Chemistry 9701/11 October/November 2022: question paper and mark scheme

Question

Which sample contains the same number of the named species as the number of molecules in 35.5 g of chlorine? A atoms in 16 g of sulfur B atoms in 23 g of sodium C ions in 74.5 g of potassium chloride D molecules in 88 g of carbon dioxide

Question

Mixture R consists of one mole of C3H6 and one mole of C4H6. What is the minimum number of moles of oxygen molecules needed for complete combustion of mixture R? A 6.5 B 7 C 10 D 20

Question

Which statement about the electrons in a ground state carbon atom is correct? A Electrons are present in four different energy levels. B There are more electrons in p orbitals than there are in s orbitals. C The occupied orbital of highest energy is spherical. D The occupied orbital of lowest energy is spherical.

Question

For the element sulfur, which pair of ionisation energies has the largest difference between them? A third and fourth ionisation energies B fourth and fifth ionisation energies C fifth and sixth ionisation energies D sixth and seventh ionisation energies

Question

How many σ bonds are present in one H–C≡C–C(CH3)=CH(CH3) molecule? A 5 B 11 C 13 D 16

Question

Which molecule has an equal number of bonding electrons and lone-pair electrons? A BH3 B CO2 C F2O D SO2

Question

The table shows properties of four solids held together by different types of bonding. Which row correctly describes the properties of a solid with a giant covalent structure? solubility in melting point polar solvents A high insoluble B high soluble C low insoluble D low soluble

Question

The carbonate of an s-block element is reacted with an excess of hydrochloric acid. 0.833 g of the carbonate releases 200 cm3 of gas, measured under room conditions. What is the identity of the metal carbonate? A Na2CO3 B K2CO3 C MgCO3 D CaCO3

Question

The enthalpy changes of formation, , of both PCl 3 and PCl 5 are exothermic. PCl 3 reacts with chlorine. PCl 3(l) + Cl 2(g) → PCl 5(s) = –124 kJ mol–1 Which pair of statements is correct? statement 1 statement 2 A is less negative than The Cl 2 bond energy is needed in calculating (PCl 5). from enthalpies of formation. B is more negative than The Cl 2 bond energy is needed in calculating (PCl 5). from enthalpies of formation. C is less negative than The Cl 2 bond energy is not needed in calculating (PCl 5). from enthalpies of formation. D is more negative than The Cl 2 bond energy is not needed in calculating (PCl 5). from enthalpies of formation.

Question

A student mixes 25.0 cm3 of 0.350 mol dm–3 sodium hydroxide solution with 25.0 cm3 of 0.350 mol dm–3 hydrochloric acid. The temperature increases by 2.5 °C. No heat is lost to the surroundings. The final mixture has a specific heat capacity of 4.2 J cm–3 K–1. What is the molar enthalpy change for the reaction? A –150 kJ mol–1 B –60 kJ mol–1 C –30 kJ mol–1 D –0.15 kJ mol–1

Question

Ammonium ions are converted into nitrate ions by bacteria. What is the change in the oxidation number of nitrogen? A –6 B +6 C +8 D +9

Question

Sodium dichromate(VI), Na2Cr2O7, reacts with hydrogen peroxide, H2O2, producing Cr3+ ions, water and oxygen. What is the correctly balanced ionic equation for this reaction? A Cr2O72– + 2H+ + H2O2 → 2Cr3+ + 2H2O + 4O2 B Cr2O72– + 8H+ + 3H2O2 → 2Cr3+ + 7H2O + 3O2 C Cr2O72– + 8H+ + 6H2O2 → 2Cr3+ + 10H2O + 6O2 D Cr2O72– + 14H+ + 3H2O2 → 2Cr3+ + 7H2O + 3O2

Question

In which equilibrium reaction is the position of equilibrium moved to the right-hand side by increasing the temperature and also by decreasing the pressure? A H2(g) + CO2(g) H2O(g) + CO(g) ∆H = 40 kJ mol–1 B N2O4(g) 2NO2(g) ∆H = 58 kJ mol–1 C 2SO2(g) + O2(g) 2SO3(g) ∆H = –197 kJ mol–1 D 2HI(g) H2(g) + I2(g) ∆H = –10 kJ mol–1

Question

Ethanol is produced industrially by reacting ethene and steam. C2H4(g) + H2O(g) C2H5OH(g) Kp has a value of 1.8 × 10–5 and the partial pressures of the reactants at equilibrium are shown. partial pressure reactant / kPa ethene 4.8 × 103 steam 2.8 × 103 Which row is correct? partial pressure of ethanol at units of Kp equilibrium / kPa A 2.42 × 102 kPa–1 B 2.42 × 102 kPa C 7.47 × 1011 kPa–1 D 7.47 × 1011 kPa

Question

A large excess of magnesium ribbon is added to dilute hydrochloric acid and the volume of hydrogen gas produced is measured as the reaction proceeds. The reaction is exothermic. The results are shown. R total volume Q / cm3 P time / s Which row explains the changes in the rate of reaction between points P and Q and between points Q and R? between points P and Q between points Q and R A the reaction temperature is increasing the acid concentration is falling B the reaction temperature is increasing the magnesium has been used up C magnesium’s surface area is decreasing the acid concentration is falling D magnesium’s surface area is decreasing the magnesium has been used up

Question

Measurements are made to determine the activation energy, Ea, of a reaction. The diagram shows Ea on the Boltzmann distribution at temperature T1. number of molecules 0 0 Ea energy Measurements are then made at a higher temperature, T2. Which diagram correctly shows the Boltzmann distribution and Ea at T2? A B number of number of molecules molecules 0 0 0 Ea 0 Ea energy energy C D number of number of molecules molecules 0 0 0 Ea 0 Ea energy energy

Question

The electrical conductivities of two compounds, Y and Z, are shown. for Y for Z conductivity of the compound good does not in the liquid state conduct conductivity of the mixture obtained good good by adding the compound to water What are compounds Y and Z? Y Z A Al 2O3 SiCl 4 B NaCl Al 2O3 C NaCl SiCl 4 D SiCl 4 Al 2O3

Question

Which row describes the relative sizes of the ionic radii of Na+, Mg2+ and S2–? smallest largest A Na+ Mg2+ S2– B Mg2+ Na+ S2– C S2– Na+ Mg2+ D S2– Mg2+ Na+

Question

The oxides BaO, CaO, MgO and SrO all produce alkaline solutions when added to water. Which oxide produces the saturated solution with the highest pH? A BaO B CaO C MgO D SrO

Question

Which row is correct? the temperature needed to the solubility of decompose Group 2 metal nitrates Group 2 sulfates A decreases down the group decreases down the group B decreases down the group increases down the group C increases down the group increases down the group D increases down the group decreases down the group

Question

Which statement about Group 17 elements and compounds is correct? A Sodium chloride produces chlorine when reacted with concentrated sulfuric acid. B Sodium chloride produces chlorine when reacted with bromine. C Sodium bromide produces bromine when reacted with concentrated sulfuric acid. D Sodium bromide produces bromine when reacted with iodine in aqueous potassium iodide.

Question

Chlorine is bubbled through 100 cm3 of hot 4.0 mol dm–3 sodium hydroxide until the reaction is complete. 6NaOH(aq) + xCl 2(aq) → yNaCl (aq) + zNaCl O3(aq) + 3H2O(l) Which row is correct? [Na+](aq) after x reaction / mol dm–3 A 3 4.0 B 3 less than 4.0 C 6 4.0 D 6 less than 4.0

Question

Which statement about ammonia or the ammonium ion is correct? A Ammonia gas is produced when an aqueous solution containing the ammonium ion is reacted with a strong acid. B Silver iodide is soluble in a concentrated aqueous solution of ammonia. C The ammonium ion has the same number of electrons as a methane molecule. D The square planar ammonium ion contains a dative covalent bond.

Question

Sulfur dioxide can be catalytically oxidised by an oxide of nitrogen in the atmosphere. Which reaction shows how the catalyst is reformed? A N2 + 2O2 2NO2 B 4NH3 + 5O2 → 4NO + 6H2O C N2 + O2 → 2NO D NO + 1 O 2 2 → NO2

Question

Separate 1.0 g samples of Na2O, MgO, Al 2O3, SiO2, NaCl, MgCl 2, Al 2Cl 6 and SiCl 4 are added to separate beakers containing water and stirred. The number of beakers containing a white solid is Q. An excess of NaOH(aq) is then added to each beaker and stirred. The number of beakers now containing a white solid is R. Which row is correct? Q R A 3 2 B 3 3 C 4 3 D 4 4

Question

Which pair of alcohols are isomers of each other? A butan-1-ol and 2,2-dimethylpropan-1-ol B butan-2-ol and 2-methylpropan-2-ol C pentan-1-ol and 2-methylpropan-2-ol D propan-2-ol and 2-methylpropan-2-ol

Question

How many chiral carbon atoms are there in one molecule of 2,2,4,5-tetramethylhexan-3-ol? A 1 B 2 C 3 D 4

Question

Which pair of reagents react together in a redox reaction? A CH3CHCH2 + Br2 B CH3CH2CH2OH + concentrated H3PO4 C CH3COCH3 + HCN D HCO2C2H5 + dilute H2SO4

Question

The structure of santonin is shown. santonin CH3 O CH3 CH3 O O Santonin is first treated with warm dilute H2SO4. The product of this reaction is treated with cold dilute acidified KMnO4. A final product, Q, is obtained. How many atoms of hydrogen in each molecule of product Q will react with sodium metal? A 2 B 4 C 5 D 6

Question

Compound R can be formed from 1-bromopropane using a nucleophilic substitution reaction followed by an oxidation reaction. What is the identity of R? A propanoic acid B propanone C propylamine D propyl ethanoate

Question

Three colourless liquids with the following formulae are contained in separate unlabelled bottles. CH3CH2CO2H CH3CH(OH)CO2H CH3COCO2H Which two tests, carried out on separate samples of each liquid, will successfully identify each liquid? test 1 test 2 A NaHCO3 2,4-DNPH reagent B NaHCO3 Tollens’ reagent C warm acidified dichromate 2,4-DNPH reagent D warm acidified dichromate Tollens’ reagent

Question

An alcohol, X, reacts with a dicarboxylic acid, Y, to form a double ester, Z. The diagram shows the structure of the ester. Z O O O O Which row about the reactants forming ester Z is correct? the class of the shape of alcohol X the ring in Y A secondary non-planar B secondary planar C tertiary non-planar D tertiary planar

Question

W reacts with alkaline I2(aq) to form a yellow precipitate and CH3CH2CO2– ions. Which row identifies W and the yellow precipitate? identity of identity of W yellow precipitate A butanone CHI3 B butanone CH3I C propanone CHI3 D propanone CH3I

Question

Ethanal reacts with hydrogen cyanide in the presence of KCN to produce a hydroxynitrile. What is the first step in the mechanism of this reaction? A B C D G– G– G– G– O O O O H+ G+ C CN– G+ C G+ C G+ C H 3C H H3C H H 3C H H3C H – CN CN–

Question

Structural isomerism and stereoisomerism should be considered when answering this question. How many isomeric compounds with molecular formula C5H6O4 contain two –CO2H groups and one C=C double bond? A 5 B 6 C 7 D 8

Question

Compound X reacts with ethanoic acid in the presence of an H+ catalyst to produce the compound shown. O H H O H 3C C C C O C CH3 H H What is the molecular formula of compound X? A C2H4O B C2H6O2 C C4H8O D C4H8O2 37 2-bromopropane reacts with hot ethanolic sodium hydroxide. Which substance is the major product of this reaction? A propan-1-ol B propan-2-ol C 2-hydroxypropene D propene

Question

In the question paper above.

Question

Which compounds can be used to make Y in a single-step reaction? Y O OH 1 propanenitrile 2 ethanenitrile 3 propyl ethanoate 4 ethyl propanoate A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Question

The monomer buta-1,3-diene can undergo addition polymerisation in various ways. Two of the polymers that can be made are called cis-poly(buta-1,3-diene) and trans-poly(buta-1,3-diene). In these names cis and trans have their usual meanings. What is the structure of the repeat unit of cis-poly(buta-1,3-diene)? A B C D n n n n

Question

In the mass spectrum of a compound, Z, the relative abundances of the M and M+1 peaks are in the ratio 13 : 1. What is compound Z? A butyl butanoate B hexan-3-one C 2,2,3-trimethylhexane D 3,3-dimethylpentan-1-ol 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 at www.cambridgeinternational.org after the live examination series. 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 16 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 – – – – – – – – – – – Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge