Chemistry 0620/12 October/November 2021: question paper and mark scheme

Question

Which row describes what happens to the particles in solid iodine when it is heated and turned into a gas? separation speed of particles of particles A closer together faster B closer together slower C further apart faster D further apart slower

Question

A student put exactly 25.00 cm3 of dilute hydrochloric acid into a conical flask. The student added 2.5 g of solid sodium carbonate and measured the change in temperature of the mixture. Which apparatus does the student need to use? A balance, measuring cylinder, thermometer B balance, pipette, stopwatch C balance, pipette, thermometer D burette, pipette, thermometer

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A student separates sugar from pieces of broken glass by dissolving the sugar in water and filtering off the broken glass. filtrate What is the filtrate? A broken glass only B broken glass and sugar solution C pure water D sugar solution

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How many protons, neutrons and electrons are there in one atom of the isotope 27 13 Al ? protons neutrons electrons A 13 13 13 B 13 14 13 C 14 13 13 D 14 14 13

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Which description of brass is correct? A alloy B compound C element D non-metal

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Rubidium is in Group I and iodine is in Group VII of the Periodic Table. Which row describes what happens when rubidium and iodine react together to form rubidium iodide? rubidium iodine A each atom gains one electron each atom loses one electron B each atom loses one electron each atom gains one electron C each atom loses more than one electron each atom gains more than one electron D each atom neither gains each atom neither gains nor loses an electron nor loses an electron

Question

Which row shows the properties for an ionic compound? electrical conductivity volatility when solid A high good B high poor C low good D low poor

Question

Which substance is described as a macromolecule? A ammonia B graphite C iron D sodium chloride

Question

The formula of sodium chlorate(V) is NaCl O3. What is the relative formula mass of sodium chlorate(V), NaCl O3? A 52.0 B 74.5 C 106.5 D 223.5

Question

Iron can be electroplated with zinc to make it resistant to corrosion. Which row about electroplating iron with zinc is correct? positive electrode negative electrode electrolyte (anode) (cathode) A iron zinc iron nitrate B iron zinc zinc nitrate C zinc iron iron nitrate D zinc iron zinc nitrate

Question

An energy level diagram for the reaction between substance X and substance Y to form substance Z is shown. Z energy X+Y progress of reaction Which statement is correct? A Energy is released as substance Z is formed. B Substance Z has more energy than substance X and substance Y. C The reaction is exothermic. D When substance X and substance Y react, the temperature increases.

Question

Which reactions are exothermic? 1 C + O2 → CO2 2 CH4 + 2O2 → CO2 + 2H2O 3 2H2 + O2 → 2H2O A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Solid copper(II) carbonate reacts with dilute sulfuric acid. CuCO3 + H2SO4 → CuSO4 + CO2 + H2O The rate of the reaction can be changed by varying the conditions. Which changes always increase the rate of this chemical reaction? 1 increasing the concentration of sulfuric acid 2 increasing the size of the pieces of copper(II) carbonate 3 increasing the temperature 4 increasing the volume of sulfuric acid A 1, 3 and 4 B 1 and 3 only C 2 and 3 D 3 and 4 only

Question

When a piece of marble is added to hydrochloric acid, bubbles of carbon dioxide gas are given off. Which method is used to find the rate of the reaction? A counting the number of gas bubbles formed B measuring the diameter of the gas bubbles C measuring the speed at which the gas bubbles rise upwards through the acid D measuring the time taken for 10 cm3 of gas to be collected

Question

Solid X is heated strongly. The colour of the solid changes from blue to white. What is solid X? A anhydrous cobalt(II) chloride B calcium carbonate C hydrated copper(II) sulfate D lead(II) bromide

Question

What happens to a chemical substance when it is reduced? A It burns. B It decomposes. C It loses oxygen. D It gains mass.

Question

Which statements about acids and bases are correct? 1 An acid reacts with a metal to give off hydrogen. 2 A base reacts with an ammonium salt to give off ammonia. 3 An acid reacts with a carbonate to give off carbon dioxide. 4 Alkaline solutions are orange in methyl orange. A 1, 2 and 3 B 1, 2 and 4 C 1, 3 and 4 D 2, 3 and 4

Question

Oxide 1 is a solid that reacts with dilute hydrochloric acid. Oxide 2 is a gas that reacts with sodium hydroxide solution. What are the formulae of the oxides? oxide 1 oxide 2 A CaO MgO B MgO NO2 C NO2 SO2 D SO2 CaO

Question

In the preparation of zinc sulfate crystals, excess zinc oxide is added to dilute sulfuric acid. Why is an excess of zinc oxide added? A to make sure crystals are formed and not powder B to avoid filtering the mixture C to use up all of the sulfuric acid D to use up all of the zinc oxide

Question

Which statement about aqueous sodium hydroxide is correct? A When it is added to a solution containing sulfate ions, a white precipitate is formed. B When it is added to a solution of copper(II) ions, a blue precipitate is formed which dissolves in excess to give deep blue solution. C When it is added to a solution of iron(II) ions, a green precipitate is formed which does not dissolve in excess. D When it is added to ammonium chloride, a gas is produced which turns blue litmus red.

Question

A period of the Periodic Table is shown. group I II III IV V VI VII VIII element R S T V W X Y Z The letters are not their chemical symbols. Which statement is correct? A Element R does not conduct electricity. B Elements R and Y react together to form an ionic compound. C Element Z exists as a diatomic molecule. D Element Z reacts with element T.

Question

Which statement about the elements in Group VII of the Periodic Table is correct? A Chlorine can displace bromine from bromides. B Group VII elements are all solids at room temperature. C Group VII elements occur as monoatomic covalent molecules. D Reactivity increases down Group VII.

Question

Part of the Periodic Table is shown. Which element is a transition element? A C B D

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The noble gases are in Group VIII of the Periodic Table. Which statement explains why noble gases are unreactive? A They all have eight electrons in their outer shells. B They all have full outer shells. C They are all gases. D They are all monoatomic.

Question

Which statement is correct for all metals? A They conduct electricity when molten. B They gain electrons when they form ions. C They have a low density. D They have a low melting point.

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Which row describes the method of extraction of aluminium and iron from their ores? aluminium iron A electrolysis electrolysis B electrolysis reduction with carbon C reduction with carbon electrolysis D reduction with carbon reduction with carbon

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Which statement about metals and their uses is correct? A Aluminium is used to make food containers because it is resistant to corrosion. B Aluminium is used to make aircraft wings because it is strong and has a high density. C Iron is used to make electrical wires because it is a good insulator of electricity. D Iron is used to make cooking utensils because it is easily recycled.

Question

The diagrams show some uses of water in the home. 1 2 3 For which uses is it important for the water to have been treated? A 1 only B 2 only C 3 only D 1, 2 and 3

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Four different test-tubes containing water and an iron nail are left for two weeks. Which nail showed the least amount of rusting? A B C D tap water boiled boiled tap water tap water tap water

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Which process does not produce a greenhouse gas? A acid rain on limestone buildings B combustion of wood C digestion in cows D zinc reacting with sulfuric acid

Question

Sulfur burns to make sulfur dioxide. Which row describes a source of sulfur and a use of sulfur dioxide? source of sulfur use of sulfur dioxide A the air food preservative B the air treating acidic soils C underground deposits food preservative D underground deposits treating acidic soils

Question

Lime (calcium oxide) is used to treat waste water from a factory. Which substance is removed by the lime? A ammonia B sodium chloride C sodium hydroxide D sulfuric acid

Question

A chemical equation for the complete combustion of methane is shown. 2CH4 + zO2 → 2CO2 + 4H2O What is the value of z? A 2 B 3 C 4 D 6

Question

Fuel X produces carbon dioxide and water when it is burned in air. So does fuel Y. What could X and Y be? X Y A C H2 B C C8H18 C CH4 H2 D CH4 C8H18

Question

Which substance is not a fossil fuel? A ethanol B gasoline C kerosene D methane

Question

Which compound belongs to a different homologous series to the others? A B C D H H H H O H OH H H C OH H C C OH H C C OH H C C C H H H H H H H H

Question

What is a property of aqueous ethanoic acid? A It changes red litmus blue. B It has a deep purple colour. C It has a pH of less than 7. D It reacts with a metal oxide to form carbon dioxide.

Question

Which statements about unsaturated hydrocarbons are correct? 1 They contain both single and double bonds. 2 They turn aqueous bromine from colourless to brown. 3 They can be manufactured by cracking. A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3

Question

Which substance is used to produce alcohol by fermentation? A phosphoric acid B platinum C iron D yeast

Question

Which statements are correct? 1 Polymers are large molecules built up from monomers. 2 Proteins are natural polymers. 3 Proteins and carbohydrates are constituents of food. A 1 and 2 only B 1 and 3 only C 2 and 3 only D 1, 2 and 3 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.).