Chemistry 0620/12 February/March 2019: question paper and mark scheme

Question

Four processes are listed. 1 Brownian motion 2 condensation 3 diffusion 4 evaporation Which processes involve a change of state? A 1 and 2 B 1 and 3 C 2 and 4 D 3 and 4

Question

A student measures the time taken for 2.0 g of magnesium to dissolve in 50 cm3 of dilute sulfuric acid. Which apparatus is essential to complete the experiment? 1 stop-clock 2 measuring cylinder 3 thermometer 4 balance A 1, 2 and 4 B 1 and 2 only C 1 and 4 only D 2, 3 and 4

Question

Which method should be used to separate a mixture of two liquids? A crystallisation B electrolysis C filtration D fractional distillation

Question

Lead(II) iodide is insoluble in water. Lead(II) iodide is made by adding aqueous lead(II) nitrate to aqueous potassium iodide. Which pieces of apparatus are needed to obtain solid lead(II) iodide from 20 cm3 of aqueous lead(II) nitrate? 1 2 3 4 5 A 1, 2 and 4 B 1, 3 and 5 C 1, 4 and 5 D 2, 4 and 5

Question

Which row describes isotopes of the same element? number of protons number of neutrons A different different B different same C same different D same same

Question

Which row describes the structure of the positive ion in sodium chloride? protons electrons neutrons A 11 11 12 B 11 10 12 C 17 17 18 D 17 18 18

Question

Which pair of statements about diamond and graphite is correct? diamond graphite A Diamond and graphite are both pure carbon. They are both macromolecules. B Diamond and graphite can both be used as electrodes. Graphite is also used as a lubricant. C Diamond has covalent bonds. Graphite has ionic bonds. D Diamond is hard with a high melting point. Graphite is soft with a low melting point.

Question

What is the nucleon number of an atom? A the number of neutrons B the number of protons C the total number of protons and neutrons D the total number of protons and electrons

Question

The relative formula mass, Mr, of calcium carbonate, CaCO3, is 100. What is the mass of carbon present in 100 g of calcium carbonate? A 12 g B 36 g C 40 g D 60 g

Question

Two electrolysis experiments were carried out as shown. The graphite electrodes are labelled 1– 4. power power supply supply + – + – 1 2 3 4 molten concentrated aqueous sodium chloride sodium chloride Which row describes the products at the electrodes in these experiments? electrode 1 electrode 2 electrode 3 electrode 4 A chlorine hydrogen chlorine hydrogen B chlorine sodium chlorine hydrogen C chlorine sodium hydrogen chlorine D sodium chlorine sodium chlorine 11 10 g of ammonium nitrate is added to water at 25 °C and the mixture stirred. The ammonium nitrate dissolves and, after one minute, the temperature of the solution is 10 °C. Which word describes this change? A endothermic B exothermic C neutralisation D reduction

Question

In the question paper above.

Question

Which process involves a chemical change? A dissolving copper(II) sulfate B distilling ethanol C freezing water D neutralising copper(II) oxide

Question

Lumps of limestone react with dilute hydrochloric acid according to the equation shown. CaCO3 + 2HCl → CaCl 2 + H2O + CO2 Which change in conditions decreases the rate of the reaction? A increase the concentration of the acid B increase the volume of the acid C increase the size of the lumps of limestone D increase the temperature

Question

Which reaction is reversible? A Cu + ZnSO4 → CuSO4 + Zn B CuO + H2SO4 → CuSO4 + H2O C CuO + H2 → Cu + H2O D CuSO4•5H2O → CuSO4 + 5H2O

Question

The reaction between magnesium and carbon dioxide is shown in the equation. 2Mg + CO2 → 2MgO + C Which statement describes what happens in this reaction? A Carbon is oxidised. B Magnesium is reduced. C Neither oxidation nor reduction happens. D The carbon in carbon dioxide is reduced.

Question

Barium hydroxide is an alkali. It reacts with hydrochloric acid. How does the pH of the hydrochloric acid change as an excess of aqueous barium hydroxide is added? A The pH decreases from pH 14 and becomes constant at pH 7. B The pH decreases from pH 14 to about pH 1. C The pH increases from pH 1 and becomes constant at pH 7. D The pH increases from pH 1 to about pH 14.

Question

Copper(II) sulfate crystals are blue. They are made by adding an excess of copper(II) oxide to sulfuric acid. The mixture is heated and stirred. It is then filtered and the filtrate is allowed to evaporate, leaving blue crystals. Why is filtration necessary? A to remove soluble properties B to remove sulfuric acid C to remove the blue crystals D to remove unreacted copper(II) oxide

Question

The results of two tests on an aqueous solution of X are shown. test observation aqueous sodium hydroxide added green precipitate formed acidified aqueous silver nitrate added yellow precipitate formed What is X? A copper(II) chloride B copper(II) iodide C iron(II) chloride D iron(II) iodide

Question

Information about the solubility in water of four oxides is shown. Which oxide, when added to water, gives a solution with a pH less than pH 7? name of oxide solubility in water A nitrogen dioxide soluble B copper(II) oxide insoluble C silicon(IV) oxide insoluble D barium oxide soluble

Question

The elements sodium to argon form Period 3 of the Periodic Table. Which row describes the trend across Period 3 from left to right? number of outer metallic group number shell electrons character A decreases decreases decreases B decreases increases decreases C increases decreases increases D increases increases increases

Question

Astatine is below iodine in Group VII in the Periodic Table. Which row describes the properties of astatine? state at room reactivity temperature A gas displaces chlorine, bromine and iodine B gas displaces iodine but does not displace chlorine or bromine C solid displaces iodine but does not displace chlorine or bromine D solid does not displace chlorine, bromine or iodine

Question

Which row describes a transition element? density colour of in g / cm3 chloride A 0.98 green B 0.98 white C 8.90 green D 8.90 white

Question

Which statement explains why elements in Group VIII of the Periodic Table are unreactive? A They are monatomic gases. B They form stable diatomic molecules. C They have a full outer shell of electrons. D They share electrons with each other.

Question

The electrical conductivity of magnesium was tested. Magnesium was then added to dilute sulfuric acid and a gas, Q, was produced. Which row is correct? electrical conductivity gas Q of magnesium A good hydrogen B good oxygen C poor hydrogen D poor oxygen

Question

Four reactions that take place in the blast furnace to produce iron are shown. Which reaction is used to keep the furnace hot? A C + O2 → CO2 B CO2 + C → 2CO C Fe2O3 + 3C → 2Fe + 3CO D Fe2O3 + 3CO → 2Fe + 3CO2

Question

The list gives the order of some metals and hydrogen in the reactivity series. Metal X is also included. most reactive K Mg Zn H X least reactive Cu Which row correctly shows the properties of metal X? reacts with oxide reduced dilute acids by carbon A no no B no yes C yes no D yes yes

Question

The properties of four elements are shown. Which element is used to make aircraft bodies? brittle or density malleable A high brittle B high malleable C low brittle D low malleable

Question

The diagram shows how water is treated to make it suitable for drinking. stage 1 stage 2 stage 3 stage 4 reservoir drinking chlorination of water water What happens in stage 2? A condensation B sublimation C evaporation D filtration

Question

A farmer treats a field with calcium hydroxide to make it less acidic. When the farmer adds ammonium nitrate fertiliser to the field immediately after the calcium hydroxide, they react. Why does this reaction make the fertiliser less effective? A It makes ammonia gas, so less nitrogen is absorbed by the soil. B It makes an acid, making the soil acidic again. C It makes nitrogen gas, so less nitrogen is absorbed by the soil. D It makes the fertiliser too strong, stopping the plants growing so well.

Question

Which row showing an air pollutant and its major source is not correct? pollutant major source of pollutant A carbon monoxide complete combustion of carbon fuels B lead compounds leaded petrol C oxides of nitrogen car engines D sulfur dioxide fossil fuels containing sulfur

Question

Which substances are needed for iron to rust? A carbon dioxide and oxygen B oxygen only C water and carbon dioxide D water and oxygen

Question

Methane and carbon dioxide are both greenhouse gases. Which row identifies a source of methane and a source of carbon dioxide? source of methane source of carbon dioxide A decomposition of vegetation hydrogen car exhausts B digestion in animals diesel car exhausts C petrol car exhausts decomposition of vegetation D respiration petrol car exhausts

Question

Which element has an oxide that is used as a food preservative? A helium B hydrogen C iron D sulfur

Question

Lime is made by heating limestone. Which equation represents this reaction? A CaCO3 → Ca + O2 + CO B CaCO3 → CaO + CO2 C CaCO3 + H2O → CaO + H2CO3 D CaCO3 + H2O → Ca(OH)2 + CO2

Question

Most objects made from synthetic polymers last for many years. Why do these polymers last for so long? chemically biodegradable unreactive A no no B no yes C yes no D yes yes

Question

The structure of a compound, G, is shown. G is in the same homologous series as ethanoic acid. H H O H C C C O H H H Which row describes some of the properties of an aqueous solution of G? produces a gas turns methyl orange with magnesium yellow A no yes B no no C yes no D yes yes

Question

The fractional distillation of petroleum is shown. refinery gas gasoline fraction paraffin fraction diesel oil lubricating fraction petroleum bitumen Which fraction is the least volatile? A bitumen B diesel oil C gasoline fraction D refinery gas

Question

Which row shows the properties of methane? soluble state at room gives a positive test in water temperature with aqueous bromine A no gas no B no gas yes C yes liquid no D yes liquid yes

Question

The formulae of five compounds are listed. 1 C4H10 2 C2H5OH 3 C4H9OH 4 C4H9COOH 5 C5H11OH Which compounds are in the same homologous series? A 1, 3 and 4 only B 2, 3 and 5 only C 3 and 4 only D 3 and 5 only

Question

Which process is used to make an alkene from a long-chain alkane? A combustion B condensation C cracking D polymerisation 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.).