Chemistry 0620/22 May/June 2021: question paper and mark scheme

Question

A gas is released at point P in the apparatus shown. P damp universal indicator paper Which gas turns the damp universal indicator paper red most quickly? A ammonia, NH3 B chlorine, Cl 2 C hydrogen chloride, HCl D sulfur dioxide, SO2

Question

A mixture of colourless compounds is separated using chromatography. Which type of reagent is used to detect these compounds after separation? A a dehydrating agent B a locating agent C an oxidising agent D a reducing agent

Question

Which statement about paper chromatography is correct? A A solvent is needed to dissolve the paper. B Paper chromatography separates mixtures of solvents. C The solvent should cover the baseline. D The baseline should be drawn in pencil.

Question

Element X has 7 protons. Element Y has 8 more protons than X. Which statement about element Y is correct? A Y has more electron shells than X. B Y has more electrons in its outer shell than X. C Y is in a different group of the Periodic Table from X. D Y is in the same period of the Periodic Table as X.

Question

A covalent molecule Q contains only six shared electrons. What is Q? A ammonia, NH3 B chlorine, Cl 2 C methane, CH4 D water, H2O

Question

Information about four substances E, F, G and H is shown. melting point / °C electrical conductivity E 1710 does not conduct when solid F 3500 conducts when solid G 120 does not conduct H 801 conducts when molten E, F, G and H are graphite, poly(ethene), sodium chloride and silicon(IV) oxide but not in that order. What are E, F, G and H? E F G H A graphite poly(ethene) silicon(IV) oxide sodium chloride B sodium chloride graphite poly(ethene) silicon(IV) oxide C poly(ethene) sodium chloride graphite silicon(IV) oxide D silicon(IV) oxide graphite poly(ethene) sodium chloride

Question

Chemical compounds formed from a Group I element and a Group VII element contain ionic bonds. How are the ionic bonds formed? A Electrons are transferred from Group VII atoms to Group I atoms. B Electrons are shared between Group I atoms and Group VII atoms. C Electrons are lost by Group I atoms and Group VII atoms. D Electrons are transferred from Group I atoms to Group VII atoms.

Question

Some information about particles P, Q, R and S is shown. nucleon number of number of number neutrons electrons P 12 6 6 Q 24 12 10 R 16 8 10 S 14 8 6 Which two particles are isotopes of the same element? A P and Q B P and S C Q and R D R and S

Question

Chlorine gas will react with iron metal. Exactly 21.3 g of chlorine reacts with 11.2 g of iron. How many iron atoms react with 30 molecules of chlorine? A 10 B 15 C 20 D 30

Question

In separate experiments, electricity was passed through concentrated aqueous sodium chloride and molten lead(II) bromide. What would happen in both experiments? A A halogen would be formed at the anode. B A metal would be formed at the cathode. C Hydrogen would be formed at the anode. D Hydrogen would be formed at the cathode.

Question

A reaction involving aluminium is shown. xAl + yO2 + 6H2O → xAl (OH)3 Which values of x and y balance the equation? x y A 2 3 B 3 2 C 3 4 D 4 3

Question

Four different fuels are used to heat a beaker of water, for the same amount of time, using the apparatus shown. thermometer stirrer screen to reduce draughts 200 g of water spirit burner fuel The initial temperature of the water and the temperature after heating by the fuel are recorded. Which fuel releases the most heat energy? initial temperature temperature after / °C heating / °C A 17 46 B 24 52 C 26 61 D 30 62

Question

An excess of calcium carbonate reacts with dilute hydrochloric acid. The volume of carbon dioxide produced is measured at regular time intervals. The results are shown as experiment 1. The experiment is repeated with only one change to the reaction conditions. The results are shown as experiment 2. experiment 2 experiment 1 volume of CO2 time Which change is made in experiment 2? A The concentration of the acid is increased. B The volume of acid is increased. C The mass of calcium carbonate is increased. D The calcium carbonate is powdered.

Question

When sulfur is heated it undergoes a ……1…… change as it melts. Further heating causes the sulfur to undergo a ……2…… change and form sulfur dioxide. Which words complete gaps 1 and 2? 1 2 A chemical chemical B chemical physical C physical chemical D physical physical

Question

Four statements about the effect of increasing temperature on a reaction are shown. 1 The activation energy becomes lower. 2 The particles move faster. 3 There are more collisions between reacting particles per second. 4 There are more collisions which have energy greater than the activation energy. Which statements are correct? A 1, 2 and 3 B 1, 3 and 4 C 2, 3 and 4 D 2 and 3 only

Question

An example of a redox reaction is shown. Zn + Cu2+ → Zn2+ + Cu Which statement about the reaction is correct? A Zn is the oxidising agent and it oxidises Cu2+. B Zn is the oxidising agent and it reduces Cu2+. C Zn is the reducing agent and it oxidises Cu2+. D Zn is the reducing agent and it reduces Cu2+.

Question

When bismuth(III) chloride, BiCl 3, reacts with water, a white precipitate of bismuth(III) oxychloride, BiOCl, is formed. The equation for the reaction is shown. BiCl 3(aq) + H2O(l) BiOCl (s) + 2H+(aq) + 2Cl –(aq) The reaction is in equilibrium. Which changes cause the white precipitate to dissolve? 1 adding acid 2 adding water 3 adding sodium chloride solution A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3

Question

Element X forms an oxide, XO, that neutralises sulfuric acid. Which row describes X and XO? element X nature of oxide, XO A metal acidic B metal basic C non-metal acidic D non-metal basic

Question

Information about the solubility of salts is shown. salt solubility chlorides soluble (except for lead(II) chloride and silver chloride) nitrates soluble sulfates soluble (except for barium sulfate and lead(II) sulfate) Aqueous solutions of which two compounds would produce a precipitate when added together? A Ba(NO3)2 and CaCl 2 B CuSO4 and Zn(NO3)2 C KCl and Na2SO4 D Pb(NO3)2 and MgSO4

Question

The equation shows the reaction between hydrogen and oxygen. 2 H–H + O=O → 2 H–O–H The bond energies are shown. bond energy in kJ / mol H–H 436 O=O 495 O–H 463 Which row shows the energy change and the type of reaction? energy change type of reaction in kJ / mol A 441 exothermic B 441 endothermic C 485 exothermic D 485 endothermic

Question

Burning fossil fuels releases sulfur dioxide which leads to acid rain. Which ion in the rain water causes it to be acidic? A H+ B OH– C O2– D SO42–

Question

Which statement about the trends shown by the elements of Period 3 in the Periodic Table is not correct? A The elements become less metallic across the period. B The group number increases across the period. C The number of electron shells increases across the period. D The number of outer electrons increases across the period.

Question

The diagram shows the positions of elements E, F, G and H in the Periodic Table. G H E F Which statements about elements E, F, G and H are correct? 1 E has a higher density than F. 2 E has a higher melting point than F. 3 G has a darker colour than H. 4 G has a lower melting point than H. A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Question

When aqueous iodine is added to a solution of vanadium ions, V2+, the V2+ ions each lose one electron. Which property of transition elements is shown by this reaction? A Transition elements have variable oxidation states. B Transition elements form a stable 1+ ion. C Transition elements are oxidising agents. D Transition elements can act as catalysts.

Question

A piece of aluminium is dropped into dilute hydrochloric acid. No immediate reaction is observed. Which statement explains this observation? A Aluminium does not neutralise acids. B Aluminium is a non-metal so does not react with acids. C Aluminium is below hydrogen in the reactivity series. D Aluminium is covered in an unreactive oxide layer.

Question

Some metal nitrates and carbonates decompose when heated strongly. Metal Q has a nitrate that decomposes to give a salt and a colourless gas only. The carbonate of metal Q does not decompose when heated with a Bunsen burner. What is metal Q? A calcium B copper C sodium D zinc

Question

Aluminium is extracted from its ore by electrolysis. Which equation represents the reaction that occurs at the anode during the electrolysis? A Al 3+ + 3e– → Al B Al 3+ → Al + 3e– C 2O2– → O2 + 4e– D 2O2– + 2e– → O2

Question

Mild steel consists mostly of iron. Mild steel can be prevented from rusting by a process called galvanising. Copper is not a very strong metal. However, if it is mixed with a suitable metal a strong alloy called brass is produced. Which statement is correct? A Copper corrodes very quickly when wet and brass does not. B Copper is mixed with zinc to produce brass. C Galvanising mild steel changes it from a pure metal into an alloy. D When a steel object is galvanised this means it is coated with a thin layer of tin.

Question

Water is used for the irrigation of crops and for drinking water. For which uses must water be chlorinated? irrigation drinking A B C D

Question

Which natural resource cannot provide a raw material for the manufacture of ammonia? A air B limestone C petroleum D water

Question

Ammonia is made in the Haber process. Which conditions are used in the Haber process? temperature pressure catalyst used / °C / atmospheres A 450 200 iron B 450 5 vanadium(V) oxide C 200 450 iron D 200 5 vanadium(V) oxide

Question

Which process in the carbon cycle is responsible for removing carbon dioxide from the atmosphere? A combustion B decomposition C photosynthesis D respiration

Question

The equations represent two reactions, P and Q, of lime (calcium oxide). P CaO + SiO2 → CaSiO3 Q CaO + SO2 → CaSO3 In which processes do the reactions occur? P Q A extraction of iron extraction of iron B extraction of iron flue gas desulfurisation C flue gas desulfurisation extraction of iron D flue gas desulfurisation flue gas desulfurisation

Question

Which statement about ethanol is not correct? A Ethanol can be made by fermentation. B Ethanol is oxidised to make ethanoic acid. C Ethanol reacts with oxygen exothermically, making it a good fuel. D Ethanol reacts with propanoic acid to make propyl ethanoate.

Question

Which pair of formulae represents two alkanes? A CH4 and C8H18 B C2H6 and C5H8 C C3H6 and C5H12 D C10H8 and C4H8

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Which statement about alkanes is correct? A They burn in oxygen. B They contain carbon, hydrogen and oxygen atoms. C They contain double bonds. D They contain ionic bonds.

Question

Which statements about ethanoic acid are correct? 1 It is a strong acid. 2 It reacts with ethanol to form an ester. 3 It has the formula CH3COOH. A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3

Question

The flow chart shows how petroleum may be turned into a plastic. process process process 1 saturated 2 unsaturated 3 petroleum plastic hydrocarbon hydrocarbon What are processes 1, 2 and 3? process 1 process 2 process 3 A cracking fractional distillation polymerisation B cracking polymerisation fractional distillation C fractional distillation cracking polymerisation D fractional distillation polymerisation cracking

Question

The structure of a synthetic polymer is shown. O O O O O C C N N C C N N C H H H H The structure shows that it is a ……1…… . It is formed by ……2…… polymerisation. Which words complete gaps 1 and 2? 1 2 A polyamide addition B polyamide condensation C polyester addition D polyester condensation

Question

Which substance is a natural polymer? A ethene B Terylene C nylon D protein 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 85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131 16 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.).