中文（繁體）
中文（简体）
English
CIE A-Level Chemistry 9701 Paper 2 Practice Paper (AS Structured) – 60 marks, 1 hour 15 minutes, answers and mark scheme included
TutorZone original practice paper – CIE A-Level Chemistry 9701 Paper 2 (AS structured)
6 questions, 27 parts – 60 marks – 1 hour 15 minutes – calculator allowed
Paper structure
| Paper | Time | Marks | Weighting |
|---|---|---|---|
| Paper 2 (AS structured) | 1 h 15 min | 60 marks | 30% of AS |
| Paper 1 (multiple choice) | 1 h | 40 marks | 15.5% of AS |
| Paper 3 (AS practical skills) | 1 h 15 min | 40 marks | 15.5% of AS |
Questions
Total: 60 marks · 1 hour 15 minutes · calculator allowed
Q 1 · Atomic structure and the mole [10]
(a) Define the term relative atomic mass. [2]
(b) Copper has two natural isotopes: 63Cu (69.2%) and 65Cu (30.8%). Calculate the relative atomic mass of copper to 3 significant figures. [2]
(c) How many moles and how many molecules are there in 4.40 g of carbon dioxide? (Ar: C=12.0, O=16.0; L=6.02×10^23) [3]
(d) 25.0 cm3 of 0.200 mol/dm3 sodium hydroxide solution: calculate the amount, in mol, and the mass of NaOH present. (Mr: NaOH = 40.0) [3]
Q 2 · Chemical bonding and structure [10]
(a) Write the electron configuration of Mg2+ and Cl- (in the form 1s2 2s2 …) and state the total number of electrons in each ion. [3]
(b) The melting point of magnesium oxide (2,852 C) is much higher than that of sodium chloride (801 C). Explain why. [3]
(c) State the shape of the ammonium ion, NH4+, and its bond angle. [2]
(d) Explain why boron trifluoride, BF3, is trigonal planar with bond angles of 120 degrees. [2]
Q 3 · Energetics [10]
(a) Use bond enthalpies to calculate the enthalpy change of hydrogenation: C2H4 + H2 -> C2H6. C=C 612, C-C 348, C-H 410, H-H 436 kJ/mol. [3]
(b) In terms of bond breaking and bond making, explain why the reaction above is exothermic. [2]
(c) Burning 0.0250 mol of a fuel raises the temperature of 50.0 g of water by 6.8 C. Specific heat capacity of water = 4.18 J g-1 K-1. Calculate the heat released, q, and the enthalpy change per mole of fuel. [3]
(d) The experimental value is usually less exothermic than the standard value in the Data Booklet. Give two reasons. [2]
Q 4 · Reaction rates and equilibrium [12]
(a) The concentration of a reactant falls from 0.060 to 0.015 mol/dm3 in 45 s. Calculate the average rate of reaction, with units. [2]
(b) Using collision theory, explain why the rate of reaction decreases as the reaction proceeds. [2]
(c) A reaction is first order with respect to a reactant and has a half-life of 24 s. Starting from 0.80 mol/dm3, what is the concentration after 72 s? [3]
(d) 0.500 mol each of H2 and I2 are mixed in a 1.00 dm3 vessel. At equilibrium [HI] = 0.780 mol/dm3. Calculate Kc for H2 + I2 <=> 2HI. [4]
(e) If the forward reaction is exothermic, state the effect of raising the temperature on the value of Kc. [1]
Q 5 · Organic chemistry: alkenes [10]
(a) State the general formula of the alkenes and explain why alkenes are described as unsaturated. [2]
(b) But-1-ene reacts with hydrogen bromide. Name the major product and state the type of reaction. [2]
(c) An alkene contains 85.7% carbon and 14.3% hydrogen by mass and has Mr = 56. Determine its empirical and molecular formulae. (Ar: C=12.0, H=1.0) [4]
(d) Describe one laboratory test to distinguish the alkene from hexane. [1]
(e) Propene undergoes addition polymerisation to form poly(propene). State the relative molecular mass of the repeat unit. [1]
Q 6 · Group 2 and periodicity [8]
(a) Explain the trend in atomic radius down Group 2. [2]
(b) State and explain the trend in reactivity of Group 2 elements with water. [2]
(c) Write the equation for the reaction of magnesium with steam, including state symbols. [1]
(d) 0.240 g of magnesium reacts with excess steam. Calculate the volume of hydrogen formed at room temperature and pressure (molar volume 24.0 dm3/mol; Ar: Mg = 24.3). [2]
(e) State how the thermal stability of Group 2 nitrates changes down the group. [1]
Answers and mark scheme
| Part | Answer | Marking points | marks |
|---|---|---|---|
| 1(a) | The weighted mean mass of the atoms of an element compared with 1/12 of the mass of an atom of carbon-12. | 1 mark: weighted mean mass of the atoms (allowance for isotopic abundances) 1 mark: compared with 1/12 of the mass of an atom of 12C |
2 |
| 1(b) | Ar(Cu) = 63×0.692 + 65×0.308 = 43.60 + 20.02 = 63.6 | 1 mark: 63×0.692 + 65×0.308 1 mark: 63.6 |
2 |
| 1(c) | Mr(CO2) = 12.0 + 2(16.0) = 44.0; n = 4.40/44.0 = 0.100 mol; molecules = 0.100 x 6.02×10^23 = 6.02×10^22 | 1 mark: Mr = 44.0 1 mark: n = 0.100 mol 1 mark: 6.02×10^22 |
3 |
| 1(d) | n = 0.200 x 25.0/1000 = 5.00×10^-3 mol; m = 5.00×10^-3 x 40.0 = 0.200 g | 1 mark: volume converted to dm3 1 mark: n = 5.00×10^-3 mol 1 mark: m = 0.200 g |
3 |
| 2(a) | Mg2+: 1s2 2s2 2p6, 10 electrons; Cl-: 1s2 2s2 2p6 3s2 3p6, 18 electrons. | 1 mark: Mg2+ configuration / 10 electrons 1 mark: Cl- configuration / 18 electrons 1 mark: both configurations fully correct |
3 |
| 2(b) | Both are giant ionic lattices; the ions in MgO carry higher charges (2+ and 2-) than in NaCl (1+ and 1-), so the electrostatic attraction is stronger and more energy is needed to break the lattice. | 1 mark: both giant ionic lattices 1 mark: higher ionic charges in MgO 1 mark: stronger electrostatic attraction / more energy needed |
3 |
| 2(c) | Tetrahedral; bond angle 109.5 degrees. | 1 mark: tetrahedral 1 mark: 109.5 degrees |
2 |
| 2(d) | Boron has three bonding pairs and no lone pairs; the three pairs repel to maximum separation, giving a planar arrangement with 120 degree angles. | 1 mark: three bonding pairs, no lone pairs 1 mark: maximum separation of pairs gives 120 degrees in one plane |
2 |
| 3(a) | Bonds broken: 612 + 4×410 + 436 = 2,688 kJ/mol; bonds formed: 348 + 6×410 = 2,808 kJ/mol; dH = 2,688 – 2,808 = -120 kJ/mol | 1 mark: broken = 2,688 1 mark: formed = 2,808 1 mark: dH = -120 kJ/mol (sign required) |
3 |
| 3(b) | The energy released when new bonds form (2,808 kJ/mol) is greater than the energy absorbed when bonds break (2,688 kJ/mol), so energy is released overall. | 1 mark: more energy released than absorbed 1 mark: supported by the values in (a) |
2 |
| 3(c) | q = mc dT = 50.0 x 4.18 x 6.8 = 1,421 J = 1.42 kJ; dH = -1.421/0.0250 = -56.8 kJ/mol | 1 mark: q = 1,421 J 1 mark: divided by 0.0250 mol 1 mark: -56.8 kJ/mol |
3 |
| 3(d) | Heat loss to the surroundings; incomplete combustion or non-standard conditions. | 1 mark: heat loss to surroundings 1 mark: incomplete combustion / non-standard conditions |
2 |
| 4(a) | rate = (0.060 – 0.015)/45 = 1.0×10^-3 mol dm-3 s-1 | 1 mark: change = 0.045 mol dm-3 1 mark: 1.0×10^-3 mol dm-3 s-1 with units |
2 |
| 4(b) | The concentration of reactants falls, so there are fewer collisions per unit time and fewer successful collisions with energy above the activation energy. | 1 mark: concentration falls so collision frequency drops 1 mark: fewer collisions with E >= Ea |
2 |
| 4(c) | 72/24 = 3 half-lives; 0.80 -> 0.40 -> 0.20 -> 0.10 mol/dm3 | 1 mark: three half-lives 1 mark: successive halving shown 1 mark: 0.10 mol dm-3 |
3 |
| 4(d) | HI formed 0.780 mol, so 0.390 mol of each reactant reacted; at equilibrium [H2] = [I2] = 0.500 – 0.390 = 0.110 mol/dm3; Kc = 0.780^2/(0.110 x 0.110) = 0.6084/0.0121 = 50.3 (no units) | 1 mark: 0.390 mol reacted 1 mark: equilibrium conc 0.110 mol dm-3 1 mark: correct Kc expression 1 mark: Kc = 50.3 |
4 |
| 4(e) | Kc decreases (equilibrium shifts in the endothermic direction). | 1 mark: Kc decreases | 1 |
| 5(a) | General formula CnH2n; they contain a C=C double bond so the carbon atoms are not bonded to the maximum number of hydrogen atoms. | 1 mark: CnH2n 1 mark: C=C present / not maximum number of hydrogens |
2 |
| 5(b) | Major product: 2-bromobutane; reaction type: electrophilic addition. | 1 mark: 2-bromobutane 1 mark: electrophilic addition |
2 |
| 5(c) | C: 85.7/12.0 = 7.14; H: 14.3/1.0 = 14.3; ratio 7.14:14.3 = 1:2, so empirical formula CH2 (Mr 14.0); 56/14 = 4, so molecular formula C4H8 | 1 mark: mol C = 7.14 1 mark: mol H = 14.3, ratio 1:2 1 mark: empirical formula CH2 1 mark: molecular formula C4H8 |
4 |
| 5(d) | Add bromine water and shake: the alkene decolourises the orange bromine water, hexane does not. | 1 mark: bromine water decolourised by alkene only | 1 |
| 5(e) | The repeat unit is C3H6, Mr = 3×12.0 + 6×1.0 = 42.0 | 1 mark: 42.0 | 1 |
| 6(a) | Each element down the group has one more occupied shell; increased shielding outweighs the greater nuclear charge, so the outer electrons are less strongly attracted and the radius increases. | 1 mark: extra shell / more shielding 1 mark: weaker attraction from nucleus, radius increases |
2 |
| 6(b) | Reactivity increases down the group; the first and second ionisation energies decrease, so less energy is needed to lose the two outer electrons. | 1 mark: reactivity increases down the group 1 mark: lower ionisation energies / electrons lost more easily |
2 |
| 6(c) | Mg(s) + H2O(g) -> MgO(s) + H2(g) | 1 mark: correct equation with state symbols | 1 |
| 6(d) | n(Mg) = 0.240/24.3 = 9.88×10^-3 mol; V(H2) = 9.88×10^-3 x 24.0 = 0.237 dm3 = 237 cm3 | 1 mark: n = 9.88×10^-3 mol 1 mark: 0.237 dm3 / 237 cm3 |
2 |
| 6(e) | Thermal stability increases down the group. | 1 mark: thermal stability increases | 1 |
Topic map
| Question | Topic | Marks |
|---|---|---|
| 1 | Atomic structure and the mole | 10 |
| 2 | Bonding and structure | 10 |
| 3 | Energetics | 10 |
| 4 | Rates and equilibrium | 12 |
| 5 | Organic chemistry: alkenes | 10 |
| 6 | Group 2 and periodicity | 8 |
Common lost marks
- Giving “average mass” for relative atomic mass without comparing with 1/12 of carbon-12.
- Using only bond breaking or only bond forming, so both the value and sign of dH are wrong.
- Substituting initial concentrations into Kc instead of equilibrium concentrations.
- Giving the final concentration of a first-order decay without showing successive halving.
- Saying “double bond” rather than C=C, or confusing empirical and molecular formulae.
FAQ
Who is this paper for?
AS students preparing for CIE A-Level Chemistry 9701 who want focused practice on Paper 2 structured questions.
Does the answer booklet include a mark scheme?
Yes. Every part lists its marking points so you can mark yourself or a tutor can mark point by point.
Can I print it?
Yes, both the question paper and the answer booklet are A4 PDFs ready to print.
This is original TutorZone practice material, not a past examination paper.
Format follows the CIE 9701 Chemistry syllabus (2025-2027) Paper 2: 1 h 15 min, 60 marks, AS structured questions.
