Chemistry 9701/11 May/June 2024: question paper and mark scheme

Question

Sample X is added to water and made up to a total volume of 200 cm3. This gives a solution of 0.100 mol dm–3 HCl. What is X? A 10 cm3 of 1.00 mol dm–3 HCl B 30 cm3 of 0.90 mol dm–3 HCl C 50 cm3 of 0.40 mol dm–3 HCl D 100 cm3 of 0.30 mol dm–3 HCl

Question

A mixture of 10 cm3 of methane and 10 cm3 of ethane was sparked with an excess of oxygen. After cooling, the residual gas was passed through aqueous potassium hydroxide. All gas volumes were measured at the same temperature and pressure. Which volume of gas was absorbed by the alkali? A 15 cm3 B 20 cm3 C 30 cm3 D 40 cm3

Question

Z is a compound of two elements, X and Y. Element X shows a very large increase between its 5th and 6th ionisation energies. It has the second largest 1st ionisation energy in its group. Element Y shows a very large increase between its 6th and 7th ionisation energies. It has the largest 1st ionisation energy in its group. What is compound Z? A NO2 B PCl 5 C P4O10 D SF6

Question

Which statement about 131 53 I is correct? A A negative ion of 131 53 I contains 53 neutrons and 52 electrons. B A negative ion of 131 53 I contains 53 neutrons and 54 electrons. C A negative ion of 131 53 I contains 78 neutrons and 52 electrons. D A negative ion of 131 53 I contains 78 neutrons and 54 electrons.

Question

When solid aluminium chloride is heated, Al 2Cl 6 is formed. Which bonding is present in Al 2Cl 6? A covalent and coordinate (dative covalent) B covalent only C ionic and coordinate (dative covalent) D ionic only

Question

The structure of the sulfur dioxide molecule is shown. O S O What is the shape of the sulfur dioxide molecule? A linear B non-linear C pyramidal D tetrahedral

Question

What is the density of a sample of fluorine gas at 32 °C and 100 000 Pa? Assume fluorine behaves as an ideal gas under these conditions. A 1.4 g dm–3 B 1.5 g dm–3 C 1.6 g dm–3 D 1.7 g dm–3

Question

The graph shows the boiling points of the hydrogen compounds of Group 16 elements. 100 H 2O boiling point / qC 0 H2Te H2Se H 2S –100 Which statement correctly explains why water does not fit the trend of the other compounds? A There are fewer electrons in the oxygen atoms so there is less shielding of the nuclear charge. B There are strong hydrogen bonds in water but not in the other compounds. C The covalent bonds in water are much stronger than in the other compounds. D The water molecules are smaller and so have stronger van der Waals’ forces.

Question

An energy cycle is shown. CH4 + 2O2 X Y C + 2H2 + 2O2 CO2 + 2H2O Z The energy changes involved are X, Y and Z. The numerical value of energy change Y is either –890 or +890. The numerical value of energy change Z is either –964 or +964. Which of the three values are negative? A X and Z B X only C Y and Z D Y only

Question

For a certain endothermic reaction, the activation energy is numerically equal to twice the enthalpy change of reaction. Which reaction pathway diagram is correct for this reaction? A B energy energy progress of reaction progress of reaction C D energy energy progress of reaction progress of reaction

Question

Sodium chromate(VI), Na2CrO4, is manufactured by heating chromite, FeCr2O4, with sodium carbonate in an oxidising atmosphere. Chromite contains Cr2O42– ions. 2FeCr2O4 + 4Na2CO3 + 3 21 O2 → 4Na2CrO4 + Fe2O3 + 4CO2 What happens in this reaction? A Chromium and iron are the only elements oxidised. B Chromium, iron and carbon are oxidised. C Only chromium is oxidised. D Only iron is oxidised.

Question

Oxygen can be prepared by the reaction of potassium manganate(VII), KMnO4, hydrogen peroxide, H2O2, and sulfuric acid, H2SO4. Each H2O2 molecule loses two electrons in this reaction. The other products of the reaction are potassium sulfate, manganese(II) sulfate and water. How many moles of oxygen gas are produced when 1.0 mol of KMnO4 reacts with an excess of H2O2 in acidic conditions? A 2.0 mol B 2.5 mol C 4.5 mol D 5.0 mol

Question

An alcohol, ROH, reacts reversibly with ethanoic acid to produce an ester. ROH(l) + CH3COOH(l) CH3COOR(l) + H2O(l) 3.0 mol of ROH, 2.0 mol of ethanoic acid and 1.0 mol of water are mixed together. At equilibrium, 1.5 mol of CH3COOR is present. What is the value of the equilibrium constant, Kc, for this reaction? A 0.20 B 0.25 C 2.00 D 5.00

Question

Graphs can be drawn to show the percentage of ammonia at equilibrium when nitrogen and hydrogen are mixed at different temperatures and pressures. Which diagram correctly represents these two graphs? A B 40 40 400 qC 500 qC % NH3 at % NH3 at 20 20 equilibrium equilibrium 500 qC 400 qC 0 0 0 10 20 0 10 20 pressure / 103 kPa pressure / 103 kPa C D 40 500 qC 40 400 qC % NH3 at % NH3 at 20 400 qC 20 500 qC equilibrium equilibrium 0 0 0 10 20 0 10 20 pressure / 103 kPa pressure / 103 kPa

Question

The Boltzmann distribution for the hydrogenation of an alkene at a particular temperature in the absence of a catalyst is shown. proportion of molecules Ea with energy E 0 0 molecular energy E Which row correctly describes the effects of adding a nickel catalyst to the reaction vessel? the shape of the activation energy, Ea Boltzmann distribution A changes decreases B changes increases C does not change decreases D does not change increases

Question

Elements Y and Z are both in Period 3 of the Periodic Table. When the chloride of element Y is added to water, it reacts and a solution of pH 2 is produced. When the chloride of element Z is added to water, it dissolves and a solution of pH 7 is produced. Which statement explains these observations? A Both chlorides hydrolyse in water. B Element Y is magnesium and element Z is sodium. C Element Y is phosphorus and element Z is aluminium. D Element Y is silicon and element Z is sodium.

Question

Aluminium, silicon and phosphorus are elements in Period 3 of the Periodic Table. Each element forms an oxide. Which row is correct? Al 2O3 SiO2 P4O10 A basic amphoteric acidic B giant ionic giant ionic simple molecular C high melting point high melting point low melting point D vigorous reaction with water slight reaction with water vigorous reaction with water

Question

Which statement is correct? A The atomic radius of silicon is larger than that of aluminium. B The boiling point of chlorine is higher than that of silicon. C The first ionisation energy of sulfur is greater than that of phosphorus. D The electrical conductivity of magnesium is greater than that of sodium.

Question

All solubility data in this question is given at the same temperature. The table gives some data for compounds of calcium and for compounds of X, an unidentified element in Group 2. decomposition solubility of sulfate solubility of hydroxide element temperature of / mol per 100 g of water / mol per 100 g of water carbonate / °C Ca 840 4.66 × 10–3 1.53 × 10–3 X 1150 What is the missing data for element X? solubility of sulfate solubility of hydroxide / mol per 100 g of water / mol per 100 g of water A 7.11 × 10–5 2.00 × 10–5 B 7.11 × 10–5 3.37 × 10–3 C 1.83 × 10–1 2.00 × 10–5 D 1.83 × 10–1 3.37 × 10–3

Question

What is the total volume of gas produced, measured at room conditions, when 0.010 mol of anhydrous magnesium nitrate is completely decomposed by heating? A 240 cm3 B 480 cm3 C 600 cm3 D 720 cm3

Question

A solid sodium halide, NaX, is reacted with concentrated sulfuric acid. The lowest oxidation state of sulfur in the products is +4. Halogen Y2 is less volatile than halogen X2. What are the identities of sodium halide NaX and halogen Y2? sodium halide NaX halogen Y2 A sodium bromide chlorine B sodium bromide iodine C sodium iodide bromine D sodium iodide astatine

Question

Compound Q dissolves in water. Q(aq) does not react with dilute sulfuric acid. Q(aq) forms a precipitate when aqueous silver nitrate is added. This precipitate is partially soluble in aqueous ammonia. What could be compound Q? A barium bromide B barium iodide C magnesium bromide D magnesium iodide

Question

Nitrogen dioxide is a gas that contributes to air pollution. It is produced in internal combustion engines. Which statement is correct? A Nitrogen dioxide acts as a catalyst in the atmospheric oxidation of sulfur dioxide to sulfur trioxide. B Nitrogen dioxide reacts to form nitrogen monoxide in the catalytic converter of a car exhaust system. C PAN forms when nitrogen dioxide reacts with the gases formed by complete combustion of the fuel. D Under high pressure in an internal combustion engine, nitrogen dioxide forms from impurities in the fuel.

Question

What is the bond angle in the ammonium ion? A 90° B 107° C 109.5° D 120°

Question

Structural isomerism and stereoisomerism should be taken into account when answering this question. The structure of 3-methylcyclobutene is shown. 3-methylcyclobutene A mixture containing all stereoisomers of 3-methylcyclobutene is treated with HBr. This produces a mixture of isomeric bromomethylcyclobutanes. How many stereoisomers does 3-methylcyclobutene have, and how many isomeric bromomethylcyclobutanes are present in the product mixture? 3-methylcyclobutene bromomethylcyclobutanes A 2 4 B 2 6 C 4 4 D 4 8

Question

The diagram shows the structure of X. X NC H H H Which row is correct? number of type of hybridisation of σ bonds in X the carbon atoms in X A 4 sp and sp2 B 4 sp2 and sp3 C 6 sp and sp2 D 6 sp2 and sp3

Question

The diagram shows the skeletal formula of citric acid. citric acid O OH O O HO OH OH What is the molecular formula of citric acid? A C6H8O7 B C6H4O7 C C8H8O7 D C10H8O7

Question

Which reaction occurs when ethane and chlorine are mixed in diffused sunlight? A a free-radical substitution with hydrogen given off B a free-radical substitution with hydrogen chloride given off C a free-radical substitution with no gas given off D a nucleophilic substitution with hydrogen chloride given off

Question

A molecule of geraniol is shown. geraniol OH What is formed when geraniol is reacted with an excess of cold dilute acidified MnO4–? A B O OH OH HO HO HO HO OH OH O O C D O + O + O O OH OH O OH OH

Question

Q is either a primary or a tertiary halogenoalkane. Q undergoes hydrolysis with aqueous sodium hydroxide. The first step in the mechanism of this reaction involves two species reacting together. Which row is correct? Q behaviour of hydroxide ion A primary halogenoalkane electrophile B primary halogenoalkane nucleophile C tertiary halogenoalkane electrophile D tertiary halogenoalkane nucleophile 31 2-bromopropane is converted to 1,2-dibromopropane in a pathway involving two reactions. reaction 1 reaction 2 2-bromopropane compound X 1,2-dibromopropane What are the reagents and conditions for the two reactions? reaction 1 reaction 2 A heat under reflux with aqueous NaOH HBr(g) at room temperature B heat under reflux with aqueous NaOH Br2(l) at room temperature C heat under reflux with ethanolic NaOH HBr(g) at room temperature D heat under reflux with ethanolic NaOH Br2(l) at room temperature

Question

In the question paper above.

Question

Compound X is a single, pure, optical isomer. Compound X is heated with an excess of concentrated H2SO4. Only one organic product is formed. What is compound X? A B C D OH OH CH2OH HO

Question

Which reagents could be used to form 2-bromobutane from butan-1-ol? A bromine and ultraviolet light B concentrated sulfuric acid with potassium bromide, under reflux C concentrated sulfuric acid followed by bromine D concentrated sulfuric acid followed by hydrogen bromide

Question

X is a non-cyclic ketone with a single carbonyl group and no other functional groups. Ketone X has the following properties. ● When ketone X is treated with NaBH4, the organic product has a Mr 2.3256% greater than the Mr of ketone X. ● Ketone X gives a yellow precipitate with alkaline I2(aq). How many isomeric ketones could be ketone X? A 1 B 2 C 3 D 4

Question

Compound Y: ● changes the colour of acidified K2Cr2O7 from orange to green ● has no effect on Fehling’s reagent ● produces an orange precipitate with 2,4-dinitrophenylhydrazine reagent. What is compound Y? A B C D CH3CCH2C H CH3CCH2CCH3 CH3CCH2CH2OH HOCH2CH2CH2CH2OH O O O O O

Question

The product of the reaction between propanone and hydrogen cyanide is hydrolysed under acidic conditions. What is the formula of the final product? A CH3CH(OH)COOH B CH3CH2CH2COOH C (CH3)2CHCONH2 D (CH3)2C(OH)COOH

Question

P is a carboxylic acid with molecular formula C5H10O2. Carboxylic acid P reacts with an excess of LiAl H4 to form compound Q. Which pairs of molecules could be carboxylic acid P and compound Q? carboxylic acid P compound Q 1 CH3(CH2)3COOH CH3(CH2)3OH 2 CH3(CH2)3COOH CH3(CH2)3CHO 3 (CH3)3CCOOH (CH3)3CCH2OH A 1 and 2 B 1 and 3 C 2 and 3 D 3 only

Question

Compound X is treated with an excess of dilute aqueous potassium hydroxide. X O O What is the structure of the organic product? A B O O – O OH HO OH C D O O – O OH HO OH

Question

A section showing two repeat units of an addition polymer is shown. CH3 CH3 CH3 CH3 C C C C Cl CH3 Cl CH3 What is the identity of the monomer that produced this polymer? A 2-chloro-3-methylbutane B 2-chloro-3-methylbut-2-ene C 2-chloropent-2-ene D 2,4-dichloro-3,3,4,5-tetramethylhexane

Question

The relative atomic mass of antimony is 121.76. Antimony has two isotopes. The mass numbers of the two isotopes differ by two. The isotope with the lower mass number is the more abundant. What is the percentage abundance of the isotope with the higher mass number? A 12% B 38% C 62% D 88% 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 138.9 140.1 140.9 144.4 – 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 – – – – – – – – – – –