Chemistry 0620/21 May/June 2022: question paper and mark scheme

Question

Which two gases will diffuse at the same rate, at the same temperature? A carbon monoxide and carbon dioxide B carbon monoxide and nitrogen C chlorine and fluorine D nitrogen and oxygen

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

The numbers of protons and neutrons and the electronic structures of four particles, W, X, Y and Z, are shown. number of number of electronic protons neutrons structure W 8 8 2,8 X 8 10 2,6 Y 8 8 2,6 Z 10 8 2,8 Which particles have the same chemical properties? A W and Y B W and Z C X and Y D X and Z

Question

Which substance should be pure for the intended use? A a drug for curing disease B limestone for iron extraction C petroleum for fractional distillation D water for washing a car

Question

Metals and ionic compounds have similarities and differences in their structure and properties. Which row about metals and ionic compounds is correct? similarity difference A both contain positive ions only ionic compounds contain anions B both contain positive ions ionic compounds conduct using a ‘sea of electrons’ C both are malleable only ionic compounds contain anions D both are malleable ionic compounds conduct using a ‘sea of electrons’

Question

Which diagram represents the outer-shell electron arrangement in a nitrogen molecule? A B C D N N N N N N N N

Question

The equation for the reaction between barium chloride and dilute sulfuric acid is shown. BaCl 2 + H2SO4 → BaSO4 + 2HCl Which row shows the state symbols for this equation? BaCl 2 H2SO4 BaSO4 2HCl A (aq) (aq) (s) (aq) B (aq) (l) (s) (aq) C (l) (aq) (s) (l) D (aq) (l) (aq) (l)

Question

The relative atomic mass, Ar, of an element is determined by comparing the mass of one atom of the element with the mass of one atom of element Q. What is Q? A carbon B chlorine C hydrogen D oxygen

Question

The equation for the reaction between aqueous lead(II) nitrate and aqueous sodium chloride is shown. Pb(NO3)2(aq) + 2NaCl (aq) → PbCl 2(s) + 2NaNO3(aq) If 100 cm3 of aqueous lead(II) nitrate of concentration 0.1 mol / dm3 is reacted with an excess of aqueous sodium chloride, which mass of lead(II) chloride is obtained? A 1.16 g B 2.42 g C 2.78 g D 3.31 g

Question

The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous sodium chloride using carbon electrodes. + – + – electrode 1 electrode 2 electrode 3 electrode 4 concentrated concentrated aqueous hydrochloric acid sodium chloride At which electrodes is hydrogen produced? A electrode 1 only B electrodes 1 and 3 C electrode 2 only D electrodes 2 and 4

Question

Aqueous copper(II) sulfate is electrolysed using copper electrodes. What is the ionic half-equation for the reaction at the cathode? A Cu → Cu2+ + 2e– B Cu2+ + 2e– → Cu C 2H+ + 2e– → H2 D 2O2– → O2 + 4e–

Question

Which row identifies a chemical change and a physical change? chemical change physical change A boiling ethanol burning ethanol B burning ethanol evaporating ethanol C dissolving ethanol in water burning ethanol D evaporating ethanol dissolving ethanol in water

Question

The equation for the reaction between gaseous hydrogen and gaseous iodine to form gaseous hydrogen iodide is shown. H2(g) + I2(g) → 2HI(g) The reaction is exothermic. Which statement explains why the reaction is exothermic? A Energy is released when H–H and I–I bonds are broken. B The bond energies of the reactants are larger than the bond energies of the products. C The products are at a higher energy level than the reactants. D More energy is released when two HI bonds are formed than is used when the H–H and I–I bonds are broken.

Question

Acidified aqueous silver nitrate is added to a test-tube containing aqueous chloride ions. The test-tube is then left in direct sunlight. Which row describes the observations and explains what happens to the reaction mixture? observation on adding observation after explanation aqueous silver nitrate leaving in sunlight A yellow precipitate precipitate dissolves silver chloride forms B yellow precipitate precipitate turns grey silver ions are reduced C white precipitate precipitate dissolves silver chloride forms D white precipitate precipitate turns grey silver ions are reduced

Question

Water is added to anhydrous copper(II) sulfate. What happens during the reaction? A The copper(II) sulfate turns blue and the solution formed gets colder. B The copper(II) sulfate turns blue and the solution formed gets hotter. C The copper(II) sulfate turns white and the solution formed gets colder. D The copper(II) sulfate turns white and the solution formed gets hotter.

Question

Aqueous iron(III) chloride, FeCl 3, reacts with aqueous potassium iodide, KI. vFeCl 3 + wKI → xFeCl 2 + yKCl + I2 Which statements are correct? 1 In the balanced equation, v, w, x and y have the same value. 2 Potassium iodide is an oxidising agent. 3 A dark brown solution is produced in the reaction. A 1 and 2 B 1 and 3 C 2 only D 2 and 3

Question

Which statement about acids is correct? A A strong acid has a higher pH than a weak acid of the same concentration. B A strong acid is a proton acceptor. C A weak acid is a proton donor. D A weak acid is fully ionised in aqueous solution.

Question

The oxides of two elements, X and Y, are separately dissolved in water and the pH of each solution tested. oxide tested pH of solution X 1 Y 13 Which information about X and Y is correct? oxide is oxide is metal non-metal acidic basic A X Y X Y B X Y Y X C Y X X Y D Y X Y X

Question

An acid is neutralised by adding an excess of an insoluble solid base. A soluble salt is formed. How is the pure salt obtained from the reaction mixture? A crystallisation → evaporation → filtration B evaporation → crystallisation → filtration C filtration → crystallisation → evaporation D filtration → evaporation → crystallisation

Question

The electronic structure of element Z is 2,8,1. Which statements about Z are correct? 1 It is a metal. 2 It has two outer-shell electrons. 3 It is in Period 3. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 only

Question

Elements in Group IV of the Periodic Table are shown. carbon silicon germanium tin lead What does not occur in Group IV as it is descended? A The proton number of the elements increases. B The elements become more metallic. C The elements have more electrons in their outer shell. D The elements have more electron shells.

Question

Element M forms both M+ and M2+ ions. In which part of the Periodic Table is M placed? A Group I B Group II C Group III D transition elements

Question

In the extraction of aluminium by electrolysis, cryolite is added to the bauxite ore. Which row describes the role of cryolite and gives the ionic half-equation at the cathode? role of cryolite ionic half-equation at the cathode A catalyst Al 3+ + 3e– → Al B catalyst Al 3+ + 3e– → 3Al C lowers melting point of electrolyte Al 3+ + 3e– → Al D lowers melting point of electrolyte Al 3+ + 3e– → 3Al

Question

Mild steel is galvanised to prevent corrosion of the iron. Which statements about galvanising are correct? 1 Galvanising prevents corrosion because the zinc forms an alloy. 2 If the coating is damaged, water and oxygen do not corrode the iron. 3 Zinc is a sacrificial metal and corrodes in preference to iron. A 1 and 2 B 1 and 3 C 2 only D 2 and 3

Question

Which diagram represents the arrangement of the outer-shell electrons of a noble gas? A B C D

Question

Which statements about the general properties of metals are correct? 1 They are good conductors of heat and electricity. 2 They have low melting points. 3 They react with dilute acids to form a salt and water. 4 They react with oxygen to form basic oxides. A 1 and 2 B 1 and 4 C 2 and 3 D 3 and 4

Question

Reactions of three metals and their oxides are shown. add dilute heat metal hydrochloric acid metal oxide to metal with carbon 1 key 2 = reacts 3 = does not react What is the order of reactivity of these metals, from most reactive to least reactive? A 1→2→3 B 1→3→2 C 2→1→3 D 2→3→1

Question

Three metal compounds, J, K and L, are heated using a Bunsen burner. The results are shown. J colourless gas produced, which relights a glowing splint K colourless gas produced, which turns limewater milky L no reaction Which row identifies J, K and L? J K L A magnesium carbonate potassium carbonate potassium nitrate B magnesium carbonate potassium nitrate potassium carbonate C potassium nitrate magnesium carbonate potassium carbonate D potassium nitrate potassium carbonate magnesium carbonate

Question

The diagram shows the uses and treatment processes of muddy river water. process 1 process 2 muddy river water clear river water disinfected water use 1 use 2 Which row identifies uses 1 and 2 and processes 1 and 2? use 1 use 2 process 1 process 2 A drinking watering crops chlorination filtration B drinking watering crops filtration chlorination C watering crops drinking chlorination filtration D watering crops drinking filtration chlorination

Question

The equation for the manufacture of ammonia in the Haber process is shown. 3H2(g) + N2(g) 2NH3(g) The forward reaction is exothermic. Which row describes the effect of the stated change on the reaction rate and the yield of ammonia? change effect on reaction rate effect on yield of ammonia A decrease pressure increases decreases B decrease temperature decreases increases C increase pressure increases decreases D increase temperature increases increases

Question

Fertilisers are used to provide three of the elements needed for plant growth. Which two compounds would give a fertiliser containing all three of these elements? A Ca(NO3)2 and (NH4)2SO4 B Ca(NO3)2 and (NH4)3PO4 C KNO3 and (NH4)2SO4 D KNO3 and (NH4)3PO4

Question

The flow chart shows part of the process for the manufacture of sulfuric acid and its electrolysis. electrolysis gas 2 concentrated dilute gas 3 sulfuric acid sulfuric acid gas 1 What are gases 1, 2 and 3? gas 1 gas 2 gas 3 A sulfur dioxide hydrogen sulfur trioxide B sulfur dioxide oxygen sulfur trioxide C sulfur trioxide hydrogen sulfur dioxide D sulfur trioxide oxygen sulfur dioxide

Question

Which statements about sulfur dioxide are correct? 1 Sulfur dioxide decolourises acidified potassium manganate(VII). 2 Sulfur dioxide forms when acids react with carbonates. 3 Sulfur dioxide is used as a bleach. 4 Sulfur dioxide is used to treat acidic soil. A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Question

What are the products when limestone (calcium carbonate) is heated strongly? A calcium hydroxide and carbon dioxide B calcium hydroxide and carbon monoxide C calcium oxide and carbon dioxide D calcium oxide and carbon monoxide

Question

The structure of ester W is shown. H O H C C H H O C H H Which row gives the names of ester W and the carboxylic acid and alcohol from which it is made? name of ester W carboxylic acid alcohol A ethyl methanoate ethanoic acid methanol B ethyl methanoate methanoic acid ethanol C methyl ethanoate ethanoic acid methanol D methyl ethanoate methanoic acid ethanol

Question

Ethanol is made industrially by the fermentation of glucose or by the catalytic addition of steam to ethene. Which statement describes an advantage of fermentation compared to catalytic addition? A Ethanol is the only product of fermentation. B Fermentation uses a batch process but catalytic addition is continuous. C Fermentation uses a higher temperature than catalytic addition. D Fermentation uses a renewable resource.

Question

Some properties of colourless liquid L are listed. ● It boils at 65 °C. ● When added to water, two layers form which do not mix. ● It does not react with sodium carbonate. ● It has no effect on bromine water. What is L? A ethanol B hexane C hexene D ethanoic acid

Question

A molecule of compound P contains two carbon atoms and four hydrogen atoms. Which row represents P? name of reacts with Mr compound aqueous bromine A ethane 30 B ethene 16 C ethene 28 D ethene 28

Question

The reaction of ethanol with acidified potassium manganate(VII) is shown. KMnO4 CH3CH2OH CH3COOH H+ Which type of reaction is taking place? A addition B condensation C hydrolysis D oxidation

Question

Which polymer is a synthetic polyamide? A nylon B poly(ethene) C protein D Terylene 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.).