Chemistry 0620/22 May/June 2019: question paper and mark scheme

Question

The apparatus shown is set up. After 20 minutes a white ring of ammonium chloride is seen at position Y. cotton wool soaked in cotton wool soaked in concentrated concentrated ammonia solution hydrochloric acid Y white ring of ammonium chloride Which statement about the molecules of ammonia and hydrogen chloride is correct? A Molecules in ammonia have a larger Mr than molecules of hydrogen chloride and so they move more slowly. B Molecules in ammonia have a larger Mr than molecules of hydrogen chloride and so they move more quickly. C Molecules in ammonia have a smaller Mr than molecules of hydrogen chloride and so they move more slowly. D Molecules in ammonia have a smaller Mr than molecules of hydrogen chloride and so they move more quickly.

Question

A student measures 25.00 cm3 of dilute hydrochloric acid accurately. Which apparatus is most suitable? A beaker B measuring cylinder C burette D dropping pipette

Question

The chromatogram of solutions of two metal ions, P and Q, is shown. solvent front P Q baseline P is coloured. A locating agent is used to find the position of Q. The Rf value of each solution is calculated. P is a ……1…… element and has an Rf value ……2…… than that of Q. Which words complete gaps 1 and 2? 1 2 A non-transition greater B non-transition smaller C transition greater D transition smaller 31

Question

What is an isotope of 15 E? 31 33 31 33 A 14 E B 15 E C 16 E D 16 E

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 describes the structure of an ionic compound? A It is a giant lattice of oppositely charged ions. B It is a giant lattice of positive ions in a ‘sea’ of electrons. C It is a giant molecule of oppositely charged ions. D It is a simple molecule of oppositely charged ions.

Question

Calcium metal reacts with water to form a solution of calcium hydroxide and hydrogen gas. Which equation is correct? A Ca(s) + H2O(aq) → CaOH(aq) + H(g) B Ca(s) + 2H2O(aq) → Ca(OH)2(s) + 2H2(g) C Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g) D Ca(s) + H2O(l) → CaOH(l) + H(g)

Question

25.0 cm3 of 0.100 mol / dm3 aqueous sodium hydroxide is neutralised by 24.6 cm3 of dilute sulfuric acid. What is the concentration of the dilute sulfuric acid? A 0.0508 mol / dm3 B 0.0984 mol / dm3 C 0.102 mol / dm3 D 0.203 mol / dm3

Question

The diagram shows the electrolysis of an aqueous solution of X using inert electrodes. power supply – + aqueous solution of X Hydrogen is produced at the cathode and chlorine is produced at the anode. What is X? A concentrated copper(II) chloride solution B concentrated hydrochloric acid C dilute hydrochloric acid D dilute sodium chloride solution

Question

Aluminium is extracted by electrolysis as shown. graphite anode steel case – + + – aluminium oxide dissolved in molten cryolite graphite cathode molten aluminium Which row shows the ionic half-equations at the cathode and the anode? cathode anode A Al 3+ → Al + 3e– 2O2– → O2 + 4e– B Al 3+ → Al + 3e– 2O2– + 4e– → O2 C Al 3+ + 3e– → Al 2O2– → O2 + 4e– D Al 3+ + 3e– → Al 2O2– + 4e– → O2

Question

Fuel cells are used as energy sources in cars. Which row gives a fuel used in a fuel cell and the products formed? fuel in a fuel cell products formed A hydrogen carbon dioxide and water B hydrogen water only C petrol carbon dioxide and water D petrol water only

Question

Two elements, X and Y, react together to form a covalent molecule as shown. The reaction is exothermic. X2(g) + Y2(g) → 2XY(g) The bond energies are shown in the table. bond energy in bond kJ / mol X–X 436 Y–Y 242 X–Y 431 What is the energy change for the reaction? A +184 kJ / mol B –184 kJ / mol C +247 kJ / mol D –247 kJ / mol

Question

Which change in reaction conditions increases both the collision rate and the proportion of molecules with sufficient energy to react? A addition of a catalyst B increasing the concentration of a reactant C increasing the surface area of a reactant D increasing the temperature of the reaction

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

The equation for the manufacture of ethanol is shown. C2H4(g) + H2O(g) C2H5OH(g) ethene steam ethanol What is the effect of doubling the pressure on this reaction? A decreases the rate of formation of ethanol B increases the yield of ethene C decreases the rate of formation of ethene D increases the yield of ethanol

Question

The ionic equation for the reaction of aqueous potassium bromide with chlorine gas is shown. 2Br – + Cl 2 → Br2 + 2Cl – Which statement is correct? A Bromide ions are oxidised by gaining electrons. B Bromide ions are oxidised by losing electrons. C Chlorine is oxidised by gaining electrons. D Chlorine is oxidised by losing electrons.

Question

Which type of oxide are carbon monoxide and aluminium oxide? carbon monoxide aluminium oxide A acidic amphoteric B acidic basic C neutral amphoteric D neutral basic

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

Which row shows the difference between a weak acid and a strong acid? weak acid strong acid A fully ionised partially ionised B concentrated dilute C dilute concentrated D partially ionised fully ionised

Question

Part of the Periodic Table is shown. X Y Z Which row describes the properties of X, Y and Z? good conductor high melting of electricity point A X Z B Y Z and X C Y and Z Z D Z and X X

Question

The melting points and boiling points of the elements of Group I of the Periodic Table are shown. melting point boiling point element / °C / °C lithium 181 1330 sodium 98 883 potassium 63 759 rubidium 39 688 caesium 28 671 Which pair of elements are liquid at 800 °C? A caesium and rubidium B potassium and sodium C lithium and sodium D potassium and caesium

Question

The electronic structures of helium, neon and argon are shown. He Ne Ar Which row describes these gases? reactivity form of the gas electronic structure A reactive monoatomic incomplete outer shell of electrons B unreactive diatomic complete outer shell of electrons C unreactive diatomic incomplete outer shell of electrons D unreactive monoatomic complete outer shell of electrons

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

A student heated the carbonates and nitrates of sodium and copper. The results are shown. compound heated gases released solid formed 1 sodium carbonate carbon monoxide sodium oxide 2 copper(II) carbonate carbon dioxide copper 3 sodium nitrate oxygen only sodium nitrite 4 copper(II) nitrate nitrogen dioxide and oxygen copper(II) oxide Which rows describe the correct results? A 1 and 3 B 2 and 3 C 3 and 4 D 4 only

Question

Zinc is extracted from its ore, zinc blende, using two chemical reactions. 1 2ZnS + 3O2 → 2ZnO + 2SO2 2 2ZnO + C → 2Zn + CO2 Which substance is reduced in reactions 1 and 2? reaction 1 reaction 2 A O2 C B O2 ZnO C ZnS C D ZnS ZnO

Question

Four metals, zinc, M, copper and magnesium, are reacted with aqueous solutions of their nitrates. The results are shown. magnesium M copper zinc metal nitrate nitrate nitrate nitrate magnesium key zinc = reacts M = no reaction copper What is the order of reactivity of these four metals starting with the most reactive? A copper → zinc → M → magnesium B copper → M → zinc → magnesium C magnesium → M → zinc → copper D magnesium → zinc → M → copper

Question

Which property of aluminium makes it useful in the manufacture of aircraft? A conducts electricity B high boiling point C low density D silver colour

Question

The exhaust gases from cars contain oxides of nitrogen. How are these oxides of nitrogen formed? A Nitrogen and oxygen from the air react together at the high temperatures in the engine. B Nitrogen and oxygen from the petrol react together in the car exhaust. C Nitrogen from the petrol reacts with oxygen at the high temperatures in the engine. D Nitrogen reacts with oxygen from the air in the catalytic converter.

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

Some of the processes involved in the carbon cycle are shown. 1 glucose + oxygen → carbon dioxide + water 2 carbon dioxide + water → glucose + oxygen 3 methane + oxygen → carbon dioxide + water What are the names of these processes? 1 2 3 A combustion respiration photosynthesis B photosynthesis combustion respiration C respiration combustion photosynthesis D respiration photosynthesis combustion

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

Ammonia is produced in the Haber process. The equation for the reaction is shown. 3H2(g) + N2(g) 2NH3(g) The forward reaction is exothermic. Which conditions of temperature and pressure produce the highest yield of ammonia? temperature pressure A high high B high low C low high D low low

Question

Which row shows the conditions used in the Contact process? temperature pressure catalyst / °C / atm A 25 2 iron B 25 200 iron C 450 2 vanadium(V) oxide D 450 200 vanadium(V) oxide

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

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

Which statement about homologous series is not correct? A All homologous series are hydrocarbons. B Members of a homologous series have the same functional group. C Members of a homologous series have similar chemical properties. D The alkanes are an example of a homologous series.

Question

In bright sunlight, ethane and chlorine combine in substitution reactions. Which compound is not formed in these reactions? A C2H3Cl B C2H5Cl C C2H4Cl 2 D HCl

Question

What are the properties of aqueous ethanoic acid? reacts with decolourises turns damp red calcium carbonate to bromine water litmus blue make carbon dioxide A B C D

Question

The structures of four molecules are shown. 1 2 3 4 O H H H H H H O H C H C OH H C C C OH H C C C OH H H H H H H OH Which molecules react together to form the ester propyl methanoate? A 1 and 2 B 1 and 3 C 2 and 4 D 3 and 4

Question

But-1-ene has the structure CH3CH2CH=CH2. What is the structure of poly(but-1-ene)? A B C D H H H H H CH2CH3 CH3 CH3 CH2CH3 CH2CH3 C C C C C C C C C C H H H H H H H H H H n n n n 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 20 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.).