Chemistry 9701/11 May/June 2025: question paper and mark scheme

Question

ICl 3 reacts with water in a redox reaction. vICl 3 + wH2O → xHCl + yHI + zHIO3 + zHCl O3 What are the numbers v, x and z in the correctly balanced equation? v x z A 2 8 1 B 2 5 1 C 3 8 1 D 3 5 1

Question

The rate of the reaction between a reactive metal and an excess of a dilute acid is investigated. The total volume of hydrogen gas produced is recorded every 30 seconds for 3 minutes. total volume of time / s hydrogen gas / cm3 0 0 30 64 60 105 90 132 120 151 150 161 180 167 The average rate of reaction during the first 30 seconds is P. The average rate of reaction during the last 30 seconds is Q. What is the value of P – Q? A 1.21 cm3 s–1 B 1.93 cm3 s–1 C 2.13 cm3 s–1 D 3.43 cm3 s–1

Question

In the diagram, curve X was obtained by measuring the volume of oxygen produced during the decomposition of 100 cm3 of 1.0 mol dm–3 hydrogen peroxide. A catalyst of manganese(IV) oxide was used. Y X volume of oxygen formed 0 0 time Which alteration to the original experimental conditions would produce curve Y? A adding more manganese(IV) oxide B adding some 0.1 mol dm–3 hydrogen peroxide C adding water D raising the temperature

Question

The first seven ionisation energies of an element between lithium and neon in the Periodic Table are shown. 1310 3390 5320 7450 11 000 13 300 71 000 kJ mol–1 What is the outer electronic configuration of the element? A 2s2 B 2s22p1 C 2s22p4 D 2s22p6

Question

The reaction of hydrogen with oxygen is shown. 2H2(g) + O2(g) → 2H2O(l) Which expression corresponds to the standard enthalpy change of this reaction? A 2× (H2O) B (H2O) – (H2) C (H2) D 2× (H2O) + 2 × (H2)

Question

P is a compound that burns in an excess of oxygen to give carbon dioxide and water only. 2.20 g of P contains 1.20 g of carbon and 0.20 g of hydrogen. When P is added to a solution of sodium carbonate, bubbles of gas are seen. What is P? A CH3CHO B CH3CO2H C CH3COCH2CH2OH D CH3CH2CH2CO2H

Question

Substance W has the physical properties shown. electrical conductivity m.p. / °C b.p. / °C of solid of liquid in water 2072 2980 poor good insoluble What is substance W? A aluminium oxide B iron C silicon dioxide D sodium fluoride

Question

Which diagram represents the lattice structure of sodium chloride? A B Na Cl Na Cl + – + – key Cl Na Cl Na – + – + Cl = chlorine atom Na Cl Na Cl + – + – Na = sodium atom – = chloride ion Cl Na Cl Na – + – + + = sodium ion C D – – – – + – + + + + + – – – – – + – + – + + + + – – – – – – + – + + + + + – – – + – + – + + + + – – – –

Question

An aqueous solution X contains substance HQ which behaves as a weak acid. HQ(aq) H+(aq) + Q–(aq) The soluble salt NaQ is added to X. What happens to the [H+(aq)] and the pH in X? [H+(aq)] pH A decreases decreases B decreases increases C increases decreases D increases increases

Question

Dinitrogen tetroxide, N2O4, decomposes reversibly. N2O4 2NO2 ΔH = +58.0 kJ mol–1 An equilibrium mixture of N2O4 and NO2 gases is placed in a closed container under standard conditions. Kc = 1.15 × 10–1 mol dm–3 The conditions are changed. Under the new conditions, Kc = 1.70 × 103 mol dm–3. Which change in conditions occurs? A The pressure increases. B The pressure decreases. C The temperature increases. D The temperature decreases. 11 50 cm3 of 1.0 mol dm–3 H2SO4 is added to 100 cm3 of 1.0 mol dm–3 NaOH in an insulated vessel. Both solutions are at a temperature of 20 °C before mixing. After mixing, the temperature rises and the highest temperature reached is 29 °C. Assume that: ● all the energy released in the reaction goes into raising the temperature of the aqueous reaction mixture ● the specific heat capacity of the mixture is 4.2 J cm–3 K–1. What is the value of the enthalpy of neutralisation determined from this experiment? A –113.4 kJ mol–1 B –56.7 kJ mol–1 C –37.8 kJ mol–1 D –18.9 kJ mol–1

Question

In the question paper above.

Question

Barium dithionate, BaS2O6•2H2O, is soluble in water. S2O62– ions slowly decompose in acidic solution. S2O62–(aq) → SO2(g) + SO42–(aq) 3.513 g of BaS2O6•2H2O is dissolved in water in a 100 cm3 volumetric flask and the solution made up to the mark with HCl (aq). At time x min, a white precipitate of mass 0.661 g is present in the flask. What is the concentration of BaS2O6 in the volumetric flask at time x min? A 0.0077 mol dm–3 B 0.0090 mol dm–3 C 0.077 mol dm–3 D 0.090 mol dm–3

Question

The diagram shows two containers of methane connected by a closed tap. Each container has a volume of 1.00 m3. 16 g methane tap 96 g methane at 100 kPa at 200 kPa The tap is opened. The temperature of the system is changed to 800 K. The system reaches constant pressure. What is the pressure of methane within the system? A 23.3 kPa B 46.6 kPa C 186 kPa D 372 kPa

Question

Which statement about a 3p orbital is correct? A It can hold a maximum of six electrons. B It has the highest energy of the orbitals with principal quantum number 3. C It is at a higher energy level than a 3s orbital but has the same shape. D It is occupied by one electron in an isolated phosphorus atom.

Question

In which pair do both species: ● have the same shape ● have the same number of covalent bonds? A methane and the ammonium ion B carbon dioxide and nitrogen C boron trifluoride and ammonia D water and oxygen

Question

A reaction involving ammonium ions is shown. NH4+ + OH– NH3 + H2O Four statements about this reaction are listed. 1 The ammonium ions are reduced. 2 In the reverse reaction, ammonia acts as a Brønsted–Lowry base. 3 The ammonium ion and the ammonia molecule have the same bond angle. 4 This reaction is not a redox reaction. Which statements are correct? A 1 and 2 B 1 and 3 C 2 and 4 D 3 and 4

Question

Which reduction process occurs on the surface of a catalytic converter? A reduction of carbon dioxide and nitrogen oxides B reduction of carbon dioxide only C reduction of nitrogen oxides only D reduction of carbon monoxide

Question

Three statements about the halogens, chlorine, bromine and iodine and their compounds are listed. 1 The halogen with the highest boiling point has atoms which form the strongest bond to hydrogen. 2 The halogen with the strongest instantaneous dipole (id–id) attractions forms the most thermally stable hydrogen halide. 3 The most volatile element most rapidly oxidises hydrogen. Which statements are correct? A 1 and 2 B 1 only C 2 and 3 D 3 only

Question

Which reagent or reagents and conditions will oxidise chlorine, Cl 2, into a compound containing chlorine in the +5 oxidation state? A AgNO3(aq) followed by NH3(aq) at room temperature B concentrated H2SO4 at room temperature C cold dilute NaOH(aq) D hot concentrated NaOH(aq)

Question

Which diagram shows the electronegativity of the elements Na, Mg, Al and Si plotted against their first ionisation energies? A B Si Si Al Al electronegativity electronegativity Mg Mg Na Na first ionisation energy first ionisation energy C D Na Na Al Mg electronegativity electronegativity Mg Al Si Si first ionisation energy first ionisation energy

Question

Radium is an element below barium in Group 2 of the Periodic Table. Which equation shows what happens when solid radium nitrate, Ra(NO3)2, is heated strongly? A 2Ra(NO3)2(s) → 2RaO(s) + 4NO2(g) + O2(g) B 2Ra(NO3)2(s) → 2RaO(s) + 2N2(g) + 5O2(g) C Ra(NO3)2(s) → RaO(s) + N2O(g) + 2O2(g) D 4Ra(NO3)2(s) → 2Ra2O(s) + 8NO2(g) + 3O2(g)

Question

The table shows some data for the elements in Period 3 of the Periodic Table. melting electrical point / K conductivity sodium 371 good magnesium 922 good aluminium 933 good silicon 1693 poor phosphorus 317 does not conduct sulfur 386 does not conduct chlorine 172 does not conduct argon 84 does not conduct Which statements are correct? 1 All the elements in the table with a giant structure have a higher melting point than each of the elements in the table with a simple molecular structure. 2 Magnesium has a higher melting point than sodium because it has more delocalised electrons and stronger electrostatic attraction between the delocalised electrons and the metal ions. 3 Phosphorus and sulfur do not conduct electricity because they are simple molecular solids at room conditions. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Each mineral listed behaves as a mixture of two carbonate compounds. They can be used as fire retardants because they decompose in the heat, producing CO2. This gas smothers the fire. barytocite, BaCa(CO3)2 dolomite, CaMg(CO3)2 huntite, Mg3Ca(CO3)4 What is the order of effectiveness as fire retardants, from best to worst? best worst A dolomite barytocite huntite B dolomite huntite barytocite C huntite barytocite dolomite D huntite dolomite barytocite

Question

Compound X contains two Period 3 elements, Y and Z. Compound X reacts with water to form only two products: a slightly soluble hydroxide and compound Q. Q is a compound of element Z and hydrogen. Compound Q burns in moist air to produce an oxide and water. The oxidation number of element Z in the oxide is +5. Which row identifies element Y and element Z? element Y element Z A Mg P B Na S C Na P D Mg S

Question

Three reagents are listed. 1 aqueous sodium carbonate 2 LiAl H4 3 water Which reagents react with pure ethanoic acid to give a solution containing ethanoate ions? A 1 and 2 B 1 and 3 C 1 only D 2 and 3

Question

Complete combustion of compound T produces carbon dioxide and water only. Compound T produces steamy fumes with PCl 5. Compound T does not give any visible product with 2,4-dinitrophenylhydrazine reagent. What can be deduced with certainty from this information? A Compound T is a carboxylic acid. B Compound T is a hydrocarbon. C Compound T is an alcohol. D Compound T is not an aldehyde.

Question

Information about carbonyl compound X is given. ● Compound X reacts with LiAl H4 to produce a secondary alcohol. ● Compound X reacts with alkaline I2(aq) to give a yellow precipitate. What is compound X? A butanal B butanone C ethanal D pentan-3-one

Question

An organic compound J reacts with an excess of sodium to produce an organic ion with a charge of –3. J reacts with an excess of NaOH(aq) to produce an organic ion with a charge of –1. What is the structural formula of J? A HOCH2CH(OH)CH2CO2H B HO2CCH(OH)CH2CHO C HO2CCH(OH)CH2CO2H D HOCH2COCH2CHO

Question

Which formula represents the organic compound formed by the reaction of propanoic acid with methanol in the presence of concentrated sulfuric acid as a catalyst? A CH3CH2COCH3 B CH3CH2CO2CH3 C CH3CO2CH2CH3 D CH3CH2CH2CO2CH3

Question

Structural isomerism and stereoisomerism should be considered when answering this question. 2,5-dibromohexane is heated under reflux with ethanolic KOH. How many isomeric compounds are formed with molecular formula C6H10? A 3 B 5 C 6 D 7

Question

Considering only structural isomers, what is the number of alcohols of each type with the formula C5H12O? primary secondary tertiary A 3 3 2 B 4 2 2 C 4 3 1 D 5 2 1

Question

Which structure represents part of the polymer chain of PVC? A B H Cl H H H Cl H Cl H Cl H Cl C C C C C C C C C C C C H H H Cl H H Cl H Cl H Cl H C D H Cl H H H Cl Cl Cl Cl Cl Cl Cl C C C C C C C C C C C C H H H H H H H H H H H H

Question

A possible mechanism for the exothermic hydrolysis of 2-chloro-2-methylpropane is shown. CH3 CH3 slow CH3 C Cl CH3 C+ + Cl – CH3 CH3 CH3 CH3 fast CH3 C+ + OH– CH3 C OH CH3 CH3 Which diagram represents the reaction pathway diagram for this mechanism? A B energy energy reaction pathway reaction pathway C D energy energy reaction pathway reaction pathway

Question

Compound W contains atoms of carbon, nitrogen and hydrogen. Compound W reacts with HCl (aq) to produce propanoic acid. Which row is correct? functional group name of in compound W compound W A amine ethylamine B nitrile ethanenitrile C amine propylamine D nitrile propanenitrile

Question

Two reactions are described. 1 2-bromo-2-methylbutane heated with NaOH(aq) 2 2-chloro-2-methylbutane heated with NaOH(aq) In both reactions, the conditions are the same and NaOH(aq) is in excess. 30.18 g of 2-bromo-2-methylbutane forms 12.32 g of product X. [Mr: 2-bromo-2-methylbutane, 150.9; 2-chloro-2-methylbutane, 106.5] Which row is correct? percentage yield relative rate of product X / % of reaction A 41 1 is faster than 2 B 41 2 is faster than 1 C 70 1 is faster than 2 D 70 2 is faster than 1

Question

An alkene P reacts with an excess of hot concentrated acidified KMnO4(aq). Methylpropanoic acid is the only organic product. What is alkene P? A 2,5-dimethylhex-3-ene B 2-methylbut-2-ene C methylpropene D oct-4-ene, C8H16

Question

Three substances are listed. 1 butane 2 hydrogen 3 hydrogen bromide Which substances are possible products of the free-radical substitution reaction between ethane and bromine? A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

The structure of the testosterone molecule is shown. OH CH3 C2 CH3 O C1 Which statements are correct? 1 Carbon atoms C1 and C2 can be oxidised with acidified K2Cr2O7. 2 There are fewer than 27 hydrogen atoms in one testosterone molecule. 3 There are six chiral carbon atoms in one testosterone molecule. A 1 only B 2 and 3 C 2 only D 3 only

Question

The structural formula of hept-1,4,5-triene is shown. CH2CHCH2CHCCHCH3 How many of the carbon atoms in one molecule of hept-1,4,5-triene are sp2 hybridised? A 4 B 5 C 6 D 7

Question

Hydrocarbon X is saturated. Each molecule contains one ring of carbon atoms. The mass spectrum of hydrocarbon X is measured. The peak representing the M+ ion is 14 mm high. The peak representing the [M+1]+ ion is 0.77 mm high. What is the m / e value for the M+ ion of X? A 56 B 58 C 70 D 72 Important values, constants and standards molar gas constant R = 8.31 J K–1 mol–1 Faraday constant F = 9.65 × 104 C mol–1 Avogadro constant L = 6.022 × 1023 mol–1 electronic charge e = –1.60 × 10–19 C molar volume of gas Vm = 22.4 dm3 mol–1 at s.t.p. (101 kPa and 273 K) Vm = 24.0 dm3 mol–1 at room conditions ionic product of water Kw = 1.00 × 10–14 mol2 dm–6 (at 298 K (25 °C)) specific heat capacity of water c = 4.18 kJ kg–1 K–1 (4.18 J g–1 K–1) The Periodic Table of Elements Group 1 2 13 14 15 16 17 18 1 2 H He hydrogen helium Key 1.0 4.0 3 4 atomic number 5 6 7 8 9 10 Li Be atomic symbol B C N O F Ne lithium beryllium name boron carbon nitrogen oxygen fluorine neon 6.9 9.0 relative atomic mass 10.8 12.0 14.0 16.0 19.0 20.2 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar sodium magnesium aluminium silicon phosphorus sulfur chlorine argon 23.0 24.3 3 4 5 6 7 8 9 10 11 12 27.0 28.1 31.0 32.1 35.5 39.9 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton 39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 20 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon 85.5 87.6 88.9 91.2 92.9 95.9 – 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 lanthanoids Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon 132.9 137.3 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 – – – 87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson – – – – – – – – – – – – – – – – – 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium 138.9 140.1 140.9 144.2 – 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.1 175.0 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium – 232.0 231.0 238.0 – – – – – – – – – – –