Chemistry 9701/11 October/November 2024: question paper and mark scheme

Question

In this question Q is used to represent a halogen atom. Magnesium and calcium each form a compound with chlorine and a compound with bromine. One of these compounds contains: ● the element in Group 2 with the higher first ionisation energy and ● the element in Group 17 with the higher Q–Q bond energy. What is the formula of this compound? A MgCl 2 B MgBr2 C CaCl 2 D CaBr2

Question

Compound X contains two elements, Y and Z. Element Y is in Period 2 of the Periodic Table. In one atom of element Y, the p sub-shell has all three orbitals occupied; only one of these three orbitals is fully occupied. Element Z is in Period 3 of the Periodic Table. In one atom of element Z, the p sub-shell has only two orbitals occupied. What is the formula of compound X? A CCl 4 B SiCl 4 C SiO2 D SO2

Question

Glauber’s salt consists of crystals of hydrated sodium sulfate, Na2SO4•xH2O, which can be used for the manufacture of detergents. When a sample of Glauber’s salt was heated, 1.91 g of water was removed leaving 1.51 g of anhydrous Na2SO4. What is the value of x in Na2SO4•xH2O? A 1 B 8.85 C 10 D 11.25

Question

What contains the greatest number of the named particles? A 6.0 dm3 of argon atoms at room conditions B 6.0 g of carbon dioxide molecules C 6.0 g of magnesium atoms D 6.0 g of water molecules

Question

Phosphorus forms a compound with hydrogen called phosphine, PH3. This compound can react with a hydrogen ion, H+. Which type of interaction occurs between PH3 and H+? A dative covalent bond B dipole–dipole forces C hydrogen bond D ionic bond

Question

The graphs show trends in four physical properties of elements in Period 3, excluding argon. Which graph has electronegativity on the y-axis? A B Na Mg Al Si P S Cl Na Mg Al Si P S Cl C D Na Mg Al Si P S Cl Na Mg Al Si P S Cl

Question

The element tin exists in two forms, grey tin and white tin. Some properties of grey tin and white tin are shown. grey tin white tin boiling point / K 2543 2533 electrical conductivity none in solid or liquid good in solid and liquid malleability brittle malleable Which structural change might take place when grey tin changes to white tin? A giant covalent to giant ionic B giant covalent to giant metallic C giant ionic to giant covalent D giant ionic to giant metallic

Question

Which solid has a simple molecular lattice? A calcium fluoride B nickel C silicon(IV) oxide D sulfur

Question

The standard enthalpy change of combustion of carbon is –394 kJ mol–1. The standard enthalpy change of combustion of hydrogen is –286 kJ mol–1. The standard enthalpy change of formation of butane is –129 kJ mol–1. What is the standard enthalpy change of combustion of butane? A –551 kJ mol–1 B –2877 kJ mol–1 C –3135 kJ mol–1 D –4307 kJ mol–1

Question

Three processes are described. 1 H+(aq) + OH–(aq) → H2O(l) 2 CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) 3 NH3(g) → NH3(l) Which statement is correct? A None of the processes have a positive enthalpy change. B Only process 1 has a positive enthalpy change. C Only process 2 has a positive enthalpy change. D Only process 3 has a positive enthalpy change.

Question

In alkaline solution, MnO4– ions oxidise SO32– ions to SO42– ions. The MnO4– ions are reduced to MnO2. What is the ratio of the two ions in the balanced chemical equation for this reaction? MnO4– SO32– A 2 3 B 3 2 C 4 7 D 7 4

Question

Lithium reacts with nitrogen at room temperature to form solid Li3N. Three vessels of equal volume are connected by taps 1 and 2 as shown. evacuated N2(g) + 3H2(g) 2NH3(g) 1 2 Li At the start, taps 1 and 2 are closed, the left-hand vessel is evacuated, the middle vessel has the indicated reaction at equilibrium and the right-hand vessel contains lithium only. Which action would allow the equilibrium mixture to contain the most ammonia? A Keep both taps 1 and 2 closed. B Open both taps 1 and 2. C Open tap 1 only. D Open tap 2 only.

Question

When 0.20 mol of hydrogen gas and 0.15 mol of iodine gas are heated at 723 K until equilibrium is established, the equilibrium mixture contains 0.26 mol of hydrogen iodide. The equation for the reaction is as follows. H2(g) + I2(g) 2HI(g) What is the correct expression for the equilibrium constant Kc? 2 × 0.26 (2 × 0.26)2 (0.26) 2 (0.26) 2 A B C D 0.20 × 0.15 0.20 × 0.15 0.07 × 0.02 0.13 × 0.13

Question

In acidic conditions, iodine reacts with propanone in a substitution reaction. CH3COCH3(aq) + I2(aq) → CH3COCH2I(aq) + HI(aq) The kinetics of the reaction are investigated using a colorimeter. As the I2 reacts, the yellow / brown colour of the I2(aq) fades to colourless, changing the absorbance of the solution. Known concentrations of I2(aq) are used to prepare a calibration curve graph and the absorbance is then measured as the reaction proceeds. calibration curve using known concentrations of I2(aq) absorbance during reaction 0.30 0.6 0.25 0.5 concentration 0.20 0.4 of iodine 0.15 absorbance 0.3 u 10–3 mol dm–3 0.10 0.2 0.05 0.1 0 0 0 0.1 0.2 0.3 0.4 0.5 0.6 0 20 30 40 50 60 absorbance time / s What is the rate of reaction at 20 s? A 5 × 10–6 mol dm–3 s–1 B 1 × 10–5 mol dm–3 s–1 C 5 × 10–3 mol dm–3 s–1 D 1 × 10–2 mol dm–3 s–1

Question

The diagram shows a Boltzmann distribution curve. The axes are not labelled. point Y point X EA Points X and Y are points on the vertical axis. What is represented by both points X and Y? point X point Y A number of molecules largest number of molecules with energy equal to EA with the same energy B number of molecules with largest number of molecules energy equal to or greater than EA with the same energy C number of molecules the amount of energy of the with energy equal to EA greatest number of molecules D number of molecules with the amount of energy of the energy equal to or greater than EA greatest number of molecules

Question

What are the acid–base nature and structure of SO2? acid–base nature structure A acidic giant covalent lattice B acidic simple molecular C basic giant covalent lattice D basic simple molecular

Question

Elements X and Y are in Period 3 of the Periodic Table. Element X is either phosphorus or sulfur. Element Y is either sodium or magnesium. Element X forms an oxide that reacts with water to give a solution containing the aqueous anion XO42–. One mole of element Y reacts with one mole of chlorine molecules. At the end of the reaction, all of the element Y and all of the chlorine molecules have been used up. What are elements X and Y? X Y A phosphorus sodium B phosphorus magnesium C sulfur sodium D sulfur magnesium

Question

Q is a semi-conductor. The chloride of Q reacts with water to form white fumes and an acidic solution. Which Period 3 element is Q? A magnesium B aluminium C silicon D phosphorus

Question

V and W are two compounds. Each one contains a different Group 2 element. A sample of each solid is added to water, shaken, and the pH of the resulting solution is measured. compound V W pH 13.6 9.4 Which row could identify V and W? V W A BaSO4 MgSO4 B MgSO4 BaSO4 C Ba(OH)2 Mg(OH)2 D Mg(OH)2 Ba(OH)2

Question

Compound L decomposes on heating. One of the products is gas M. M reacts with unburned hydrocarbons to form peroxyacetyl nitrate, PAN. What could be the formula of L? A CaNO3 B Ca(NO3)2 C MgCO3 D Mg(CO3)2

Question

In reaction 1, concentrated sulfuric acid is added to potassium chloride and the fumes produced are bubbled into aqueous potassium iodide solution. In reaction 2, potassium chloride is dissolved in aqueous ammonia and this is then added to aqueous silver nitrate. What are the observations for reactions 1 and 2? observation for observation for reaction 1 reaction 2 A brown solution colourless solution B brown solution white precipitate C colourless solution colourless solution D colourless solution white precipitate

Question

The table refers to the hydrogen halides. Which row is correct? oxidation thermal stability A easier to oxidise down the group increases down the group B more difficult to oxidise down the group increases down the group C easier to oxidise down the group decreases down the group D more difficult to oxidise down the group decreases down the group 23 7.5 g of nitrogen monoxide reacts with 7.0 g of carbon monoxide on the surface of the catalytic converter in the exhaust system of a car. What is the total volume of the product gases measured at room conditions? A 3.0 dm3 B 6.0 dm3 C 9.0 dm3 D 12.0 dm3

Question

In the question paper above.

Question

Three statements about ammonia molecules and ammonium ions are given. 1 In aqueous solution, ammonia molecules form coordinate bonds with hydroxide ions. 2 Ammonium ions are Brønsted–Lowry acids. 3 The H–N–H bond angle is larger in the ammonium ion than in the ammonia molecule. Which statements are correct? A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3

Question

Ethene reacts with steam in the presence of sulfuric acid. C2H4 + H2O → CH3CH2OH Which type of reaction is this? A acid–base B addition C hydrolysis D substitution

Question

Compound Z has the molecular formula C4H8O2. Compound Z reacts with propan-1-ol in the presence of concentrated H2SO4. The diagram shows the skeletal formulae of three compounds, S, T and U. S T U O O O O O O What are the possible skeletal formulae of the products of the reaction between compound Z and propan-1-ol? A S and T B U only C S and U D T only

Question

Geraniol and nerol are isomers of each other. geraniol nerol CH3 CH3 C CH2OH C H H 2C C H 2C C H CH2OH H 3C H2C H 3C H 2C C C C C H 3C H H 3C H Which type of isomerism is shown here? A chain B geometrical (cis / trans) C optical D positional

Question

Which compound has the greatest number of stereoisomers? A 2-methylhex-2-ene B 3-methylhex-2-ene C 4-methylhex-2-ene D 5-methylhex-2-ene

Question

Vitamin A contains retinol. retinol OH Under appropriate conditions, acidified KMnO4(aq) can be used to break C=C bonds. After these bonds have been broken, further oxidation of the fragments may occur. Under which conditions is the acidified KMnO4(aq) used and what do the final oxidation products include? conditions final oxidation products A cold, dilute aldehydes and carboxylic acids B cold, dilute ketones and carboxylic acids C hot, concentrated aldehydes and carboxylic acids D hot, concentrated ketones and carboxylic acids

Question

The structure of limonene is shown. limonene What are the number of moles of carbon dioxide and water produced when a sample of limonene is completely combusted in oxygen? number of moles number of moles of carbon dioxide of water A 4 3 B 5 4 C 5 8 D 9 7

Question

The reaction of chlorine with methane is carried out in the presence of light. What is the function of the light? A to break the C–H bonds in methane B to break the chlorine molecules into atoms C to break the chlorine molecules into ions D to heat the mixture

Question

When X is added to NaOH(aq) and heated under reflux, pentan-2-ol is made. Which organic product is made when X is heated with a solution of KCN dissolved in ethanol? A B C D CN CN CN CN 33 1-chlorobutane and 1-iodobutane both react with aqueous sodium hydroxide by a nucleophilic substitution mechanism. Which reaction has the greatest rate under the same conditions and which mechanism is followed by this reaction? greatest rate mechanism A 1-chlorobutane SN1 B 1-chlorobutane SN2 C 1-iodobutane SN1 D 1-iodobutane SN2

Question

In the question paper above.

Question

Compound Y reacts with alkaline I2(aq). When the products of this reaction are acidified, a dicarboxylic acid is produced. The formula of the dicarboxylic acid is HOOC–R–COOH where R consists of one or more CH2 groups. Which compound is Y? A pentan-1,4-diol B pentan-1,5-diol C pentan-2,3-diol D pentan-2,4-diol

Question

Which alcohol gives only one possible oxidation product when warmed with dilute acidified potassium dichromate(VI)? A butan-1-ol B butan-2-ol C 2-methylpropan-1-ol D 2-methylpropan-2-ol

Question

Which compound, on reaction with hydrogen cyanide, produces a compound with a chiral centre? A CH3CHO B CH3CH2COCH2CH3 C CH3CO2CH3 D HCHO

Question

The diagram shows three reactions of ethanal. In each case, an excess of ethanal is used. solid 2 alkaline I2(aq) heat acidified K2Cr2O7 ethanal Fehling’s solution solution 1 solid 3 heat CH3CHO boil Observations are made after each of the three reactions. What are the colours of solution 1 and solids 2 and 3? solution 1 solid 2 solid 3 A green yellow silver mirror B green yellow red C orange red silver mirror D orange red red

Question

(CH3)3CCN reacts to form alcohol Y via the reaction sequence shown. H+(aq) LiAl H4 (CH3)3CCN X alcohol Y reaction 1 reaction 2 Which row names the molecule X and the class of alcohol Y? name of molecule X class of alcohol Y A 2,2-dimethylbutanoic acid primary B 3,3-dimethylbutanoic acid tertiary C dimethylpropanoic acid primary D dimethylpropanoic acid tertiary

Question

The diagram shows a section of an addition polymer. The polymer is made using two different monomers. H Cl H CH3 H Cl H CH3 C C C C C C C C C Cl CH3 CH3 Cl Cl CH3 CH3 Cl Cl CH3 What are the names of the two monomers needed to make this polymer? A 1,2-dichloropropene and 2-chlorobut-2-ene B 2,3-dichlorobut-2-ene and chloropropene C 1,2-dichloropropene and chloroethene D chloropropene and 2-chlorobut-2-ene

Question

The diagram shows the mass spectrum of a sample of chlorine. Peaks V, W, X, Y and Z are labelled. 100 X V 80 Y 60 relative intensity 40 W 20 Z 0.0 30 40 50 60 70 80 m/e Which statements about this spectrum are correct? 1 The relative atomic mass of chlorine can be calculated from the abundances and m / e values of 2 of the 5 peaks. 2 37.0 g of the species responsible for peak Z contains 3.011 × 1023 molecules. 3 The relative molecular mass of chlorine can be calculated from the abundances and m / e values of peaks X, Y and Z. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 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 – – – – – – – – – – –