Chemistry 0620/41 May/June 2023: question paper and mark scheme

Question

Some symbol equations and word equations, A to J, are shown. A Fe3+ + 3OH– → Fe(OH)3 B H+ + OH– → H2O C ethane + chlorine → chloroethane + hydrogen chloride D C12H26 → C8H18 + C4H8 E ethene + steam → ethanol F chlorine + aqueous potassium iodide → iodine + aqueous potassium chloride G C6H12O6 → 2C2H5OH + 2CO2 H ethanoic acid + ethanol → ethyl ethanoate + water I calcium carbonate → calcium oxide + carbon dioxide J 6CO2 + 6H2O → C6H12O6 + 6O2 Use the equations to answer the questions that follow. Each equation may be used once, more than once, or not at all. Give the letter, A to J, for the equation that represents: [Total: 6]

Question

(a) The symbols of the elements in Period 2 of the Periodic Table are shown. Li Be B C N O F Ne Use the symbols of the elements in Period 2 to answer the questions that follow. Each symbol may be used once, more than once or not at all. Give the symbol of the element that: (vi) (b) Boron, B, has two isotopes. (i) State the meaning of the term isotopes. . …… . …… [2] (ii) Table 2.1 shows the relative masses and the percentage abundances of the two isotopes of boron. Table 2.1 relative mass of isotope percentage abundance of isotope 10 20 11 80 Calculate the relative atomic mass of boron to one decimal place. relative atomic mass = …… [2] [Total: 10]

Question

This question is about ionic and covalent compounds. (a) (i) Sodium reacts with oxygen to form the ionic compound sodium oxide. The electronic configurations of an atom of sodium and an atom of oxygen are shown in Fig. 3.1. sodium atom oxygen atom Na O Fig. 3.1 Ions are formed by the transfer of electrons from sodium atoms to oxygen atoms. Complete the dot-and-cross diagrams in Fig. 3.2 to show the electronic configuration of one sodium ion and one oxide ion. Show the charges on the ions. sodium ion oxide ion Na O Fig. 3.2 [3] (ii) Write the formula of sodium oxide. . …… [1] (b) Carbon dioxide, CO2, is a covalent compound. Complete the dot-and-cross diagram in Fig. 3.3 to show the electronic configuration in a molecule of carbon dioxide. Show outer shell electrons only. O C O Fig. 3.3 [2] (c) The melting points of sodium oxide and carbon dioxide are shown in Table 3.1. Table 3.1 melting point / °C sodium oxide 1275 carbon dioxide –78 (i) Explain, in terms of bonding, why sodium oxide has a high melting point. . …… . …… . …… . …… [2] (ii) Carbon dioxide has a low melting point. State the general term for the weak forces that cause carbon dioxide to have a low melting point. . …… [1] [Total: 9]

Question

Oxygen is produced by the decomposition of aqueous hydrogen peroxide. Manganese(IV) oxide, MnO2, is a catalyst for this reaction. (a) State the meaning of the term catalyst. . …… . …… [2] (b) A student adds powdered manganese(IV) oxide to aqueous hydrogen peroxide in a conical flask as shown in Fig. 4.1. The mass of the conical flask and its contents is measured at regular time intervals. The mass decreases as time increases. loosely fitting cotton wool plug aqueous hydrogen peroxide powdered manganese(IV) oxide (catalyst) balance Fig. 4.1 (i) State why the mass of the conical flask and its contents decreases as time increases. . …… [1] (ii) The rate of reaction is highest at the start of the reaction. The rate decreases and eventually becomes zero. Explain why the rate of reaction is highest at the start of the reaction. . …… . …… [1] (iii) Explain why the rate of reaction eventually becomes zero. . …… . …… [1] (c) The experiment is repeated at an increased temperature. All other conditions stay the same. Explain in terms of collision theory why the rate of reaction is higher at an increased temperature. . …… . …… . …… . …… [3] (d) The equation for the decomposition of aqueous hydrogen peroxide, H2O2(aq), is shown. 2H2O2(aq) → 2H2O(l) + O2(g) 50.0 cm3 of a 0.200 mol / dm3 solution of H2O2(aq) is used. Calculate the mass of O2 that forms. Use the following steps. ● Calculate the number of moles of H2O2 used. …… mol ● Determine the number of moles of O2 produced. …… mol ● Calculate the mass of O2 produced. …… g [3] (e) State the effect on the mass of oxygen produced if the mass of powdered manganese(IV) oxide catalyst is increased. . …… [1] (f) Oxygen can also be produced by the decomposition of mercury(II) oxide, HgO. The only products of this decomposition are mercury and oxygen. Write a symbol equation for this decomposition. . …… [2] [Total: 14]

Question

This question is about electricity and chemical reactions. (a) The electrolysis of concentrated aqueous potassium bromide using graphite electrodes forms: ● hydrogen at the cathode ● bromine at the anode. The electrolyte becomes aqueous potassium hydroxide. (i) State what is meant by the term electrolysis. . …… . …… [2] (ii) State why graphite is suitable for use as an electrode. . …… [1] (iii) Write an ionic half-equation for the formation of hydrogen at the cathode. . …… [2] (iv) Name the type of particle responsible for the transfer of charge in the conducting wires. . …… [1] (v) Name the type of particle responsible for the transfer of charge in aqueous potassium bromide. . …… [1] (vi) State the names of the products formed when electricity is passed through dilute aqueous potassium bromide using graphite electrodes. at the anode . …… at the cathode. …… [2] (b) Bauxite is an ore containing aluminium. Aluminium is extracted by electrolysis of purified bauxite in molten cryolite using carbon electrodes. (i) Name the aluminium compound in purified bauxite. . …… [1] (ii) State two reasons why cryolite is used in this electrolysis. 1 . …… 2 . …… [2] (iii) The anode is made from carbon. Explain why the carbon anode has to be replaced regularly. . …… . …… [1] (c) Hydrogen–oxygen fuel cells can be used to produce electricity in vehicles. (i) Write the symbol equation for the overall reaction in a hydrogen–oxygen fuel cell. . …… [2] (ii) State one advantage of using hydrogen–oxygen fuel cells instead of petrol in vehicle engines. . …… [1] [Total: 16]

Question

This question is about sulfur and compounds of sulfur. Sulfur is converted into sulfuric acid, H2SO4, by the Contact process. The process involves four stages. stage 1 Molten sulfur is converted into sulfur dioxide. stage 2 Sulfur dioxide reacts with oxygen to form sulfur trioxide. stage 3 Sulfur trioxide combines with concentrated sulfuric acid to form oleum, H2S2O7. stage 4 Oleum reacts to form concentrated sulfuric acid. (a) (i) In stage 1, iron pyrites, FeS2, can be used instead of molten sulfur. The iron pyrites is heated strongly in air. Balance the equation for the reaction occurring when iron pyrites reacts with oxygen in the air. ……FeS2 + ……O2 → ……Fe2O3 + ……SO2[1] (ii) Name Fe2O3. Include the oxidation number of iron. . …… [1] (b) The equation for stage 2 is shown. 2SO2(g) + O2(g) 2SO3(g) The forward reaction is exothermic. The reaction is carried out at a temperature of 450 °C and a pressure of 2 atm. Using explanations that do not involve cost: (i) explain why a temperature greater than 450 °C is not used . …… . …… [1] (ii) explain why a pressure lower than 2 atm is not used. . …… . …… [1] (c) When sulfuric acid reacts with ammonia the salt produced is ammonium sulfate. Write the symbol equation for this reaction. . …… [2] (d) Lead(II) sulfate is an insoluble salt. Lead(II) sulfate can be made from aqueous ammonium sulfate using a precipitation reaction. (i) Name a solution that can be added to aqueous ammonium sulfate to produce a precipitate of lead(II) sulfate. . …… [1] (ii) Write an ionic equation for this precipitation reaction. Include state symbols. . …… [3] (iii) The precipitate of lead(II) sulfate forms in an aqueous solution. Describe how pure lead(II) sulfate can be obtained from the mixture. . …… . …… . …… [3] [Total: 13]

Question

This question is about organic compounds. (a) Butane reacts with chlorine in a photochemical reaction. C4H10 + Cl 2 → C4H9Cl + HCl (i) State the meaning of the term photochemical. . …… [1] (ii) An organic compound with the formula C4H9Cl is formed when one molecule of butane reacts with one molecule of chlorine. Draw the displayed formulae of two possible structural isomers with the formula C4H9Cl formed in this reaction. [2] (b) The structure of compound A is shown in Fig. 7.1. COOH H C C H CH2OH Fig. 7.1 (i) Deduce the molecular formula of compound A. . …… [1] (ii) There are three functional groups in compound A. Name the homologous series of compounds that contain the following functional groups: –C=C– …… –OH …… –COOH. . …… [3] (iii) State what is observed when compound A is added to: aqueous bromine . …… aqueous sodium carbonate. …… [2] (iv) Compound A can be used as a single monomer to produce two different polymers. Draw one repeat unit of the addition polymer formed from compound A. [2] (v) Compound A can be converted into a dicarboxylic acid. Name the type of condensation polymer formed from a dicarboxylic acid and a diol. . …… [1] [Total: 12] The Periodic Table of Elements Group I II III IV V VI VII VIII 1 2 H He hydrogen helium Key 1 4 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 7 9 relative atomic mass 11 12 14 16 19 20 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 24 27 28 31 32 35.5 40 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 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 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 16 85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131 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 133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – – 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 139 140 141 144 – 150 152 157 159 163 165 167 169 173 175 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 – 232 231 238 – – – – – – – – – – – The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).