Chemistry 0620/32 May/June 2020: question paper and mark scheme

Question

(a) A list of symbols and formulae is shown. CH4 Cl – CO2 Cr3+ Cu2+ Fe2+ H2 K+ N2 O2 SO2 Answer the following questions about these symbols and formulae. Each symbol or formula may be used once, more than once or not at all. Which symbol or formula represents: (i) a compound produced by the thermal decomposition of calcium carbonate . …… [1] (ii) an element which is used as a fuel . …… [1] (iii) a gas which forms 78% of clean dry air . …… [1] (iv) an ion which forms a blue precipitate when added to aqueous sodium hydroxide . …… [1] (v) an ion formed when an atom gains an electron? . …… [1] (b) Complete the table to show the relative charge and approximate relative mass of a proton, a neutron and an electron. type of approximate relative charge particle relative mass proton 1 neutron electron –1 [3] (c) Deduce the number of electrons and neutrons in an atom of the isotope of potassium shown. 19K 41 number of electrons . …… number of neutrons …… [2] [Total: 10]

Question

A solution is obtained by filtering a mixture of soil and water. The table shows the mass of some of the ions in 1000 cm3 of this solution. mass of ion in 1000 cm3 name of ion formula of ion of soil solution / mg aluminium Al 3+ 0.2 NH4+ 22.0 calcium Ca 2+ 0.2 iron(II) Fe2+ 79.0 magnesium Mg2+ 0.1 nitrate NO3– 28.0 phosphate PO43– 14.0 potassium K+ 39.0 SO42– 5.1 (a) Answer these questions using the information in the table. (i) Which negative ion has the lowest concentration? . …… [1] (ii) State the name of the SO42– ion. . …… [1] (iii) Calculate the mass of nitrate ions in 200 cm3 of this solution. mass = …… mg [1] (iv) Name the compound that contains NH4+ ions and NO3– ions. . …… [1] (b) Describe a chemical test for calcium ions. test . …… observations …… [2] (c) The names and formulae for some compounds are shown. aluminium nitrate, Al (NO3)3 magnesium nitrate, Mg(NO3)2 sodium nitrate, NaNO3 Deduce the formula for calcium nitrate. . …… [1] [Total: 7]

Question

Many compounds have important uses. (a) Complete the table to show the name, number of atoms in the formula and use. name of number of atoms formula use compound in the formula hydrogen = 2 water H 2O oxygen = 1 sulfur = 1 SO2 oxygen = 2 calcium = …… calcium hydroxide oxygen = …… Ca(OH)2 (slaked lime) hydrogen = …… [5] (b) The table compares the reactions of four metals with steam. metal reaction with steam copper does not react magnesium reacts rapidly sodium reacts explosively zinc reacts slowly when warmed Put the four metals in order of their reactivity. Put the least reactive metal first. least reactive most reactive [2] (c) Sodium reacts with molten sodium hydroxide. Complete the chemical equation for this reaction. 2Na + ……NaOH → ……Na2O + H2[2] [Total: 9]

Question

The properties of the first four Group I elements are shown in the table. density melting point boiling point element in g / cm3 / °C / °C lithium 0.53 181 1342 sodium 0.97 98 883 potassium 0.86 63 760 rubidium 39 686 (a) Answer these questions using only the information in the table. (i) Describe the general trend in the boiling points of the Group I elements. . …… [1] (ii) Explain why it is difficult to predict the density of rubidium. . …… . …… [1] (iii) Deduce the state of rubidium at 45 °C. Explain your answer. . …… . …… [2] (b) When sodium reacts with carboxylic acids, hydrogen is produced. (i) Describe a test for hydrogen. test …… observations …… [2] (ii) The structure of a carboxylic acid is shown. H H H H O H H C C C C C H H H H O Deduce the formula of this carboxylic acid to show the number of atoms of carbon, hydrogen and oxygen. . …… [1] (c) Universal indicator is added to an aqueous solution of sodium oxide. ●● What colour change is observed? from green to …… ●● Give a reason for your answer. . …… . …… [2] [Total: 9]

Question

Molten magnesium bromide is electrolysed. The incomplete apparatus is shown. – + (a) (i) Complete the diagram by: ●● labelling the anode and cathode ●● adding the power supply and connecting wires. [2] (ii) Predict the products of this electrolysis at the: positive electrode . …… negative electrode. …… [2] (b) The electrodes must be able to conduct electricity. (i) Give one other property that the electrodes must have. . …… [1] (ii) Name a suitable element that can be used as an electrode. . …… [1] (c) Aqueous chlorine reacts with aqueous magnesium bromide. Cl 2 + MgBr2 → Br2 + MgCl 2 (i) How does this reaction show that chlorine is more reactive than bromine? . …… [1] (ii) What colour is bromine in aqueous solution? . …… [1] (d) Complete the chemical equation for the reaction of chlorine with phosphorus. ……Cl 2 + 2P → ……PCl 5[2] [Total: 10]

Question

Acids have characteristic properties. (a) Hydrochloric acid reacts with magnesium carbonate. Name the products of this reaction and give the observations. . …… . …… . …… . …… . …… [4] (b) The rate of reaction of iron with sulfuric acid can be determined by measuring the time taken to produce 20 cm3 of hydrogen. A student measured the time taken to produce 20 cm3 of hydrogen using three different concentrations of sulfuric acid. In each experiment the student used: ●● 1 g of iron powder ●● the same temperature ●● the same volume of sulfuric acid. The results are shown in the table. concentration of acid time in mol / dm3 /s 0.1 33 0.2 17 0.5 8 (i) Use the information in the table to describe how the rate of reaction changes with the concentration of sulfuric acid. . …… [1] (ii) Describe the effect of each of the following on the rate of this reaction with 0.5 mol / dm3 of sulfuric acid. ●● Larger pieces of iron are used. All other conditions stay the same. . …… ●● The temperature is increased. All other conditions stay the same. . …… [2] (c) Heat is given out when iron reacts with sulfuric acid. What term describes a reaction which gives out heat? . …… [1] (d) The reaction of iron with steam is shown. 3Fe + 4H2O → Fe3O4 + 4H2 How does this equation show that iron gets oxidised? . …… . …… [1] (e) Rust contains hydrated iron(III) oxide. Describe and explain one method of preventing iron from rusting. . …… . …… [2] [Total: 11]

Question

The structure of nerol is shown. H H H C H H C H H H H H H C C C C H H C C C C O H H H H H (a) Draw a circle around the alcohol functional group on the structure of nerol. [1] (b) What feature of the nerol molecule shows that it is an unsaturated compound? . …… [1] (c) Nerol can be extracted from some plants. Crushed plant leaves containing nerol are mixed with an organic solvent called octane. Nerol dissolves in octane. (i) Describe how you would separate the crushed plant leaves from the solution of nerol in octane. . …… [1] (ii) The boiling point of nerol is 224 °C. The boiling point of octane is 126 °C. Explain how distillation separates nerol from the octane. . …… . …… . …… . …… [2] (d) The mixture of coloured compounds in plant leaves can be separated by chromatography. The apparatus is shown. lid chromatography paper On the diagram: ●● draw an ‘X’ to show where the mixture of coloured compounds is placed at the start of the experiment ●● draw a line to show the level of the solvent at the start of the experiment. [2] (e) Ethanol is a solvent. (i) Draw the structure of ethanol to show all of the atoms and all of the bonds. [2] (ii) Complete the sentences about the manufacture of ethanol using words from the list. catalyst hydrocarbon hydrogen oxygen plastic steam Ethanol is manufactured by the reaction of ethene with …… . The rate of this reaction is increased by the use of a …… . [2] (f) Ethene and propene are in the same homologous series of organic compounds. Which two statements about ethene and propene are correct. Tick two boxes. They have the same physical properties. They have the same number of carbon atoms. They have similar chemical properties. They have the same number of hydrogen atoms. They have the same functional group. [2] [Total: 13]

Question

The diagram shows part of the structures of caesium chloride and carbon dioxide. caesium chloride carbon dioxide O O Cl – Cl – Cl – C C O Cs + Cs + Cs + O O O Cl – Cl – Cl – C O C Cs + Cs + Cs + O (a) Describe both caesium chloride and carbon dioxide in terms of: ●● bonding . …… . …… . …… . …… ●● solubility in water . …… . …… ●● arrangement of particles. . …… . …… [5] (b) Caesium oxide is a compound. What is meant by the term compound ? . …… . …… [1] (c) Explain why caesium is not extracted from caesium oxide by heating with carbon. . …… [1] (d) Caesium is a metal. Describe two properties that are characteristic of most metals. 1 . …… 2 . …… [2] (e) Carbon dioxide is a gas. (i) Which one of these processes does not produce carbon dioxide? Tick one box. the reaction of hydrochloric acid with calcium carbonate respiration in animals and plants the reaction of hydrochloric acid with magnesium the thermal decomposition of calcium carbonate [1] (ii) Carbon dioxide is a greenhouse gas. Give one effect of an increase in the concentration of greenhouse gases in the atmosphere. . …… [1] [Total: 11] 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 20 rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon 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 89–103 104 105 106 107 108 109 110 111 112 114 116 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium – – – – – – – – – – – – – 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.).