Chemistry 0620/11 October/November 2020: question paper and mark scheme

Question

‘The movement of a substance very slowly from an area of high concentration to an area of low concentration.’ Which process is being described? A a liquid being frozen B a solid melting C a substance diffusing through a liquid D a substance diffusing through the air

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What happens to the average speed of gas particles when pressure and temperature are increased? average speed of particles pressure increases temperature increases A faster faster B unchanged slower C slower faster D unchanged faster

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Which piece of apparatus can only measure a single fixed volume? A 250 cm3 beaker B 50 cm3 burette C 100 cm3 measuring cylinder D 25 cm3 pipette

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In the chromatography experiment shown, which label represents the solvent front? A B D C

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Which substances can be separated by filtration? A insoluble liquid and water B insoluble solid and water C solution of soluble liquid in water D solution of soluble solid in water

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An atom of element R contains 15 protons, 16 neutrons and 15 electrons. What is R? A gallium B phosphorus C sulfur D zinc

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Which row describes the properties of potassium iodide, KI? type of boiling solid conducts aqueous solution bonding point electricity conducts electricity A covalent low no no B covalent high no yes C ionic high yes yes D ionic high no yes

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Which diagram represents a mixture of compounds? A B C D

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Rubidium is in Group I of the Periodic Table and bromine is in Group VII. Rubidium reacts with bromine to form an ionic compound. Which row shows the electron change taking place for rubidium and the correct formula of the rubidium ion? electron change formula of ion formed A electron gained Rb+ B electron gained Rb– C electron lost Rb+ D electron lost Rb–

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Which statement explains why graphite is used as a lubricant? A All bonds between the atoms are weak. B It conducts electricity. C It has a low melting point. D Layers in the structure can slide over each other.

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The equation for burning propane in air is shown. C3H8(g) + xO2(g) → 3CO2(g) + yH2O(g) Which values of x and y balance the equation? x y A 3 4 B 4 8 C 5 4 D 10 8

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The relative atomic mass of chlorine is 35.5. When calculating relative atomic mass, which particle is the mass of a chlorine atom compared to? A a neutron B a proton C an atom of carbon-12 D an atom of hydrogen-1

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Concentrated aqueous sodium chloride is electrolysed using platinum electrodes. What is the major product formed at each electrode? anode cathode A chlorine hydrogen B chlorine sodium C oxygen hydrogen D oxygen sodium

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Three substances are listed. 1 copper 2 dilute sulfuric acid 3 solid lead(II) bromide Which substances conduct electricity? A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

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Sodium nitrate is added to water in a beaker and stirred until it dissolves. At the end of the experiment, the beaker feels cold. Which row describes the reaction? temperature type of of solution reaction A decreases endothermic B decreases exothermic C increases endothermic D increases exothermic

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Which substance does not require oxygen in order to produce energy? A coal B hydrogen C natural gas 235 D U

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Which process involves a physical change? A heating calcium carbonate B burning wood C melting an ice cube D mixing an acid and a base

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A sign displayed in a flour mill is shown. DANGER Explosion Hazard No Smoking No Open Flames Which statement explains why there is a danger of explosion in a flour mill? A Flour burns very quickly because it is a fine powder. B Flour is a catalyst for combustion. C Flour mills get hot and speed up the rate of combustion. D The combustion of flour is exothermic.

Question

The graph shows the results of two experiments investigating the rate of reaction between excess calcium carbonate and dilute hydrochloric acid. In each experiment the volume of carbon dioxide produced is measured at fixed time intervals. experiment 1 volume of CO2 experiment 2 0 0 time Which statement describes the difference in conditions between experiments 1 and 2? A In experiment 2 a higher concentration of dilute hydrochloric acid is used. B In experiment 2 a higher temperature is used. C In experiment 2 the mass of calcium carbonate is greater. D In experiment 2 the particle size of calcium carbonate is greater.

Question

When pink crystals of cobalt(II) chloride are heated, steam is given off and the colour of the solid changes to blue. CoCl 2•6H2O CoCl 2 + 6H2O What happens when water is added to the blue solid? colour temperature A changes to pink decreases B changes to pink increases C remains blue decreases D remains blue increases

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In which change is the sulfur, S, in sulfur(I) oxide, S2O, reduced? SO3 A D B S S2O SO2 C SO

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What is a characteristic of acids? A Acids turn methyl orange indicator yellow. B Acids have a high pH value. C Acids react with ammonium salts to give ammonia gas. D Acids react with carbonates to produce salts.

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Four different groups of oxides are shown. 1 MgO FeO CuO 2 CaO SO2 TiO2 3 PbO CaO Cl 2O 4 NO2 Br2O P2O5 Which statement about these oxides is correct? A 1, 2 and 3 contain basic oxides only. B 2, 3 and 4 contain basic oxides only. C 1 contains basic oxides only and 4 contains acidic oxides only. D 1 contains acidic oxides only and 4 contains basic oxides only.

Question

A student carries out an experiment to prepare pure magnesium sulfate crystals. The diagram shows the first stage of the preparation. stirrer magnesium carbonate dilute sulfuric acid He adds magnesium carbonate until no more reacts. Which process should he use for the next stage? A crystallisation B evaporation C filtration D neutralisation

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Which ion produces a green precipitate when aqueous sodium hydroxide is added? A Cu2+ B Fe2+ C Fe3+ D Zn2+

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The positions of four elements in the Periodic Table are shown. Which element is a gas that displaces iodine from sodium iodide? B C D A

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A flammable gas needs to be removed from a tank at an industrial plant. For safety reasons, an inert gas is used. Which gas is suitable? A argon B hydrogen C methane D oxygen

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A substance, X, has the following properties. 1 It has a high melting point. 2 It conducts electricity in the solid and liquid states. 3 It is malleable. 4 It has a high density. What is X? A a ceramic B copper C graphite D sodium chloride

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A reactivity series is shown. sodium calcium magnesium carbon zinc iron hydrogen copper Which statement is correct? A All the metals above carbon are extracted by electrolysis. B Iron can only be extracted by electrolysis. C Calcium can be extracted by heating calcium oxide with carbon. D Copper can only be extracted by passing hydrogen over heated copper(II) oxide.

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What is the symbol of the metal used in the manufacture of aircraft because of its strength and low density? A Al B Cu C Fe D Zn

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Oxides of nitrogen are given out from car exhausts. Which row best shows why oxides of nitrogen are unwanted in the atmosphere? acidic toxic A no no B no yes C yes no D yes yes

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Two reactions, M and N, both form carbon dioxide. M N CaCO3 CO2 CH4 Which types of reaction are M and N? M N A thermal decomposition thermal decomposition B thermal decomposition combustion C combustion thermal decomposition D combustion combustion

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Which row describes two uses of sulfur dioxide? use 1 use 2 A bleaching paper pulp neutralising acidic industrial waste B bleaching paper pulp preserving food and drink C extracting iron from hematite neutralising acidic industrial waste D extracting iron from hematite preserving food and drink

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Which statement about lime and limestone is correct? A Calcium oxide is formed from limestone in a displacement reaction. B Lime is used to treat alkaline soils. C Limestone is a waste material in the manufacture of iron. D Slaked lime is used in the process of flue gas desulfurisation.

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Which compound has a chemical name ending in –ol ? A C2H5OH B C2H6 C CH3COOH D C2H4

Question

Petroleum is separated into fractions by fractional distillation. Separation occurs in a fractionating column. Some properties of three of these fractions are shown. number of boiling point fraction carbon atoms in range / °C the molecules 1 5 –10 2 320–350 16–24 3 120–210 Which statement is correct? A Fraction 1 has a higher boiling point range than fraction 2. B Fraction 2 is removed from a higher point in the fractionating column than fraction 1. C Molecules in fraction 3 have shorter chains than those in fraction 2. D None of the fractions are liquid at room temperature.

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Which statement about alkenes is correct? A Alkenes are saturated hydrocarbons. B Alkenes can be made by cracking other hydrocarbon compounds. C Alkenes change bromine water from colourless to brown. D Alkene molecules contain double bonds between carbon atoms and hydrogen atoms.

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The flow chart shows the preparation of ethanol and some important chemistry of ethanol. fermentation process Y substance X ethanol carbon dioxide + substance Z What are X, Y and Z? X Y Z A yeast combustion oxygen B glucose combustion steam C glucose polymerisation water D yeast fermentation glucose

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Which statements about aqueous ethanoic acid are correct? 1 It is an alkane. 2 It reacts with sodium carbonate to form carbon dioxide. 3 It changes the colour of litmus solution from blue to red. 4 It is a hydrocarbon. A 1 and 2 B 1 and 4 C 2 and 3 D 3 and 4

Question

Which substance is a polymer? A diamond B graphite C nylon D sodium chloride 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 89–103 104 105 106 107 108 109 110 111 112 114 116 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.).