07.webp)
![8 For complete combustion, 0.100 mol of an alkane requires 22.8 dm3 of O2, measured at RTP.
Which alkane has undergone complete combustion?
A pentane
B hexane
C heptane
D octane
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_08.webp)
![9 Which compound has the greatest number of peaks in its proton NMR spectrum?
O
A
O
Br
B Br
O O
C
HO OH
OH
D O
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_09.webp)
![10 Which ester is most likely to produce a mass spectrum with a fragment ion at m / z = 43?
OH O
A H3C C C O CH3
CH3
O
B
HO CH2 C O CH2CH2CH3
OH O
C H3C CH CH2 C O CH3
OH O
D
CH3CH2 C C O CH2CH2OH
CH3
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_10.webp)
![11 The infrared spectrum of an organic compound is shown below.
100
transmittance (%) 50
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
Which compound could have produced this spectrum?
A
COOH
B H3C OCOCH3
C HO CHO
D HOCH2 OCH3
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_11.webp)
![12 Which compound reacts with ethanoyl chloride?
O
A
O
B
O
Cl
C
O
D NH2
O
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_12.webp)
![13 Which compound(s) is/are aliphatic?
1
2
3
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_13.webp)
![14 Which compound(s) is/are hydrolysed by HCl (aq) to produce butanoic acid?
1 CH3CH2CH2COOCH3
2 CH3CH2CH2CH2CN
3 CH3CH2CH2CH2Cl
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_14.webp)
![15 Which ion(s) contain(s) bond angles of approximately 120º?
1 CH3COO–
2 C6H5O–
3 (CH3)3C+
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN23_H4322/JUN23_H4322_15.webp)
![1 Which substance has a giant covalent lattice structure in its solid state?
A potassium
B silicon
C sodium chloride
D water
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_01.webp)
![2 What is the meaning of the term electronegativity?
A The ability of an atom to attract the electrons in a covalent bond.
B The ability of an atom to gain an electron.
C The electrostatic attraction between a negative ion and a positive ion.
D The size of the charge on a negative ion.
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_02.webp)
![3 Which compound is an alkali?
A CH3COOH
B CH3OH
C HNO3
D NH3
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_03.webp)
![4 What is the number of paired orbitals in a sulfur atom?
A 4
B 6
C 7
D 8
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_04.webp)
![5 Which element has the lowest melting point?
A S
B P
C Cl
D Ar
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_05.webp)
![6 The first four ionisation energies of a Period 3 element X are shown in the table.
Ionisation energy / kJ mol–1
1st 2nd 3rd 4th
738 1451 7733 10 541
Element X is reacted with chlorine.
What is the formula of the chloride formed?
A XCl
B XCl 2
C XCl 3
D XCl 4
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_06.webp)
![7 A sample of lead(II) sulfate (M = 303.3 g mol–1) is decomposed by heat, as shown in the equation
below.
2PbSO4(s) → 2PbSO3(s) + O2(g)
The reaction forms 2.40 g of O2(g).
What is the mass of lead(II) sulfate that has been heated? Assume a 100% yield.
A 22.7 g
B 30.3 g
C 45.5 g
D 60.7 g
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_07.webp)
![8 Which volume of 18.0 mol dm–3 hydrochloric acid should be diluted to 250.0 cm3 to prepare a
0.450 mol dm–3 solution of hydrochloric acid?
A 4.50 cm3
B 6.25 cm3
C 10.0 cm3
D 32.4 cm3
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_08.webp)
![9 What is the number of ions in 4.00 mol of magnesium chloride, MgCl 2?
A 1.81 × 1024
B 2.41 × 1024
C 4.82 × 1024
D 7.22 × 1024
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_09.webp)
![10 What is the correct explanation for the trend in the boiling points of chlorine, bromine, and iodine
down the group?
A Bond enthalpy increases.
B Chemical reactivity decreases.
C Electronegativity decreases.
D London forces increase.
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_10.webp)
![11 Combustion of hydrazine, N2H4, produces NO2 and H2O as in the equation below.
N2H4(l) + 3O2(g) → 2NO2(g) + 2H2O(l)
The table shows standard enthalpy changes of formation, ∆f H o .
Substance ∆f H o / kJ mol−1
N2H4(l) +50.6
O2(g) 0
NO2(g) +33.2
H2O(l) –285.8
What is the enthalpy change of combustion, in kJ mol–1, for hydrazine, N2H4(l)?
A –555.8
B –303.2
C +303.2
D +555.8
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_11.webp)
![12 Which prediction can be made using le Chatelier’s principle?
A The effect of a catalyst on the reaction rate.
B The effect of a catalyst on the equilibrium position.
C The effect of temperature on the reaction rate.
D The effect of concentration on the equilibrium position.
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_12.webp)
![13 Four equilibrium reactions are set up.
The concentration of each gas in the equilibrium mixtures is 0.1 mol dm–3.
Which equilibrium has a numerical Kc value of 0.01?
A CH4(g) + 2H2O(g) CO2(g) + 4H2(g)
B N2(g) + 3H2(g) 2NH3(g)
C H2(g) + I2(g) 2HI(g)
D 2NO2(g) N2O4(g)
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_13.webp)
![14 What is the number of σ-bonds in the molecule below?
A 1
B 3
C 7
D 9
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_14.webp)
![15 What is the number of hydrogen atoms in one molecule of the compound below?
O OH
A 8
B 10
C 12
D 14
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_15.webp)
![16 Complete combustion of an alkane forms 30 cm3 of carbon dioxide and 40 cm3 of water vapour,
under the same conditions of temperature and pressure.
Which alkane has undergone complete combustion?
A butane
B ethane
C heptane
D propane
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_16.webp)
![17 Which alkene is an E stereoisomer?
CH3CH2 CH3
A C C
H H
H3C CH2CH3
B C C
H CH3
H CH3
C C C
CH3CH2 C(CH3)3
H3C CH3
D C C
H CH(CH3)2
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_17.webp)
![18 When heated with NaOH(aq), 1-chlorobutane is hydrolysed at a slower rate than 1-bromobutane.
Which statement explains the different rates?
A The C–Br bond enthalpy is greater than the C–Cl bond enthalpy.
B The C–Br bond enthalpy is less than the C–Cl bond enthalpy.
C The C–Br bond is less polar than the C–Cl bond.
D The C–Br bond is more polar than the C–Cl bond.
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_18.webp)
![19 Which organic compound could have produced the infrared spectrum below?
100
transmittance
50
(%)
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
A CH3COCH2CH3
B CH3CH2CHOHCH3
C CH3COCH2CH2OH
D CH3CH2COOH
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_19.webp)
![20 Which alcohol is likely to have fragment ions at m / z = 15, 29 and 43 in its mass spectrum?
OH
A
B
OH
OH
C
OH
D
Your answer [1]](/img/JUN22_H0321/JUN22_H0321_20.webp)
![1 An aqueous solution contains a mixture of chloride, bromide and iodide ions.
AgNO3(aq) is added to this mixture, followed by an excess of dilute NH3(aq).
The resulting mixture is then filtered.
Which compound(s) is/are present in the residue on the filter paper?
A AgCl only
B AgCl and AgBr
C AgBr only
D AgBr and AgI
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_01.webp)
![2 20 cm3 of nitrogen gas reacts with 10 cm3 of oxygen gas to form 20 cm3 of a gaseous product.
Which equation is the most likely for the reaction?
A N2(g) + O2(g) 2NO(g)
B N2(g) + 2O2(g) N2O4(g)
C 2N2(g) + O2(g) 2N2O(g)
D 2N2(g) + 2O2(g) 4NO(g)
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_02.webp)
![3 0.541 g of an element X is reacted with oxygen to form 0.790 g of the oxide X2O3.
What is the element X?
A Al
B Cr
C Ga
D Sc
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_03.webp)
![4 Hydrogen peroxide, H2O2, can be oxidised by manganate(VII) ions under acid conditions as
shown below.
2MnO4 –(aq) + 5H2O2(aq) + 6H+(aq) 2Mn2+(aq) + 5O2(g) + 8H2O(l)
In a titration, 25.00 cm3 of a disinfectant containing hydrogen peroxide reacts with 22.00 cm3 of
0.125 mol dm–3 KMnO4(aq).
What is the concentration of H2O2, in mol dm–3, in the disinfectant?
Assume that KMnO4 only reacts with H2O2 in the disinfectant.
A 0.0440
B 0.110
C 0.275
D 0.550
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_04.webp)
![5 The mass of 4 molecules of a substance is 2.125 × 10–22 g.
What is the possible formula of the substance?
A CH4
B O2
C SO2
D I2
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_05.webp)
![6 Prussian blue, C18Fe7N18, is a deep blue pigment containing Fe2+, Fe3+ and CN− ions.
What are the numbers of Fe2+ and Fe3+ ions in one formula unit of C18Fe7N18?
A 2 Fe2+ and 5 Fe3+
B 3 Fe2+ and 4 Fe3+
C 4 Fe2+ and 3 Fe3+
D 5 Fe2+ and 2 Fe3+
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_06.webp)
![7 Bond enthalpies are shown in the table.
Bond C–C C–H O–H C–O C=O O–O O=O
Bond
enthalpy 347 435 464 358 805 144 498
/ kJ mol–1
What is the enthalpy change, in kJ mol–1, for the reaction below?
CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
A –730
B –544
C +544
D +730
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_07.webp)
![8 The half-life for a first order reaction is 80 s.
What is the rate constant k, in s–1, for this reaction?
A 8.66 × 10–3
B 0.0125
C 55.5
D 115
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_08.webp)
![9 Which equation represents the change that accompanies the standard enthalpy change of
atomisation of bromine?
A ½ Br2(l) Br(g)
B Br2(l) 2Br(g)
C ½ Br2(g) Br(g)
D Br2(g) 2Br(g)
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_09.webp)
![10 For the condensation of ammonia gas, what are the signs of ∆H and ∆S?
A ∆H –ve ∆S –ve
B ∆H –ve ∆S +ve
C ∆H +ve ∆S +ve
D ∆H +ve ∆S –ve
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_10.webp)
![11 The equilibrium equation for an indicator, HA, is shown below.
Equation: HA(aq) A–(aq) + H+(aq)
Colour: Blue Yellow
The indicator is added to a solution. The indicator turns a yellow colour.
An excess of aqueous sodium hydroxide is then added.
Which statement describes how the colour of this solution would be expected to change?
A Colour changes from yellow to blue.
B Colour changes from yellow to green.
C Colour changes from yellow to green and then to blue.
D Colour stays yellow.
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_11.webp)
![12 Ammonia and water react to set up an acid–base equilibrium.
What are the Brønsted–Lowry acids in the equilibrium mixture?
A H2O and OH–
B OH– and NH3
C NH4 + and H2O
D NH4 + and NH3
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_12.webp)
![13 Standard electrode potentials for two redox systems are shown below.
Cr3+(aq) + 3e– Cr(s) –0.74 V
Cr3+(aq) + e– Cr2+(aq) –0.42 V
What is the standard electrode potential for Cr2+(aq) + 2e– Cr(s)?
A –0.32 V
B –0.90 V
C –1.16 V
D –1.80 V
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_13.webp)
![14 The three reactions below each form one product only.
Which reaction(s) form(s) a product with non-polar molecules?
1 2CO + O2
2 Si + 2Cl 2
3 S + 3F2
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_14.webp)
![15 Which ion(s) contain(s) one or more unpaired electrons?
1 Mn3+
2 V3+
3 Cu+
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN22_H4321/JUN22_H4321_15.webp)
![1 Which statement is correct for the different rates of hydrolysis of RCl and RBr?
A RBr is hydrolysed faster because Cl is more electronegative than Br.
B RBr is hydrolysed faster because the C–Cl bond enthalpy is greater than C–Br.
C RCl is hydrolysed faster because Cl is more electronegative than Br.
D RCl is hydrolysed faster because the C–Br bond enthalpy is greater than C–Cl.
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_01.webp)
![2 Which statement about absorption of radiation is correct?
A Infrared radiation can result in the breakdown of the ozone layer.
B Ultraviolet radiation can cause some polymers to photodegrade to benefit the environment.
C Ultraviolet radiation is linked to global warming.
D Ultraviolet radiation is used in modern breathalysers to measure ethanol in the breath.
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_02.webp)
![3 What is the number of sigma bonds in a molecule of methylbenzene?
A 7
B 10
C 12
D 15
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_03.webp)
![4 The skeletal formula of an organic compound is shown below.
N
OH
O
Which functional groups are present?
A amide and alcohol
B amide and carboxylic acid
C amine and carboxylic acid
D amine, ketone and alcohol
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_04.webp)
![5 The structure of a drug is shown below:
O
HO OH
HO
F
O
How many chiral carbon atoms are there in a molecule of the drug?
A 5
B 6
C 7
D 8
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_05.webp)
![6 Which process has the highest atom economy for preparing ethene, C2H4?
In each process, assume that ethene is the only product that is used.
A C10H22 3C2H4 + C4H10
B C6H14 2C2H4 + C2H6
C C2H5Cl C2H4 + HCl
D C2H5OH C2H4 + H2O
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_06.webp)
![7 Complete combustion of 0.050 mol of an alkane produces 5.40 g of H2O.
What is the molecular formula of the alkane?
A C2H6
B C3H8
C C4H10
D C5H12
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_07.webp)
![8 The structure of the painkiller, paracetamol, is shown below.
OH
O
N
H
paracetamol
A tablet contains 3.31 × 10–3 mol of paracetamol.
What is the mass of paracetamol in the tablet?
A 493 mg
B 497 mg
C 500 mg
D 506 mg
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_08.webp)
![9 The compound below reacts with hydrogen gas to form a saturated compound.
CN
What is the volume of hydrogen, measured at room temperature and pressure, that reacts with
0.0500 mol of the compound?
A 2.40 dm3
B 3.60 dm3
C 4.80 dm3
D 6.00 dm3
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_09.webp)
![10 Butyl propanoate is hydrolysed by aqueous sodium hydroxide.
Which compound is one of the products of this hydrolysis?
A C3H7ONa
B C3H5O2Na
C C4H9ONa
D C4H7O2Na
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_10.webp)
![11 The infrared spectrum of an organic compound is shown below.
100
Transmittance (%)
0
4000 3000 2000 1500 1000 500
Wavenumber / cm–1
Which compound could have produced this spectrum?
A H2C=CHCH2CH2OH
B CH3COOCH2CH3
C H2NCH2COOCH3
D (CH3)2CHCONH2
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_11.webp)
![12 Which compound produces two triplets in its 1H NMR spectrum?
A CH3CH2COOCH2CH3
B CH3CH2COCH2CH3
C HOOCCH2CH2COOH
D HOOCCH2CH2CH2COOH
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_12.webp)
![13 Which equation(s) could be part of the propagation step in the radical substitution of C5H12 to
form C5H11Cl ?
1 C5H11• + Cl 2 C5H11Cl + Cl •
2 C5H12 + Cl • C5H11Cl + H•
3 C5H11• + Cl • C5H11Cl
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_13.webp)
![14 Which species could react as a nucleophile?
1 NH3
2 OH–
3 CH3NH2
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_14.webp)
![15 Which isomer(s) of C5H12O has/have 4 peaks in its/their 13C NMR spectrum?
1 3-methylbutan-2-ol
2 2-methylbutan-2-ol
3 2-methylbutan-1-ol
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN22_H4322/JUN22_H4322_15.webp)
![1 Which compound has the highest boiling point?
A ethanol
B heptane
C sodium chloride
D water
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_01.webp)
![2 Pauling electronegativity values for the halogens F to I and some elements in period 2 of the
periodic table are shown below.
B C N O F
2.04 2.55 3.04 3.44 3.98
Cl
3.16
Br
2.96
I
2.66
Which bond has the correct polarity?
A B C D
δ– N—I δ+ δ– C—F δ+ δ– B—Cl δ+ δ– Br—Cl δ+
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_02.webp)
![3 Which compound releases hydroxide ions when it dissolves in water?
A CH3COOH
B HNO3
C H2SO4
D NH3
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_03.webp)
![4 Which alkane is 82.8% carbon by mass?
A CH4
B C2H6
C C4H10
D C8H18
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_04.webp)
![5 Which gas sample has the greatest mass at RTP?
A 50 cm3 of Ar(g)
B 100 cm3 of O2(g)
C 150 cm3 of N2(g)
D 200 cm3 of Ne(g)
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_05.webp)
![6 A student mixes 250.0 cm3 of 0.100 mol dm–3 KOH with 750.0 cm3 of 0.100 mol dm–3 Ca(OH)2.
What is the OH– concentration, in mol dm–3, in the resulting mixture?
A 0.0250
B 0.100
C 0.150
D 0.175
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_06.webp)
![7 After delivering a solution from a pipette, a droplet remains in the tip of the pipette.
How should a student ensure that the pipette delivers the volume of solution stated on the
pipette?
A Fill the pipette just above the graduation line to compensate for the volume of the droplet
that remains in the tip.
B Leave the droplet in the tip.
C Shake the pipette to force out the droplet left in the tip.
D Use a pipette filler to force the droplet out of the tip.
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_07.webp)
![8 Which sequence has elements in order of increasing first ionisation energy?
A Na < Mg < Al
B Mg < Al < Si
C Al < Si < P
D Si < P < S
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_08.webp)
![9 Which element has atoms with the largest number of unpaired p-electrons?
A aluminium
B oxygen
C chlorine
D phosphorus
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_09.webp)
![10 The equation for the complete combustion of propene, C3H6, is shown below.
C3H6(g) + 4½O2(g) → 3CO2(g) + 3H2O(l)
Standard enthalpy changes of formation, ∆f H o, are shown in the table.
Compound ∆f H o / kJ mol–1
C3H6(g) +20
O2(g) 0
CO2(g) –394
H2O(l) –286
What is the standard enthalpy change of combustion of C3H6(g), in kJ mol–1?
A –2060
B –700
C +700
D +2060
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_10.webp)
![11 The Boltzmann distributions below show a gas at two different temperatures.
Which Boltzmann distribution shows the dotted curve at a higher temperature?
number of
A molecules
energy
number of
B molecules
energy
number of
C molecules
energy
number of
D molecules
energy
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_11.webp)
![12 Which statement about dynamic equilibrium is not correct?
A A catalyst increases the rate of both forward and reverse reactions by the same amount.
B Dynamic equilibrium exists only in a closed system.
C The concentrations of the reactants and products are equal.
D The rate of the forward reaction is equal to the rate of the reverse reaction.
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_12.webp)
![13 What is the number of unsaturated isomers (structural and stereoisomers) that have the molecular
formula C4H8?
A 3
B 4
C 5
D 6
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_13.webp)
![14 What do curly arrows always show in reaction mechanisms?
A Movement of one electron.
B Movement of a pair of electrons.
C Movement of a lone pair of electrons.
D Movement of the electrons in a covalent bond.
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_14.webp)
![15 Which structural isomer of C7H16 has the weakest induced dipole–dipole interactions (London
forces)?
A 2,3-dimethylpentane
B 3-ethylpentane
C 2-methylhexane
D 2,2,3-trimethylbutane
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_15.webp)
![16 Which compound contains the smallest bond angle?
A bromoethane
B ethanol
C ethane
D ethene
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_16.webp)
![17 What is the systematic name of the compound below?
OH
A 3-methylhex-5-en-4-ol
B 4-methylhex-1-en-3-ol
C 2-ethylpent-4-en-3-ol
D 4-ethylpent-1-en-3-ol
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_17.webp)
![18 The ‘dienes’ are a homologous series of non-cyclic compounds with two double bonds.
The simplest diene is shown below.
What is the general formula of the dienes homologous series?
A CnH2n+2
B CnH2n
C CnH2n–2
D CnH2n–4
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_18.webp)
![19 Which statement about absorption of radiation is correct?
A Absorption of IR radiation can break covalent bonds, forming radicals.
B Absorption of IR radiation causes covalent bonds to vibrate more.
C Absorption of UV radiation is a major cause of global warming and climate change.
D Absorption of UV radiation is used in modern breathalysers to measure ethanol in the
breath.
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_19.webp)
![20 The repeat unit of an addition polymer is shown below.
H CH2OH
C C
H H
What is the monomer?
OH
A
B
OH
OH
C
D
OH
Your answer [1]](/img/NOV21_H0321/NOV21_H0321_20.webp)
![1 Which statement describes electronegativity?
A A measure of the reactivity of an element.
B The ability of an atom to attract an electron to become a 1– ion.
C The attraction of a bonded atom for the electrons in a covalent bond.
D The attraction of an atom for a lone pair of electrons.
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_01.webp)
![2 A chlorate(VII) ion has a 1– charge.
What is the formula for sodium chlorate(VII)?
A NaCl O3
B NaCl O4
C NaCl O7
D NaCl O8
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_02.webp)
![3 The unbalanced equation for the reaction of silver with concentrated nitric acid is shown below.
….. Ag(s) + ….. NO3 –(aq) + ….. H+(aq) → ….. Ag+(aq) + .…. NO(g) + ..… H2O(l)
Which numbers for Ag and H2O will balance the equation?
Ag(s) H2O(l)
A 1 2
B 2 3
C 3 1
D 3 2
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_03.webp)
![4 Which sample contains the greatest number of molecules?
A 140.0 g C2H2
B 180.0 g C2H6
C 240.0 g C4H10
D 400.0 g C6H6
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_04.webp)
![5 Chromium(III) oxide, Cr2O3, is reduced to chromium by heating with magnesium.
What is the minimum mass of Mg required to reduce 11.4 g of chromium(III) oxide?
A 0.61 g
B 0.91 g
C 3.65 g
D 5.47 g
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_05.webp)
![6 A student is supplied with 100.0 cm3 of a solution of 0.400 mol dm–3 magnesium iodide, MgI2.
A student plans to dilute this solution so that the iodide concentration is 0.250 mol dm–3.
What volume of water, in cm3, does the student need to add?
A 60.0
B 160.0
C 220.0
D 320.0
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_06.webp)
![7 Which row shows elements in order of increasing first ionisation energy?
A Ca < Si < P < N
B N < P < Si < Ca
C Ca < N < P <Si
D C < Si < P < Ca
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_07.webp)
![8 Bond enthalpies are given in the table.
Bond H–S O=O S=O O–H
Bond enthalpy
+346 +498 +531 +464
/ kJ mol–1
What is the enthalpy change, in kJ mol–1, for the reaction below?
2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g)
A –174
B –1102
C –1794
D –2098
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_08.webp)
![9 An equilibrium system is shown below.
CO(g) + NO2(g) CO2(g) + NO(g)
Different amounts of CO, NO2, CO2 and NO are added to four containers, as shown below.
Container CO / mol NO2 / mol CO2 / mol NO / mol
A 1 1 0 0
B 1 0 1 1
C 1 1 1 0
D 0 1 1 1
Which container would have the largest concentration of CO(g) at equilibrium?
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_09.webp)
![10 An aqueous solution of ethanoic acid, CH3COOH, has a concentration of 0.50 mol dm–3.
pKa for CH3COOH = 4.76 at 25 °C.
What is the pH of the ethanoic acid solution at 25 °C?
A 2.53
B 2.68
C 4.91
D 5.06
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_10.webp)
![11 The feasibility of a chemical reaction depends on the temperature and the signs of ΔH and ΔS.
Which row has signs for ΔH and ΔS for a reaction that is feasible at high temperatures but is not
feasible at low temperatures?
ΔH ΔS
A + +
B + –
C – +
D – –
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_11.webp)
![12 Two redox systems are shown below.
Fe2+(aq) + 2e– Fe(s) E o– = –0.44 V
Cu2+(aq) + 2e– Cu(s) E o– = +0.34 V
Which species in the two redox systems is the strongest oxidising agent?
A Fe2+(aq)
B Fe(s)
C Cu2+(aq)
D Cu(s)
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_12.webp)
![13 Which statement(s) explain(s) the trend in boiling points down the halogens group?
1: The induced dipole–dipole interactions (London forces) become stronger.
2: The covalent bonds become stronger.
3: The permanent dipole–dipole interactions become stronger.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_13.webp)
![14 Which statement(s) about a molecule of Cl–N=O is/are correct?
1: It is a polar molecule.
2: It contains 6 lone pairs of electrons.
3: It has a bond angle of 180°.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_14.webp)
![15 NH4Fe(SO4)2•12H2O is a hydrated ‘double salt’.
A student analyses this double salt using test tube tests.
Which row(s) gives/give correct result(s) for the stated test?
Test Results
1 Reaction with cold NaOH(aq) Green precipitate
2 Reaction with Ba(NO3)2(aq) White precipitate
3 Reaction with warm NaOH(aq) Red-brown precipitate and an alkaline gas
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/NOV21_H4321/NOV21_H4321_15.webp)
![1 2-Methylbutane is reacted with chlorine by radical substitution.
What is the number of structural isomers with the molecular formula C5H11Cl that could be
formed?
A 2
B 3
C 4
D 5
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_01.webp)
![2 Which type(s) of stereoisomerism is/are shown by 2,4-dimethylhex-2-ene?
A E / Z isomerism only.
B Optical isomerism only.
C Both E / Z isomerism and optical isomerism.
D Neither E / Z isomerism nor optical isomerism.
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_02.webp)
![3 Which sample contains the greatest number of carbon atoms?
A 20.0 g C6H5OH
B 30.0 g C2H5COOH
C 40.0 g CH3CHO
D 50.0 g CH3OH
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_03.webp)
![4 What is the correct equation for the incomplete combustion of butan-1-ol?
A CH3CH2CH2CH2OH + 1½O2 4CO + 5H2
B CH3CH2CH2CH2OH + 2O2 4CO + 5H2
C CH3CH2CH2CH2OH + 4O2 4CO + 5H2O
D CH3CH2CH2CH2OH + 4½O2 4CO + 5H2O
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_04.webp)
![5 2-Methylcyclopentanone, shown below, is reacted with NaCN(aq)/H+(aq) to form an organic
product.
O
CH3
2-methylcyclopentanone
Which statement is correct?
A In the mechanism, a CN– ion accepts an electron pair.
B The mechanism is electrophilic addition.
C The organic product has one chiral centre.
D The organic product has the molecular formula C7H11NO.
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_05.webp)
![6 CH3CH2COOCH3 is heated with aqueous sodium hydroxide to produce two organic products.
What are the two organic products?
A CH3CH2COOH and CH3OH
B CH3CH2COONa and CH3OH
C CH3CH2COOH and CH3ONa
D CH3CH2COONa and CH3ONa
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_06.webp)
![7 Menthol, shown below, is heated with an acid catalyst.
OH
menthol
Which structure could be formed?
A B C D
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_07.webp)
![8 Which compound contains a bond angle of approximately 120º?
A CH3CH2CN
B CH3CH(OH)CH3
C CH3COOCH2CH2CH3
D CH3CH2CH2NH2
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_08.webp)
![9 Which reaction is not a reduction?
A C6H5NO2 C6H5NH2
B CH3CN CH3CH2NH2
C CH3CH2Cl CH3CH2NH2
D CH3COCH3 CH3CHOHCH3
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_09.webp)
![10 A TLC chromatogram for two compounds is shown below.
solvent front
origin
What is the Rf value for the compound that is most strongly adsorbed onto the stationary phase?
A 0.25
B 0.33
C 0.69
D 0.78
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_10.webp)
![11 Which compound could have produced the IR spectrum below?
100
transmittance (%) 50
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
A (CH3)2CHCHO
B (CH3)2CHCOOH
C CH3CH(OH)CH=CH2
D CH3COCH(OH)CH3
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_11.webp)
![12 Which peak would be in the mass spectrum of propanal, CH3CH2CHO, but not in the mass
spectrum of propanone, CH3COCH3?
A m /z = 15
B m /z = 29
C m /z = 43
D m /z = 58
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_12.webp)
![13 Which compound(s) has/have four peaks in a 13C NMR spectrum?
O
1
2
O
3
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_13.webp)
![14 Which of the following statement(s) provide(s) evidence for the delocalised model of benzene
rather than the Kekulé model?
1 The enthalpy change of hydrogenation is more exothermic than expected.
2 Benzene only reacts with bromine in the presence of a halogen carrier.
3 The carbon-carbon bonds all have the same length.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_14.webp)
![15 Compounds 1, 2 and 3 are heated with NaOH(aq).
Which compound(s) react(s)?
OH
1
COOH
2
CH2Br
3
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/NOV21_H4322/NOV21_H4322_15.webp)
![1 Which substance contains polar molecules?
A C2H4
B CO2
C NCl 3
D SF6
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_01.webp)
![2 What is the formula of silver carbonate?
A AgCO3
B Ag(CO3)2
C Ag2CO3
D Ag3CO3
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_02.webp)
![3 Which statement explains why ice is less dense than water?
A Hydrogen bonds are stronger in ice than in water.
B Hydrogen bonds hold H2O molecules apart in ice.
C Ice is a solid but water is a liquid.
D Ice contains hydrogen bonds, but water does not contain hydrogen bonds.
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_03.webp)
![4 Some Group 2 compounds can be used to neutralise acid soils and to treat acid indigestion.
Which Group 2 compound would not be suitable for either use?
A BaSO4
B CaCO3
C Ca(OH)2
D Mg(OH)2
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_04.webp)
![5 Which p-block element contains atoms with one unpaired electron?
A Al
B Si
C P
D S
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_05.webp)
![6 The equation for a redox reaction is shown below.
2HCl O3 + 2HCl → 2Cl O2 + Cl 2 + 2H2O
Which statement is correct?
A Cl is both oxidised and reduced.
B Cl is oxidised and O is reduced.
C O is both oxidised and reduced.
D O is oxidised and Cl is reduced.
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_06.webp)
![7 Potassium ferrate(VI) contains two potassium ions for every ferrate(VI) ion.
What is the formula of the ferrate(VI) ion?
A FeO3 2−
B FeO4 2−
C FeO5 2−
D FeO6 2−
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_07.webp)
![8 The unbalanced equation for the reaction of copper with concentrated nitric acid is shown below.
.........Cu + .........HNO3 → .........Cu(NO3)2 + .........NO2 + .........H2O
What is the number of moles of HNO3 that react with 1 mole of Cu?
A 2
B 3
C 4
D 6
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_08.webp)
![9 2.0 dm3 of Cl 2 gas reacts with 2.0 dm3 of Cl F3 gas to form 6.0 dm3 of a gaseous compound.
The reaction has 100% atom economy and all volumes are measured at the same temperature
and pressure.
What is the molecular formula of the compound formed?
A Cl F
B Cl 2F3
C Cl 3F2
D Cl 3F3
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_09.webp)
![10 Which sample contains the greatest number of molecules?
A 1 g of methanol, CH3OH
B 2 g of nitrogen dioxide, NO2
C 3 g of phosphorus, P4
D 4 g of iodine, I2
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_10.webp)
![11 Hydrogen and oxygen react as shown below.
2H2(g) + O2(g) → 2H2O(g) ∆rH = −486 kJ mol−1
Bond enthalpies are shown in the table.
Bond H−H O=O
Bond enthalpy
+436 +498
/ kJ mol−1
What is the bond enthalpy, in kJ mol−1, for the O−H bond?
A +221
B +355
C +464
D +928
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_11.webp)
![12 Hydrogen gas can be produced as shown below.
CH4(g) + H2O(g) CO(g) + 3H2(g) ∆H = +206 kJ mol−1
Which conditions produce the greatest equilibrium yield of hydrogen?
A Low temperature and high pressure
B Low temperature and low pressure
C High temperature and high pressure
D High temperature and low pressure
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_12.webp)
![13 The reversible reaction below is in equilibrium.
2SO2(g) + O2(g) 2SO3(g)
The equilibrium concentrations are shown in the table.
Substance SO2(g) O2(g) SO3(g)
Equilibrium concentration
4.00 2.40 1.44
/ mol dm−3
What is the numerical value of Kc?
A 0.0375
B 0.0540
C 0.150
D 18.5
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_13.webp)
![14 Which statement is correct for the two structures below?
A They have the same empirical formula.
B They have different relative molecular masses.
C They are structural isomers.
D They have different functional groups.
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_14.webp)
![15 Which property explains the low reactivity of alkanes?
A Electron pair repulsion between σ-bonds
B Free rotation about σ-bonds
C High C–C bond enthalpy
D High polarity of the C–H bonds
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_15.webp)
![16 What are the correct reagents for the conversion below?
CH3CH2CHOHCH3 → CH3CH2CHBrCH3
A Br2 and H2SO4
B Br2 and NaOH
C NaBr and H2SO4
D NaBr and NaOH
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_16.webp)
![17 Which compound could react with both
• K2Cr2O7/H2SO4 in an oxidation reaction and
• an acid catalyst (e.g. H2SO4) in an elimination reaction?
A
OH
B
OH
C
HO
D
HO OH
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_17.webp)
![18 A student reacts 24.24 g of 2-bromobutane in the reaction below.
CH3CH2CHBrCH3 + NaOH → CH3CH2CHOHCH3 + NaBr
Mr = 136.9 Mr = 74.0
The reaction produces 4.81 g of CH3CH2CHOHCH3.
What is the percentage yield of CH3CH2CHOHCH3?
A 10.7%
B 19.8%
C 36.7%
D 54.1%
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_18.webp)
![19 Which row describes a nucleophile?
A electron pair donor attracted to high electron density
B electron pair donor attracted to low electron density
C electron pair acceptor attracted to high electron density
D electron pair acceptor attracted to low electron density
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_19.webp)
![20 The mass spectrum of a carboxylic acid contains peaks at m /z = 29 and m /z = 102.
Which compound could have produced the spectrum?
O
A
OH
OH
B
O
OH
C
O
OH
D
O
Your answer [1]](/img/NOV20_H0321/NOV20_H0321_20.webp)
![1 Several students titrate 25.00 cm3 of the same solution of sodium hydroxide, NaOH(aq) with
hydrochloric acid, HCl (aq).
One student obtains a smaller titre than the other students.
Which procedure explains the smaller titre?
A The burette readings are taken from the top of the meniscus instead of the bottom of the
meniscus.
B The conical flask is rinsed with water before carrying out the titration.
C An air bubble is released from the jet of the burette during the titration.
D The pipette is rinsed with water before filling with NaOH(aq).
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_01.webp)
![2 Which statement gives the numerical value of the Avogadro constant?
A The number of moles in 12 g of carbon-12.
B The number of electrons lost by 20.05 g of calcium when it reacts with oxygen.
C The number of molecules in 16.0 g of oxygen.
D The number of atoms in 1 mole of chlorine molecules.
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_02.webp)
![3 0.80 g of element X is reacted with 0.40 g of O2 to form an oxide with the formula X2O3.
What is the identity of element X?
A Aluminium
B Titanium
C Germanium
D Molybdenum
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_03.webp)
![4 Phosphoric acid is a tribasic acid.
What is the mass of Ca(OH)2 that completely neutralises 100 cm3 of 0.100 mol dm−3 phosphoric
acid?
A 0.49 g
B 0.74 g
C 1.11 g
D 2.22 g
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_04.webp)
![5 Which statement about elements in the d block of Period 4 of the periodic table is correct?
A Cr atoms have the electron configuration: 1s22s22p63s23p63d54s1.
B Cu+ ions contain an incomplete 3d sub-shell.
C Fe2+ ions contain 3 unpaired electrons.
D Sc forms ions with different oxidation states.
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_05.webp)
![6 The equation for the combustion of C7H8 is shown in the following equation.
C7H8(l) + 9O2(g) 7CO2(g) + 4H2O(l)
Enthalpy changes of formation are shown in the table.
Substance C7H8(l) CO2(g) H2O(l)
∆f H / kJ mol−1 +12 −394 −286
Calculate the enthalpy of combustion, in kJ mol−1, for the hydrocarbon C7H8.
A −3914
B −692
C +692
D +3914
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_06.webp)
![7 The diagram represents a Boltzmann distribution curve of molecules at a given temperature.
number of
molecules
energy
Which statement for this Boltzmann distribution curve is correct at a higher temperature?
A The peak increases in height and moves to the left.
B The peak increases in height and moves to the right.
C The peak decreases in height and moves to the left.
D The peak decreases in height and moves to the right.
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_07.webp)
![8 A graph is plotted of ln(k) against 1 /T.
(k = rate constant, T = temperature in K)
The gradient has the numerical value of −55 000.
What is the activation energy, in kJ mol−1?
A +1.5 × 10−7
B +2.22 × 10−6
C +6.62
D +457
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_08.webp)
![9 The reversible reaction of nitrogen and hydrogen to form ammonia is shown below.
N2(g) + 3H2(g) 2NH3(g)
In the equilibrium mixture, the partial pressure of N2 is 18.75 MPa and the partial pressure of H2 is
2.50 MPa.
The total pressure is 25 MPa.
What is the value of Kp, in MPa−2?
A 1.2 × 10−4
B 0.048
C 0.075
D 21
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_09.webp)
![10 The equation for the reaction of ICl and H2 is shown below.
2ICl (g) + H2(g) 2HCl (g) + I2(g)
The rate constant k for this reaction is 1.63 × 10−6 dm3 mol−1 s−1.
What is the overall order of the reaction?
A 0
B 1
C 2
D 3
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_10.webp)
![11 20 cm3 of 0.10 mol dm−3 hydrochloric acid is added to 10 cm3 of 0.10 mol dm−3 sodium hydroxide.
What is the pH of the resulting mixture?
A 1.00
B 1.18
C 1.30
D 1.48
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_11.webp)
![12 Iodide ions, I−(aq), react with MnO4 −(aq). The unbalanced equation is shown below.
I−(aq) + MnO4 −(aq) + H2O(l) IO−(aq) + MnO2(s) + OH−(aq)
What is the ratio of MnO2(s) to OH−(aq) in the balanced equation?
A 1 : 3
B 1 : 2
C 1 : 1
D 3 : 2
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_12.webp)
![13 Which statement(s) is/are correct when a catalyst is added to a system in dynamic equilibrium?
1 The rates of the forward and reverse reactions increase by the same amount.
2 The concentrations of the reactants and products do not change.
3 The value of Kc increases.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_13.webp)
![14 Which statement(s) for Group 2 elements is/are correct?
1 The 2nd ionisation energy of magnesium is greater than the 2nd ionisation energy of
calcium.
2 A strontium ion, Sr2+, contains a total of 6 electrons in s orbitals.
3 The equation for the reaction of barium with water is:
2Ba + 2H2O 2BaOH + H2.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_14.webp)
![15 Which statement(s) for the complex ion [Co(NH2CH2CH2NH2)3]2+ is/are correct?
1 It has cis and trans isomers.
2 It has optical isomers.
3 It is six-fold coordination.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/NOV20_H4321/NOV20_H4321_15.webp)
![1 What is the name of the compound below?
H3C CH2CH3
C C
H Br
A E-3-bromopent-2-ene
B E-3-bromopent-3-ene
C Z-3-bromopent-2-ene
D Z-3-bromopent-3-ene
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_01.webp)
![2 Which statement about bonds is correct?
A The C=C bond in ethene is more polar than the C−C bond in ethane.
B A σ-bond is stronger than a π-bond.
C The H−C−H bond angle in ethane is greater than the H−C−H bond angle in ethene.
D A σ-bond is formed from sideways overlap of p orbitals.
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_02.webp)
![3 Which of these reagent(s) will not react with HOCH2CH2CH2COOH?
A NaCN in ethanol
B C2H5OH in the presence of an acid catalyst
C (CH3CO)2O
D concentrated H2SO4
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_03.webp)
![4 Which compound can be refluxed with acidified potassium dichromate(VI) to form an organic
product with molecular formula C5H8O2?
A
HO O
B
HO O
O
HO
C
O
D HO
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_04.webp)
![5 Which structure shows a section of poly(propene)?
A
B
C
D
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_05.webp)
![6 Which alcohol reacts with an acid catalyst to form a mixture of stereoisomers?
A 3-methylbutan-2-ol
B pentan-1-ol
C 2-methylhexan-2-ol
D heptan-4-ol
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_06.webp)
![7 Which one of the following reacts with ethanoic acid and with phenol?
A Aqueous potassium hydroxide
B Bromine
C Calcium carbonate
D Methanol and an acid catalyst
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_07.webp)
![8 Which isomer of C6H12O2 produces the smallest number of peaks in its 13C NMR spectrum?
O
A
OH
O
B
O
O
C
OH
O
D
OH
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_08.webp)
![9 What is the structural formula of ethyl 3-methylbutanoate?
A CH3CH2COOCH2CH2CH(CH3)2
B CH3CH2COOCH(CH3)CH2CH3
C CH3CH2CH(CH3)COOCH2CH3
D (CH3)2CHCH2COOCH2CH3
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_09.webp)
![10 What is the number of alicyclic structural isomers of C5H10?
A 3
B 4
C 5
D 6
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_10.webp)
![11 Complete combustion of 1.00 g of a hydrocarbon gives 3.38 g carbon dioxide.
What is the empirical formula of the hydrocarbon?
A CH
B CH2
C C2H5
D C3H8
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_11.webp)
![12 What is the molecular formula of the steroid molecule below?
OH
HO
A C18H24O2
B C18H26O2
C C18H28O2
D C18H30O2
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_12.webp)
![13 Which statement(s) is/are correct for gas chromatography?
1 The components in a mixture can be identified from their retention time.
2 The relative peak areas give the proportions of components in a mixture.
3 Calibration curves are used to confirm the concentrations of components in a mixture.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_13.webp)
![14 Which of the following reactions produce propan-1-ol?
1 The alkaline hydrolysis of 1-chloropropane.
2 The acid hydrolysis of propyl methanoate.
3 The acid hydrolysis of propanenitrile.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_14.webp)
![15 Which compound(s) could be prepared by reacting benzene with an acyl chloride in the presence
of a halogen carrier?
CH2COCH3
1
CHO
2
COCH3
3
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/NOV20_H4322/NOV20_H4322_15.webp)
![1 Which statement about the periodic table is not correct?
A The elements are arranged in groups with similar chemical properties.
B The elements are arranged in periods with repeating trends in properties.
C The elements are arranged in order of increasing atomic number.
D The elements in the halogen group increase in reactivity down the group.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_01.webp)
![2 Which molecule contains the largest bond angle?
A C2H4
B H2O
C NH3
D CH4
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_02.webp)
![3 What is the percentage composition by mass of nitrogen in (NH4)2CO3?
A 14.58%
B 17.95%
C 29.17%
D 37.50%
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_03.webp)
![4 Which chemical process is the most sustainable in terms of the atom economy of the organic
product?
A CO2 + 3H2 → CH3OH + H2O
B CH3CH2OH + NaCl + H2SO4 → CH3CH2Cl + NaHSO4 + H2O
C CH3CH2Br + NaOH → CH3CH2OH + NaBr
D CH3CH2CH2CH2OH → CH3CH2CH=CH2 + H2O
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_04.webp)
![5 8.0 dm3 of NO is mixed with 6.0 dm3 of O2 at room temperature and pressure (RTP).
The reaction below takes place until one of the reactants is used up.
2NO(g) + O2(g) → 2NO2(g)
What is the volume of the mixture at RTP after the reaction has taken place?
A 8.0 dm3
B 10.0 dm3
C 12.0 dm3
D 14.0 dm3
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_05.webp)
![6 What is the volume of 0.0100 mol of N2 at 350 °C and 200 kPa?
A 145 cm3
B 259 cm3
C 145 dm3
D 259 dm3
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_06.webp)
![7 0.24 g of an element, X, is reacted with 0.0100 mol Cl 2 to form a chloride with the formula XCl 2.
What is element X?
A carbon
B magnesium
C molybdenum
D titanium
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_07.webp)
![8 A phosphate(V) ion has the formula PO4 3−.
What is the formula for copper(I) phosphate(V)?
A Cu(PO4)5
B Cu5PO4
C Cu(PO4)3
D Cu3PO4
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_08.webp)
![9 Which reaction shows chlorine only being oxidised?
A Cl 2 + H2O → HCl + HCl O
B 2Cl O2 + 2NaOH → NaCl O2 + NaCl O3 + H2O
C 4KCl O3 → 3KCl O4 + KCl
D MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_09.webp)
![10 A reversible reaction has the enthalpy profile diagram shown below.
150
energy
reactants
/kJ mol–1
120
products
progress of reaction
Which statement about this reaction is correct?
A The activation energy of the forward reaction is 120 kJ mol−1.
B The activation energy of the reverse reaction is 270 kJ mol−1.
C The enthalpy change of the forward reaction is −30 kJ mol−1.
D The reverse reaction is exothermic.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_10.webp)
![11 Hydrogen and chlorine react as shown below.
H2(g) + Cl 2(g) → 2HCl (g) ∆H o = −184.6 kJ mol−1
Which statement about this reaction is correct?
A Less energy is released on bond making than is taken in during bond breaking.
B The enthalpy change for the reverse equation is +184.6 kJ mol−1.
C The enthalpy change of formation of HCl (g) is –184.6 kJ mol−1.
D The temperature decreases during the reaction.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_11.webp)
![12 What is the main reason for the increase in reaction rate with increasing temperature?
A The activation energy decreases.
B The activation energy increases.
C More molecules have an energy greater than the activation energy.
D The molecules collide more frequently.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_12.webp)
![13 A catalyst is added to a system in equilibrium.
What is the effect on the rates of the forward and reverse reactions?
A There is no effect on the rate in either direction.
B Both rates increase by the same factor.
C The rate in the forward direction increases by a greater factor than the reverse direction.
D The rate in the reverse direction increases by a greater factor than the forward direction.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_13.webp)
![14 What is the best description for the bonding between the carbon atoms in an ethene molecule?
A One σ-bond and one π-bond
B One π-bond
C Two σ-bonds
D Two π-bonds
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_14.webp)
![15 Which compound is unsaturated, alicyclic and contains an alkyl group?
A
B
C
D
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_15.webp)
![16 Which statement about an electrophile is correct?
A It is an electron pair acceptor.
B It is a proton donor.
C It is a negative ion.
D It is a species with an unpaired electron.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_16.webp)
![17 A section of a polymer is shown below.
CN CN CN
Which monomer could form this polymer?
A CH3CH(OH)CN
B HOCH2CH2CN
C H2C=CHCN
D NCCH=CHCN
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_17.webp)
![18 Which compound is not likely to have a fragment ion at m / z = 43 in its mass spectrum?
H H O
A H C C C
H H OH
H O
B H C C
H OH
H CH3 H
C H C C C OH
H H H
H H H
D H C C C OH
H H H
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_18.webp)
![19 Which statement about infrared radiation is not correct?
A The energy from IR radiation causes some covalent bonds to vibrate more.
B Absorption of IR radiation by some atmospheric gases is linked by some scientists to global
warming.
C IR radiation is used to monitor gases causing air pollution.
D The action of IR radiation on CFCs in the upper atmosphere leads to the formation of chlorine
radicals.
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_19.webp)
![20 An unknown compound produces the infrared spectrum below.
100
transmittance
50
(%)
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
Which compound could have produced the infrared spectrum?
O
A
OH
O
B
HO
OH
C
O
D
Your answer [1]](/img/JUN19_H0321/JUN19_H0321_20.webp)
![1 In the diagrams below, each box represents an orbital and each electron is shown as an arrow.
Which diagram shows the correct arrangement of electrons in an atom of carbon?
2p
2s
A energy
1s
2p
2s
B energy
1s
2p
2s
C energy
1s
2p
2s
D energy
1s
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_01.webp)
![2 Which statement about the reactions of halogens with halide ions is correct?
A I2(aq) can oxidise Br−(aq).
B Cl 2(aq) can reduce Br−(aq).
C Br−(aq) can reduce Cl 2(aq).
D Cl −(aq) can oxidise I2(aq).
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_02.webp)
![3 One molecule of a gas has a mass of 2.658 × 10−23 g.
What is a possible formula of the gas?
A CH4
B O2
C SO2
D SO3
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_03.webp)
![4 In the laboratory, acid spills can be cleaned up and made safe by spreading anhydrous sodium
carbonate over the spill to neutralise the acid.
A student accidentally spills 50.0 cm3 of 2.00 mol dm−3 HCl (aq) on the bench.
What is the minimum mass of anhydrous sodium carbonate required to neutralise the acid?
A 4.15 g
B 5.30 g
C 8.30 g
D 10.6 g
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_04.webp)
![5 What is the oxidation number of N in Mg(NO2)2•3H2O?
A +2
B +3
C +4
D +5
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_05.webp)
![6 Which reaction is a redox reaction?
A NaCl + AgNO3 AgCl + NaNO3
B NaNO2 + HCl NaCl + HNO2
C CaSO3 + 2HCl CaCl 2 + H2O + SO2
D 3CuO + 2NH3 3Cu + 3H2O + N2
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_06.webp)
![7 Which set of elements in the solid state contain a simple molecular lattice, a giant covalent lattice
and a giant metallic lattice?
A S, Si, Al
B P, Si, C
C S, P, Si
D Mg, P, S
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_07.webp)
![8 3.528 g of a Group 2 metal, M, is reacted with an excess of chlorine.
The reaction forms 9.775 g of a chloride.
What is metal M?
A magnesium
B calcium
C strontium
D barium
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_08.webp)
![9 Which statement is not correct for Group 2 hydroxides?
A Mg(OH)2 can be used to treat indigestion.
B Ca(OH)2 is used in agriculture to neutralise alkaline soils.
C The anion in Sr(OH)2 contains 10 electrons.
D Ba(OH)2 is a product from the reaction of barium and water.
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_09.webp)
![10 Radical reactions are responsible for the catalysed breakdown of the ozone layer.
The overall equation is shown below.
2O3 3O2 ∆rH = −284 kJ mol−1
The molar gas volume in the ozone layer is approximately 2.5 m3 mol−1.
What is the energy released, in kJ, during the breakdown of 1.0 m3 of ozone in the ozone layer?
A 56.8
B 113.6
C 355
D 710
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_10.webp)
![11 A graph of ln k against 1
T (T in K) for a reaction has a gradient with the numerical value of −4420.
What is the activation energy, in kJ mol−1, for this reaction?
A −532
B −36.7
C +36.7
D +5.32 × 105
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_11.webp)
![12 The equation shows the dissociation of the acid H3AsO4 in water.
H3AsO4 + H2O H2AsO4 – + H3O+
Which pair is a conjugate acid–base pair?
A H3AsO4 and H2O
B H2AsO4 − and H3O+
C H3AsO4 and H3O+
D H3O+ and H2O
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_12.webp)
![13 What is the number of stereoisomers that Ni(H2NCH2CH2NH2)2Cl 2 can form?
A 2
B 3
C 4
D 6
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_13.webp)
![14 Which property/properties is/are correct for a transition element?
1 The element has atoms with a partially filled d sub-shell.
2 The existence of more than one oxidation state in its compounds.
3 The formation of coloured ions.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_14.webp)
![15 Four redox systems relevant to hydrogen–oxygen fuel cells are shown below.
Eө / V
H2O(l) + e− OH−(aq) + ½H2(g) −0.83
H+(aq) + e− ½H2(g) 0.00
½O2(g) + H2O(l) + 2e− 2OH−(aq) +0.40
½O2(g) + 2H+(aq) + 2e− H2O(l) +1.23
Which statement(s) is/are correct for an alkaline hydrogen–oxygen fuel cell?
1 The reaction at the positive electrode is: ½O2(g) + 2H+(aq) + 2e− H2O(l).
2 The overall cell reaction is: H2(g) + ½O2(g) H2O(l).
3 The cell potential is 1.23 V.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN19_H4321/JUN19_H4321_15.webp)
![1 Which alkane has the highest boiling point?
A CH3(CH2)5CH3
B (CH3)3CCH(CH3)2
C CH3(CH2)3CH(CH3)2
D (CH3)2CHCH2CH(CH3)2
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_01.webp)
![2 Butane reacts with chlorine in the presence of ultraviolet radiation to form a mixture of organic
products.
Which equation shows a propagation step in the mechanism for this reaction?
A Cl 2 → •Cl + •Cl
B •Cl + •C4H8Cl → C4H8Cl 2
C C4H9Cl + •Cl → C4H8Cl 2 + •H
D •Cl + C4H9Cl → •C4H8Cl + HCl
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_02.webp)
![3 What is the name of the compound below?
H CH3
C
C
H3C CH2 CH2 CH2 CH3
A 3-Propylpent-2-ene
B 3-Propylpent-3-ene
C 3-Ethylhex-2-ene
D 4-Ethylhex-4-ene
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_03.webp)
![4 The structure of a stereoisomer is shown below.
H3C CH(CH3)2
C C
CH3CH2 CH2CH2CH3
Which term correctly describes this stereoisomer?
A cis-
B trans-
C E-
D Z-
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_04.webp)
![5 Which types of bonds are broken and formed in the reaction of ethene and bromine?
Types of bond broken Types of bond formed
A σ π
B π σ
C σ and π π
D σ and π σ
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_05.webp)
![6 What is the organic product of the reaction below?
CH2Cl
KOH(aq)
Cl
CH2OH
A
Cl
CH2Cl
B
OH
CH2OH
C
OH
HO CH2Cl
D
Cl
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_06.webp)
![7 What is the number of chiral carbon atoms in the steroid molecule below?
OH
O
A 5
B 6
C 7
D 8
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_07.webp)
![8 Phenol reacts with bromine.
Which is the least likely organic product?
OH
Br
A
Br
OH
Br Br
B
OH
Br
C
Br
OH
Br Br
D
Br
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_08.webp)
![9 The repeat unit of a polymer is shown below.
H H H H O
O C C O C C C C
H H O H H
Which monomers could form this polymer?
O
OH HO
A
HO OH
O
O
OH
HO OH
B
HO
O
O O
HO OH
C
HO OH
O O
D
HO
HO OH OH
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_09.webp)
![10 Which compound shows 4 peaks in its carbon-13 NMR spectrum?
A
B
C
D
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_10.webp)
![11 A student reacts 4.50 g of C6H5NH2 with excess CH3COCl in the reaction below.
C6H5NH2 + CH3COCl → C6H5NHCOCH3 + HCl
Mr = 93.0 Mr = 135.0
The reaction produces 3.25 g of C6H5NHCOCH3.
What is the percentage yield of C6H5NHCOCH3?
A 49.8
B 68.9
C 72.2
D 95.4
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_11.webp)
![12 A compound produces the 13C NMR spectrum below.
80 70 60 50 40 30 20 10 0
chemical shift, d / ppm
Which compound could have produced this spectrum?
A Propane
B 2-Methylbutane
C 2-Methylpropan-1-ol
D 2-Methylpropan-2-ol
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_12.webp)
![13 A carbonyl compound is reacted with NaBH4.
Which compound(s) could be formed?
1 2-Methylpentan-2-ol
2 2-Methylpentan-1-ol
3 3-Methylpentan-2-ol
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_13.webp)
![14 Which chemical(s) can react with phenol?
1 Potassium hydroxide
2 Ethanoyl chloride
3 Nitric acid
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_14.webp)
![15 The structure of a compound used to treat influenza is shown below.
O
O
O
HN
NH2
O
Which functional group(s) is/are in a molecule of the compound?
1 Ester
2 Secondary amide
3 Ketone
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN19_H4322/JUN19_H4322_15.webp)
![1 The electron configuration of element X is: 1s22s22p63s23p4
What is the formula of a compound formed when sodium reacts with element X?
A NaX
B NaX2
C Na2X
D Na2X3
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_01.webp)
![2 What is the number of oxygen atoms in 88.0 g of CO2?
A 3.01 × 1023
B 1.20 × 1024
C 2.41 × 1024
D 4.82 × 1024
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_02.webp)
![3 A compound has the composition by mass:
H, 5.00%; N, 35.00%; O, 60.00%.
Which compound has this composition?
A HNO3
B NH4NO3
C HNO2
D NH2OH
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_03.webp)
![4 Sodium reacts with water as shown below.
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
Which mass of sodium reacts with water to produce 960 cm3 of hydrogen gas at RTP?
A 0.46 g
B 0.92 g
C 1.84 g
D 3.68 g
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_04.webp)
![5 Which equation does not represent a neutralisation reaction?
A Zn + 2HCl → ZnCl 2 + H2
B 2NH3 + H2SO4 → (NH4)2SO4
C Na2CO3 + 2CH3COOH → 2CH3COONa + CO2 + H2O
D CuO + 2HNO3 → Cu(NO3)2 + H2O
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_05.webp)
![6 What is the oxidation number of Fe in K2FeO4?
A +4
B +5
C +6
D +7
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_06.webp)
![7 Which reaction shows oxidation of sulfur?
A 2HBr + H2SO4 → SO2 + 2H2O + Br2
B SO2 + 2NaOH → Na2SO3 + H2O
C 8HI + H2SO4 → 4I2 + H2S + 4H2O
D H2S + Cl 2 → 2HCl + S
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_07.webp)
![8 What determines the order of elements in the Periodic Table?
A first ionisation energy
B number of electrons in the outer shell
C number of protons in the nucleus
D relative atomic mass
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_08.webp)
![9 The first five successive ionisation energies of an element Y are shown below.
1st 2nd 3rd 4th 5th
496 4563 6913 9544 13352
What is the formula of a chloride of Y?
A YCl
B YCl 2
C YCl 3
D YCl 4
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_09.webp)
![10 Which element has induced dipole–dipole interactions (London forces) in its solid lattice?
A boron
B magnesium
C silicon
D sulfur
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_10.webp)
![11 The equation for the reaction of aluminium sulfide, Al 2S3, with oxygen is shown below.
2Al 2S3(s) + 9O2(g) → 2Al 2O3(s) + 6SO2(g)
The table shows standard enthalpy changes of formation, ∆f H o.
Substance Al 2S3(s) O2(g) Al 2O3(s) SO2(g)
∆f H o / kJ mol−1 −723.8 0 −1675.7 −296.8
What is the standard enthalpy change of combustion of Al 2S3(s), in kJ mol−1?
A −3684.6
B −1842.3
C +1842.3
D +3684.6
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_11.webp)
![12 A student carried out an experiment to measure the enthalpy change of combustion of methanol.
The energy from the combustion of methanol was used to heat a beaker containing water.
The student’s calculated enthalpy change of combustion was more exothermic than the value in
data books.
Which error could have caused this difference?
A Some methanol had evaporated from the wick before the final weighing.
B In the calculation, the student used the molar mass of ethanol instead of methanol.
C There was incomplete combustion.
D The water boiled for 5 minutes before the final temperature was taken.
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_12.webp)
![13 The reversible reaction below is at equilibrium.
2SO2(g) + O2(g) 2SO3(g) ∆H = −197 kJ mol−1
Which changes in pressure and temperature would shift the equilibrium position towards the
products?
Pressure Temperature
A Decrease Decrease
B Decrease Increase
C Increase Decrease
D Increase Increase
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_13.webp)
![14 The reversible reaction below is at equilibrium.
N2(g) + 3H2(g) 2NH3(g)
What is the expression for Kc?
[N2(g)] [H2(g)]3
A
[NH3(g)]2
[NH3(g)]2
B [N2(g)] [H2(g)]3
[N2(g)] + 3[H2(g)]
C
2[NH3(g)]
2[NH3(g)]
D
[N2(g)] + 3[H2(g)]
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_14.webp)
![15 1 mol of a compound reacts with 8 mol O2 for complete combustion.
What is the formula of the compound?
A C4H8
B C4H9OH
C C5H11OH
D C5H12
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_15.webp)
![16 How many structural isomers of C6H14O are tertiary alcohols?
A 1
B 2
C 3
D 4
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_16.webp)
![17 The structure of naphthalene is shown below.
What is the molecular formula of naphthalene?
A C10H8
B C10H10
C C12H10
D C12H12
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_17.webp)
![18 A student reacts pent-2-ene with bromine in the laboratory.
Which compound is formed?
A 1,1-dibromopentane
B 1,2-dibromopentane
C 2,2-dibromopentane
D 2,3-dibromopentane
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_18.webp)
![19 The molecule below has two double bonds, labelled 1 and 2.
1 2
The arrangement around each double bond can be identified as E or Z.
Which row in the table is correct for double bond 1 and double bond 2?
Double bond 1 Double bond 2
A E Z
B Z E
C E E
D Z Z
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_19.webp)
![20 Which alcohol is likely to have a fragment ion at m / z = 31 in its mass spectrum?
A CH3CH2CH(OH)CH3
B CH3CH2CH2C(OH)(CH3)2
C CH3CH(OH)CH2CH2CH3
D (CH3)2CHCH2OH
Your answer [1]](/img/JUN18_H0321/JUN18_H0321_20.webp)
![1 A sample of boron contains the isotopes 10B and 11B.
The relative atomic mass of the boron sample is 10.8.
What is the percentage of 11B atoms in the sample of boron?
A 8.0%
B 20%
C 80%
D 92%
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_01.webp)
![2 In the compound [ICl2]+ [SbCl6]–, the oxidation number of chlorine is –1.
What are the oxidation numbers of I and Sb in the compound?
I Sb
A +1 +5
B +1 +7
C +3 +5
D +3 +7
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_02.webp)
![3 What is the number of hydrogen atoms in 0.125 mol of C2H5OH?
A 7.525 × 1022
B 4.515 × 1023
C 3.7625 × 1023
D 3.612 × 1024
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_03.webp)
![4 A student titrates a standard solution of barium hydroxide, Ba(OH)2, with nitric acid, HNO3.
25.00 cm3 of 0.0450 mol dm–3 Ba(OH)2 are needed to neutralise 23.35 cm3 of HNO3(aq).
What is the concentration, in mol dm–3, of the nitric acid?
A 0.0241
B 0.0482
C 0.0900
D 0.0964
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_04.webp)
![5 Which statement best explains why nitrogen has a larger first ionisation energy than oxygen?
A N atoms have less repulsion between p-orbital electrons than O atoms.
B N atoms have a smaller nuclear charge than O atoms.
C N atoms lose an electron from the 2s subshell, while O atoms lose an electron from the 2p
subshell.
D N atoms have an odd number of electrons, while O atoms have an even number.
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_05.webp)
![6 In the Periodic Table, element X is in Group 2 and element Y is in Group 15 (5).
What is the likely formula of an ionic compound of X and Y?
A X2Y5
B X2Y3
C X3Y2
D X5Y2
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_06.webp)
![7 Which statement about ammonium carbonate is not correct?
A It reacts with Ba(NO3)2(aq) to form a white precipitate.
B It effervesces with dilute nitric acid.
C It release an alkaline gas with warm NaOH(aq).
D It has the formula NH4CO3.
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_07.webp)
![8 A reaction is first order with respect to a reactant X.
Which rate–concentration graph for reactant X is the correct shape?
A
B
C
D
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_08.webp)
![9 The reversible reaction of sulfur dioxide and oxygen to form sulfur trioxide is shown below.
2SO2(g) + O2(g) 2SO3(g)
An equilibrium mixture contains 2.4 mol SO2, 1.2 mol O2 and 0.4 mol SO3.
The total pressure is 250 atm.
What is the partial pressure of SO3?
A 15 atm
B 25 atm
C 100 atm
D 200 atm
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_09.webp)
![10 A buffer solution is prepared by mixing 200 cm3 of 2.00 mol dm–3 propanoic acid, CH3CH2COOH,
with 600 cm3 of 1.00 mol dm–3 sodium propanoate, CH3CH2COONa.
Ka for CH3CH2COOH = 1.32 × 10–5 mol dm–3
What is the pH of the buffer solution?
A 4.58
B 4.70
C 5.06
D 5.18
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_10.webp)
![11 The table below shows standard entropies, Sө.
Substance CO(g) H2(g) CH3OH(l)
Sө / J mol–1 K–1 197.6 130.6 239.7
What is the entropy change, ∆Sө, in J mol–1 K–1, for the following reaction?
CO(g) + 2H2(g) CH3OH(l)
A –219.1
B –88.5
C +88.5
D +219.1
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_11.webp)
![12 The redox equilibria for a hydrogen–oxygen fuel cell in alkaline solution are shown below.
2H2O(l) + 2e– H2(g) + 2OH–(aq) Eө = –0.83 V
1/2O2(g) + H2O(l) + 2e– 2OH–(aq) Eө = +0.40 V
What is the equation for the overall cell reaction?
A H2(g) + 4OH–(aq) 3H2O(l) + 1/2O2(g)
B 3H2O(l) + 1/2O2 H2(g) + 4OH–(aq)
C H2O(l) H2(g) + 1/2O2(g)
D H2(g) + 1/2O2(g) H2O(l)
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_12.webp)
![13 Which enthalpy change(s) is/are endothermic?
1 The bond enthalpy of the C–H bond
2 The second electron affinity of oxygen
3 The standard enthalpy change of formation of magnesium
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_13.webp)
![14 Which statement(s) explain(s) why reaction rates increase as temperature increases?
1 The activation energy is less.
2 Collisions between molecules are more frequent.
3 A greater proportion of molecules have energy greater than the activation energy.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_14.webp)
![15 Which statement(s) is/are correct for the complex Pt(NH3)2Cl2?
1 One of its stereoisomers is used as an anti-cancer drug.
2 It has bond angles of 109.5°.
3 It has optical isomers.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN18_H4321/JUN18_H4321_15.webp)
![1 Which compound is used as a standard for NMR chemical shift measurements?
A Si(CH3)4
B CDCl 3
C D2O
D CCl 4
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_01.webp)
![2 Which compound is a secondary amide?
O
CH3
A HO C CH2 N
H
O
CH3
B HO C CH2 N
CH3
O
CH3
C H3C C N
H
O
CH3
D H3C C N
CH3
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_02.webp)
![3 Which compound does not react with nucleophiles?
A CH3CH2CHO
B CH3CHCH2
C CH3CH2COCH3
D CH3CH2CH2Cl
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_03.webp)
![4 Which structure represents an alicyclic compound?
A
B
C
D
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_04.webp)
![5 Which molecule is not planar?
A C2H4
B C2H6
C H2CO
D HCN
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_05.webp)
![6 What is the number of peaks in the 1H NMR spectrum of HOOCCH2CHOHCH2COOH?
A 3
B 4
C 5
D 6
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_06.webp)
![7 Ethanol can be prepared by different reactions.
Which reaction has the lowest atom economy?
A C6H12O6 → 2C2H5OH + 2CO2
B C2H4 + H2O → C2H5OH
C C2H5Br + H2O → C2H5OH + HBr
D CH3COOC2H5 + H2O → C2H5OH + CH3COOH
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_07.webp)
![8 The breakdown of ozone is catalysed by NO radicals.
Which equation is a propagation step in the mechanism for this process?
A NO + O2 → N + O3
B NO + O2 → NO2 + O
C N + O3 → NO + O2
D NO2 + O → NO + O2
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_08.webp)
![9 Which compound could have produced the IR spectrum below?
100
transmittance (%)
50
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
A CH3CH2OH
B CH3CHOHCN
C CH3COOH
D CH3CONH2
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_09.webp)
![10 Benzene reacts with an organic reagent in the presence of a halogen carrier to form
phenylethanone.
O
C
CH3
phenylethanone
Which organic reagent is required?
A CH3CH2OH
B CH3CHO
C CH3COCl
D CH3COOH
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_10.webp)
![11 How many straight-chain structural isomers of C7H15Cl contain a chiral carbon atom?
A 1
B 2
C 3
D 4
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_11.webp)
![12 The mass spectrum of (CH3)2CHCH2OH is shown below.
100
80
60
relative
intensity
40
20
0
10 20 30 40 50 60 70 80 90
m /z
Which ion is responsible for the peak with the greatest relative intensity?
A CHCH2OH+
B CH3CH2CH+
C (CH3)2CH+
D CH3CO+
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_12.webp)
![13 Which statement(s) support(s) the delocalised model for the structure of benzene?
1 All carbon–carbon bonds have the same length.
2 The enthalpy change of hydrogenation of benzene is less exothermic than expected.
3 Bromine reacts with benzene less readily than with cyclohexene.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_13.webp)
![14 A solid organic compound can be purified by recrystallisation.
Which statement(s) about recrystallisation is/are true?
1 The organic compound is more soluble in hot solvent.
2 The hot solution is cooled before the purified organic compound is collected.
3 The melting point of the purified organic compound is lower than the impure compound.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_14.webp)
![15 Which of the following could react with the compound below to form a carbon–carbon bond?
H O
C C
Br OH
1 CH3Cl and Al Cl 3
2 KCN in ethanol
3 CH3OH and H2SO4
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN18_H4322/JUN18_H4322_15.webp)
![1 Which ion has a different number of electrons from the other three ions?
A Ga3+
B Cl −
C S2−
D Ca2+
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_01.webp)
![2 An organic compound has the composition by mass:
C, 53.33 %; H, 11.11%; O, 35.56%.
What is the empirical formula of the organic compound?
A C4H8O2
B C4H10O2
C C2H4O
D C2H5O
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_02.webp)
![3 Samples of four hydrocarbons are completely burnt under the same conditions of temperature
and pressure.
Which sample produces the greatest volume of CO2?
A 0.4 mol C2H6
B 0.3 mol C3H8
C 0.2 mol C4H10
D 0.1 mol C5H12
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_03.webp)
![4 Which reaction produces the smallest atom economy of BaCl2?
A BaCl2•2H2O → BaCl2 + 2H2O
B BaO + 2HCl → BaCl2 + H2O
C BaCO3 + 2HCl → BaCl 2 + CO2 + H2O
D Ba + 2HCl → BaCl 2 + H2
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_04.webp)
![5 The burette readings from a titration are shown below.
Final reading / cm3 24.95
Initial reading / cm3 5.00
The burette used has an uncertainty of ±0.05 cm3 in each reading.
What is the percentage uncertainty of the resulting titre?
A 0.20%
B 0.25%
C 0.45%
D 0.50%
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_05.webp)
![6 Which element has atoms with the greatest number of singly occupied orbitals?
A C
B Cl
C Ca
D Ga
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_06.webp)
![7 Which compound has polar molecules?
A OCl2
B BCl3
C CCl4
D SCl6
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_07.webp)
![8 Which element has the highest melting point?
A silicon
B phosphorus
C sulfur
D chlorine
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_08.webp)
![9 What is the best explanation for the trend in boiling points down the halogens group?
A The covalent bonds become stronger.
B The hydrogen bonds become stronger.
C The permanent dipole–dipole interactions become stronger.
D The induced dipole–dipole interactions (London forces) increase.
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_09.webp)
![10 Which silver compound is insoluble in concentrated NH3(aq)?
A AgNO3
B AgCl
C AgBr
D AgI
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_10.webp)
![11 50.0 cm3 of 1.00 mol dm–3 NaOH is neutralised by 50.0 cm3 of 1.00 mol dm–3 HNO3.
The temperature increases by 6.0 °C.
The experiment is repeated using:
25.0 cm3 of 1.00 mol dm–3 NaOH and 25.0 cm3 of 1.00 mol dm–3 HNO3.
What is the increase in temperature in the second experiment?
A 1.5 °C
B 3.0 °C
C 6.0 °C
D 12.0 °C
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_11.webp)
![12 The table shows standard enthalpy changes of combustion, ΔcH.
Substance ΔcH / kJ mol–1
C(s) –393.5
H2(g) –285.8
C4H10(g) –2876.5
What is the enthalpy change for the following reaction?
4C(s) + 5H2(g) → C4H10(g)
A –2197.2 kJ mol–1
B –126.5 kJ mol–1
C +126.5 kJ mol–1
D +2197.2 kJ mol–1
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_12.webp)
![13 The reversible reaction below is allowed to reach equilibrium.
H2(g) + I2(g) 2HI(g) ΔH = –9.4 kJ mol–1
Which change in conditions would be expected to shift the equilibrium position towards the
products?
A decrease the pressure
B decrease the temperature
C increase the pressure
D increase the temperature
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_13.webp)
![14 What is the systematic name of the compound below?
Br
A E-2-bromobut-2-ene
B Z-2-bromobut-2-ene
C E-1,2-dimethyl-1-bromoethene
D Z-1,2-dimethyl-1-bromoethene
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_14.webp)
![15 The skeletal formula of an organic compound is shown below.
O
OH
What is the molecular formula of the organic compound?
A C6H10O2
B C6H11O2
C C6H12O2
D C6H13O2
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_15.webp)
![16 How many structural isomers have the molecular formula C5H12?
A 2
B 3
C 4
D 5
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_16.webp)
![17 Which organic compound has the lowest boiling point?
A 2,3,4-trimethylpentane
B 2,3-dimethylhexane
C 2-methylheptane
D octane
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_17.webp)
![18 Which alcohol reacts with an acid catalyst to form E and Z stereoisomers?
A pentan-3-ol
B pentan-1-ol
C 2-methylbutan-2-ol
D 2,2-dimethylpropan-1-ol
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_18.webp)
![19 An alcohol A is heated under reflux with sulfuric acid and potassium dichromate(VI).
The organic compound formed produces the infrared spectrum below.
100
transmittance
(%)
50
0
4000 3000 2000 1500 1000 500
wavenumber / cm–1
Which compound could be alcohol A?
A OH
OH
B
C
OH
D
HO
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_19.webp)
![20 Which alcohol is not likely to have a fragment ion at m / z = 43 in its mass spectrum?
A CH3CH2CH(OH)CH3
B CH3CH2CH2CH2OH
C CH3CH(OH)CH2CH2CH3
D (CH3)2CHCH2OH
Your answer [1]](/img/JUN17_H0321/JUN17_H0321_20.webp)
![1 Which atom is not an isotope of iodine?
Number of neutrons Mass number
A 72 125
B 74 127
C 75 128
D 77 129
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_01.webp)
![2 What is the bonding between the ligands and the metal ion in [Fe(H2O)6]2+?
A Metallic
B Ionic
C Hydrogen
D Dative covalent
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_02.webp)
![3 What is the oxidation number of Mn in K2MnO4?
A +4
B +5
C +6
D +7
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_03.webp)
![4 Which calcium compound contains the greatest percentage by mass of calcium?
A calcium carbonate
B calcium nitrate
C calcium hydroxide
D calcium sulfate
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_04.webp)
![5 0.0200 mol of calcium oxide is reacted completely with 2.00 mol dm–3 HCl.
What is the volume, in cm3, of 2.00 mol dm–3 HCl required for this reaction?
A 15
B 20
C 30
D 60
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_05.webp)
![6 How many electrons are removed from 2.02 × 10–2 g of Ne(g) atoms to form Ne+(g) ions?
A 3.36 × 10–26
B 1.66 × 10–27
C 6.02 × 1020
D 1.22 × 1022
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_06.webp)
![7 Silicon can be made by heating silicon tetrachloride, SiCl 4, with zinc.
SiCl 4 + 2Zn Si + 2ZnCl 2
8.50 g of SiCl 4 is reacted with an excess of zinc. The percentage yield of silicon is 90%.
What is the mass of silicon made?
A 1.26 g
B 1.31 g
C 1.40 g
D 1.55 g
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_07.webp)
![8 Four pairs of solutions are mixed.
Which pair of solutions forms a white precipitate?
A NH4Cl (aq) and NaOH(aq)
B KBr(aq) and AgNO3(aq)
C FeCl 3(aq) and NH3(aq)
D Cr2(SO4)3(aq) and BaCl 2(aq)
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_08.webp)
![9 Enthalpy values are provided below.
H2(g) + I2(g) 2HI(g) ΔrH = –9 kJ mol–1
Bond enthalpy
Bond
/ kJ mol–1
H–H +436
I – I +151
What is the bond enthalpy, in kJ mol–1, of the H–I bond?
A –596
B –298
C +298
D +596
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_09.webp)
![10 A reaction is zero order with respect to a reactant A.
Which concentration–time graph for reactant A is the correct shape?
A
B
C
D
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_10.webp)
![11 Aqueous Cr3+ ions are reacted with an excess of aqueous sodium hydroxide.
Which product is formed?
A Cr(OH)6 3–
B Cr(OH)3
C [Cr(OH)4(H2O)2]–
D [Cr(OH)4]3–
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_11.webp)
![12 HA and HB are two strong monobasic acids.
25.0 cm3 of 6.0 mol dm–3 HA is mixed with 45.0 cm3 of 3.0 mol dm–3 HB.
What is the H+(aq) concentration, in mol dm–3, in the resulting solution?
A 1.9
B 2.1
C 4.1
D 4.5
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_12.webp)
![13 A mixture of N2 and O2 gases has a total pressure of 1.42 atm.
The mole fraction of N2 is 0.700.
What is the partial pressure, in atm, of O2 in the mixture?
A 0.211
B 0.426
C 0.493
D 0.994
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_13.webp)
![14 A cell is constructed from the two redox systems below.
Cu2+(aq) + 2e– Cu(s) E ө = +0.34 V
Ag+(aq) + e– Ag(s) E ө = +0.80 V
Which statement(s) is/are correct for the cell?
1 The cell potential is 1.14 V.
2 The reaction at the copper electrode is Cu(s) Cu2+(aq) + 2e–.
3 The silver electrode increases in mass.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_14.webp)
![15 Which electron configuration(s) is/are correct?
1 Cr atom: 1s22s22p63s23p63d54s1
2 Cu atom: 1s22s22p63s23p63d104s1
3 Fe2+ ion: 1s22s22p63s23p63d54s1
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]](/img/JUN17_H4321/JUN17_H4321_15.webp)
![1 A chemist compares the rates of hydrolysis of 1-chloropropane and 1-bromopropane in ethanol.
Which reagent in aqueous solution should be used?
A Silver chloride
B Silver nitrate
C Potassium chloride
D Potassium nitrate
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_01.webp)
![2 How can the molecule below be described?
OH
A Aromatic and alicyclic
B Aliphatic and unsaturated
C Aromatic and unsaturated
D Alicyclic and saturated
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_02.webp)
![3 Complete combustion of an organic compound forms 40 cm3 of carbon dioxide and 40 cm3 of
water vapour, under the same conditions of temperature and pressure.
Which molecular formula could the organic compound have?
A C3H8
B C2H2O
C C2H4O
D C2H3N
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_03.webp)
![4 Which molecule is a Z-isomer?
H3C H Cl F F CH3 H CH3
C C C C C C C C
H F H CH3 Cl H H F
A B C D
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_04.webp)
![5 Which type of reaction has the greatest atom economy?
A Substitution
B Hydrolysis
C Elimination
D Addition
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_05.webp)
![6 Four atoms, 1–4, are labelled in the structure below.
4
NH2
1 CH 3 OH
H3C 2 C
O
Which atom has a trigonal planar arrangement of bonds around it?
A Atom 1
B Atom 2
C Atom 3
D Atom 4
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_06.webp)
![7 Which molecule is a secondary amine?
NH N
O O
NH N
O O
A B C D
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_07.webp)
![8 What is the number of chiral centres in the molecule below?
NH2
H
N
S
O
N
HO
O
OH
O
A 2
B 3
C 4
D 5
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_08.webp)
![9 What is the molecular formula of the compound below?
A C7H10
B C7H12
C C7H14
D C7H16
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_09.webp)
![10 Equal amounts of the four compounds are added to the same volume of water.
Which compound would produce the most acidic solution?
A CH3CONH2
B CH3COOH
C CH3COOCH3
D CH3COCl
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_10.webp)
![11 The compound below is analysed by 1H NMR spectroscopy.
O O
HO OH
How many peaks are observed in the 1H NMR spectrum?
A 5
B 4
C 3
D 2
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_11.webp)
![12 0.1 mol of HOOCCH2COOH are reacted with 0.1 mol of aqueous NaOH.
How many molecules of water are formed?
A 6.02 × 1022
B 3.01 × 1022
C 6.02 × 1023
D 3.01 × 1023
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_12.webp)
![13 Which reagents could be used to prepare CH3CH2CONHCH3?
A CH3CH2COCl + CH3NH2
B CH3CH2CONH2 + CH3Br
C CH3CH2COONa + CH3NH2
D CH3CH2COCH3 + NH3
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_13.webp)
![14 Ethane reacts with chlorine by radical substitution to form chloroethane.
Which radical(s) is/are present in the mechanism?
1 H
2 Cl
3 C2H5
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_14.webp)
![15 Which compound(s) is a/are structural isomer(s) of C6H12O2?
1 hexanoic acid
2 ethyl butanoate
3 propyl propanoate
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer
[1]](/img/JUN17_H4322/JUN17_H4322_15.webp)
![1 Which row shows the atomic structure of 37Cl–?
protons neutrons electrons
A 17 18 20
B 17 20 18
C 18 19 17
D 20 17 21
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_01.webp)
![2 What is the formula of ammonium sulfide?
A NH4S
B NH4SO4
C (NH4)2S
D (NH4)2SO4
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_02.webp)
![3 Calcium nitrate, Ca(NO3)2, decomposes when heated, as shown below.
Ca(NO3)2(s) → CaO(s) + 2NO2(g) + ½O2(g)
A student decomposes 0.00500 mol of Ca(NO3)2 and collects the gas that is produced.
Calculate the volume of gas that the student should expect to collect, measured at room
temperature and pressure.
A 60 cm3
B 120 cm3
C 240 cm3
D 300 cm3
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_03.webp)
![3
4 Which equation is not a neutralisation reaction?
A Ca(s) + 2HCl(aq) → CaCl2(aq) + H2(g)
B H+(aq) + OH–(aq) → H2O(l)
C K2CO3(s) + 2HNO3(aq) → 2KNO3(aq) + H2O(l) + CO2(g)
D NH3(aq) + HCl(aq) → NH4Cl(aq)
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_04.webp)
![5 What is the oxidation number of nitrogen in Mg(NO3)2?
A –3
B +2
C +5
D +6
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_05.webp)
![6 How many orbitals are occupied in a silicon atom?
A 5
B 7
C 8
D 9
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_06.webp)
![4
7 A ‘dot-and-cross’ diagram for nitrogen trichloride, NCl3, is shown below.
X X
Cl X N Cl
X
X
Cl
Which row shows the correct shape and bond angle in a molecule of NCl3?
Name of shape Bond angle
A Pyramidal 104.5°
B Pyramidal 107°
C Tetrahedral 107°
D Trigonal planar 120°
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_07.webp)
![8 What is the shape around the carbon atoms in graphene?
A linear
B pyramidal
C tetrahedral
D trigonal planar
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_08.webp)
![5
9 Electron configurations for atoms of different elements are shown below.
Which electron configuration represents the element with the largest first ionisation energy?
A 1s22s2
B 1s22s22p4
C 1s22s22p6
D 1s22s22p63s2
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_09.webp)
![10 Successive ionisation energies of four elements in Period 3 are shown below.
Which letter could represent magnesium?
Ionisation energy / kJ mol–1
1st 2nd 3rd 4th 5th
A 1251 2298 3822 5159 6542
B 738 1451 7733 10543 13630
C 496 4563 6913 9544 13352
D 578 1817 2745 11577 14842
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_10.webp)
![11 A student adds aqueous sodium carbonate to one test-tube and aqueous silver nitrate to a second
test-tube.
The student adds dilute sulfuric acid to each test-tube.
Which row has the correct observations?
Aqueous sodium carbonate Aqueous silver nitrate
A no change precipitate
B no change no change
C effervescence no change
D effervescence precipitate
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_11.webp)
![6
12 The enthalpy change of formation of butane can be calculated using the enthalpy changes of
combustion, ΔcH, below.
Substance C(s) H2(g) C4H10(g)
ΔcH / kJ mol–1 –394 –286 –2877
Calculate the enthalpy change of formation of C4H10(g).
4C(s) + 5H2(g) → C4H10(g)
A –2197 kJ mol–1
B –129 kJ mol–1
C +129 kJ mol–1
D +2197 kJ mol–1
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_12.webp)
![13 The skeletal formulae of four alcohols, E, F, G and H, are shown below.
OH
OH
E F
HO OH
G H
Which pair of alcohols are structural isomers of each other?
A E and F
B E and G
C E and H
D F and G
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_13.webp)
![7
14 What is the name of the following compound?
Cl Cl
H3C C C CH3
H CH3
A 1,2-dichloro-1,2-dimethylpropane
B 2,3-dichloro-2,3-dimethylpropane
C 2,3-dichloro-2-methylbutane
D 2,3-dichloro-3-methylbutane
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_14.webp)
![15 Which compound has non-polar molecules?
A E-1,2-dichlorobut-2-ene
B E-2,3-dichlorobut-2-ene
C Z-2,3-dichlorobut-2-ene
D Z-1,4-dichlorobut-2-ene
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_15.webp)
![8
16 The displayed formula for a hydrocarbon is shown below.
H H
H C
C C H
H C C
H
H H
How many σ and π bonds are present in a molecule of this hydrocarbon?
σ bonds π bonds
A 2 4
B 10 2
C 10 4
D 12 2
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_16.webp)
![17 Chlorine reacts with 1-chloropropane in the presence of ultraviolet radiation via a radical
substitution mechanism.
Which equation shows a propagation step in the mechanism for this reaction?
A Cl2 → •Cl + •Cl
B •Cl + •C3H6Cl → C3H6Cl2
C C3H7Cl + •Cl → C3H6Cl2 + •H
D •Cl + C3H7Cl → •C3H6Cl + HCl
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_17.webp)
![9
18 Which alcohol can be oxidised by K2Cr2O7 and H2SO4 to form a ketone?
A
OH
B
OH
C
OH
OH
D
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_18.webp)
![10
19 A reaction sequence is shown below:
Step 1 CH3CH=CHCH3 + HBr → CH3CH2CHBrCH3
Step 2 CH3CH2CHBrCH3 + NaOH → CH3CH2CH(OH)CH3 + NaBr
Which type of reaction mechanism is involved in each step?
Step 1 Step 2
A electrophilic addition electrophilic substitution
B electrophilic addition nucleophilic substitution
C nucleophilic addition electrophilic substitution
D nucleophilic addition nucleophilic substitution
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_19.webp)
![20 When heated with NaOH(aq), 1-iodobutane is hydrolysed at a much faster rate than 1-chlorobutane.
Which statement explains the different rates?
A The C–I bond enthalpy is greater than the C–Cl bond enthalpy.
B The C–I bond is less polar than the C–Cl bond.
C The C–I bond has a C atom with a greater δ+ charge than in the C–Cl bond.
D The C–I bond requires less energy to break than the C–Cl bond.
Your answer [1]](/img/JUN16_H0321/JUN16_H0321_20.webp)
