Chemistry 0620/13 May/June 2019: question paper and mark scheme

Question

Which row describes the arrangement and motion of the particles in a liquid? arrangement motion A irregular and most particles touching moving slowly B irregular spaces between all particles moving slowly C regular and most particles touching moving slowly D regular spaces between all particles moving quickly

Question

Which piece of apparatus is used to measure 24.8 cm3 of gas produced during a reaction? A beaker B conical flask C measuring cylinder D pipette

Question

Calcium carbonate is insoluble in water. Sodium chloride is soluble in water. Which sequence of steps is used to obtain a pure, dry sample of calcium carbonate from a mixture of calcium carbonate and aqueous sodium chloride? A filter → dry the residue with filter paper → wash the residue with water B filter → heat the filtrate to crystallising point → leave the filtrate to cool and crystallise C filter → wash the filtrate with water → dry the filtrate D filter → wash the residue with water→ dry the residue

Question

A student uses paper chromatography to identify the food dyes in a coloured sweet, S. The student uses four known food dyes, W, X, Y, and Z, and ethanol as the solvent. The chromatogram obtained is shown. W X Y Z S Which statements are correct? 1 S contains only two dyes. 2 X is insoluble in ethanol. 3 S contains Y and Z. 4 S contains W. A 1, 2 and 4 only B 2 and 3 only C 2 and 4 only D 4 only

Question

The structure of an atom is shown. key = electron 7p n = neutron 8n p = proton Which element is the atom an isotope of? A nitrogen B oxygen C phosphorus D titanium

Question

What happens when sodium atoms combine with chlorine atoms to form sodium chloride? A Sodium atoms gain one electron and chlorine atoms lose one electron. B Sodium atoms lose one electron and chlorine atoms gain one electron. C Sodium atoms and chlorine atoms share one electron with each other. D Sodium atoms and chlorine atoms share two electrons with each other.

Question

Which row describes the formation of single covalent bonds in methane? A atoms share a pair of electrons both atoms gain a noble gas electronic structure B atoms share a pair of electrons both atoms have the same number of electrons in their outer shell C electrons are transferred from one both atoms gain a atom to another noble gas electronic structure D electrons are transferred from one both atoms have the same number atom to another of electrons in their outer shell

Question

Which statement about diamond is correct? A It is a giant covalent structure consisting of carbon atoms and each atom is bonded to four other atoms. B It is a giant covalent structure consisting of flat sheets of carbon atoms. C It is a structure held together by ionic bonds and each ion is bonded to four other ions. D It is a structure held together by ionic bonds and each ion is bonded to three other ions.

Question

The compound magnesium nitrate has the formula Mg(NO3)2. What is the relative formula mass of magnesium nitrate? A 86 B 134 C 148 D 172

Question

Which substance does not produce a gas at both electrodes during electrolysis? A concentrated aqueous sodium chloride B concentrated hydrochloric acid C dilute sulfuric acid D molten lead(II) bromide

Question

Which row describes the changes that occur when metals burn in oxygen? temperature metal is A decreases oxidised B decreases reduced C increases oxidised D increases reduced

Question

Which process is a physical change? A burning magnesium in air B dissolving sodium chloride in water C adding magnesium to hydrochloric acid D heating green copper(II) carbonate until it turns black

Question

A student reacts strips of zinc with dilute sulfuric acid and measures the time taken to produce 100 cm3 of hydrogen. The experiment is repeated using different conditions. The results are shown in the table. time to produce 100 cm3 experiment of hydrogen / s 1 250 2 100 Which changes in conditions produce the results shown in experiment 2? 1 Add a catalyst. 2 Dilute the acid. 3 Use zinc powder. 4 Heat the acid. A 1, 3 and 4 only B 1 and 4 only C 2 and 3 only D 2 and 4 only

Question

When blue-green crystals of nickel(II) sulfate are heated, water is produced and a yellow solid remains. When water is added to the yellow solid, the blue-green colour returns. Which process describes these changes? A combustion B corrosion C neutralisation D reversible reaction

Question

Zinc is formed when zinc oxide is heated with carbon. zinc oxide + carbon → zinc + carbon monoxide Which substance is oxidised in this reaction? A carbon B carbon monoxide C zinc D zinc oxide

Question

Which row shows the colours of litmus and methyl orange with solutions of acids and bases? solution litmus methyl orange A acid red red B acid blue yellow C base blue red D base red yellow

Question

The positions of elements W, X, Y and Z in the Periodic Table are shown. W Y X Z Which elements form basic oxides? A W, X and Y B W and X only C Y only D Z only

Question

Copper(II) sulfate is made when copper(II) carbonate reacts with dilute sulfuric acid. CuCO3 + H2SO4 → CuSO4 + H2O + CO2 Pure copper(II) sulfate crystals are obtained. Which reagent is in excess and how are the crystals obtained? reagent in excess how the crystals are obtained A copper(II) carbonate filter and evaporate the solution to dryness B copper(II) carbonate filter, evaporate to crystallising point and then cool C dilute sulfuric acid evaporate the solution to dryness D dilute sulfuric acid evaporate to crystallising point and then cool

Question

Two separate tests are done on a solution of a compound, X. The results are shown. 1 Adding aqueous ammonia forms a blue precipitate that dissolves in an excess of aqueous ammonia. 2 Adding dilute nitric acid and aqueous barium nitrate forms a white precipitate. What is X? A chromium(III) chloride B chromium(III) sulfate C copper(II) chloride D copper(II) sulfate

Question

Part of the Periodic Table is shown. W X Y Z Which row describes W, X, Y and Z? metal non-metal A X W, Y and Z B X and Y W and Z C W and Z X and Y D W, Y and Z X

Question

Which statement about the properties of elements in Group I and in Group VII is correct? A Bromine displaces iodine from an aqueous solution of potassium iodide. B Chlorine, bromine and iodine are diatomic gases at room temperature. C Lithium, sodium and potassium are soft non-metals. D Lithium, sodium and potassium have an increasing number of electrons in their outer shells.

Question

Some information about four elements, P, Q, R and S, is shown. melting point density colour of in °C in g / cm3 chloride P 1247 7.43 pink Q 1410 2.33 white R 1910 6.11 purple S 115 2.07 red Which elements are transition elements? A P and R B P and S C Q and R D R and S

Question

Gas G has 10 electrons. Gas H has eight more electrons than gas G. Both gases are monoatomic. Which statement about G and H is correct? A Both gases are in the same group of the Periodic Table. B Both gases are in the same period of the Periodic Table. C Both gases are very reactive. D Gas G has a higher atomic mass than gas H.

Question

The diagrams show the structure of two substances used to make electrical conductors. X Y Which statement correctly describes X and Y? A X is a pure metal and Y is a compound. B X is a pure metal and Y is an alloy. C X is a solid and Y is a liquid. D X is harder and stronger than Y.

Question

Three metals, L, M and N, are added separately to dilute hydrochloric acid and cold water. The results are shown. reaction with reaction with metal hydrochloric acid cold water L hydrogen forms no reaction M hydrogen forms hydrogen forms N no reaction no reaction What is the order of reactivity of the metals? least most reactive reactive A L N M B M L N C N L M D N M L

Question

Iron is extracted from its ore in a blast furnace. Hematite, coke, limestone and hot air are added to the furnace. Which explanation is not correct? A Coke burns and produces a high temperature. B Hematite is the ore containing the iron as iron(III) oxide. C Hot air provides the oxygen for the burning. D Limestone reduces the iron(III) oxide to iron.

Question

Aluminium is used to make containers for storing food. Which property makes it suitable for this use? A conducts heat B low density C resists corrosion D shiny surface

Question

Water can be treated by filtration then chlorination. Which uses do not need water of this quality? 1 water for cooling in industry 2 water for washing clothes 3 water for drinking A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Which statement about acid rain is not correct? A It causes limestone buildings and statues to erode. B It is formed from the burning of compounds which contain sulfur. C It is formed from the combustion of hydrogen as a fuel. D It is formed from the oxides of nitrogen formed in car engines.

Question

The diagram shows an experiment to investigate how paint affects the rusting of iron. P Q iron painted iron air water What happens to the water level in tubes P and Q? tube P tube Q A falls rises B no change rises C rises falls D rises no change

Question

Which gas is produced when ammonium chloride is warmed with aqueous sodium hydroxide? A ammonia B chlorine C hydrogen D nitrogen

Question

Which statement describes a disadvantage of sulfur dioxide? A It can be used as a bleach when making wood pulp. B It can be used to kill bacteria in food. C It can be used to manufacture sulfuric acid. D It dissolves in water to form acid rain.

Question

The diagram represents a lime kiln used to heat limestone to a very high temperature. waste gases lime kiln limestone fuel in fuel in air in air in X What leaves the kiln at X? A calcium carbonate B calcium hydroxide C calcium oxide D calcium sulfate

Question

The structures of four compounds are shown. 1 2 3 4 H H H H H O H H H C C H C C H C C H C C OH H H H H H OH H H Which row gives the names of the compounds? 1 2 3 4 A ethene ethane ethanol ethanoic acid B ethane ethene ethanoic acid ethanol C ethene ethane ethanoic acid ethanol D ethane ethene ethanol ethanoic acid

Question

Which fuel could be gasoline? Is it obtained from petroleum? yes no Is it used as Is it used as fuel for cars? fuel for cars? yes no yes no A B C D

Question

A hydrocarbon W burns to form carbon dioxide and water. W decolourises bromine water. What is the name of W and what is its structure? name of W structure of W H H A ethane H C C H H H H H B ethane C C H H H H C ethene H C C H H H H H D ethene C C H H

Question

Which statements about homologous series are correct? 1 All members have similar chemical properties. 2 All members have the same molecular mass. 3 Ethane and ethene are members of the same homologous series. 4 Ethane and propane are members of the same homologous series. A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Question

Which statements about ethanol are correct? 1 It can be made by fermentation. 2 It is an unsaturated compound. 3 It burns in air and can be used as a fuel. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Which statement about aqueous ethanoic acid is correct? A It reacts with metal carbonates to form salts, hydrogen and water. B It reacts with metal oxides to form salts and oxygen. C It reacts with reactive metals to form salts and hydrogen. D It turns damp red litmus paper blue.

Question

Which substances are synthetic polymers? 1 Terylene 2 nylon 3 protein 4 poly(ethene) A 1, 2 and 4 B 1 only C 2 and 3 D 3 and 4 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.).