Chemistry 0620/13 May/June 2021: question paper and mark scheme

Question

A 1 cm3 sample of substance X is taken. This is sample 1. X is then converted to a different physical state and a 1 cm3 sample is taken. This is sample 2. Sample 2 contains more particles in the 1 cm3 than sample 1. Which process caused this increase in the number of particles in 1 cm3? A boiling of liquid X B condensation of gaseous X C evaporation of liquid X D sublimation of solid X

Question

Solid carbon dioxide changes directly into a gas under suitable conditions of temperature and pressure. Carbon dioxide gas moves from a high concentration to a low concentration. Which row names these two processes? moving from a changing from high concentration to solid to gas a low concentration A evaporation Brownian motion B evaporation diffusion C sublimation Brownian motion D sublimation diffusion

Question

Which statement about paper chromatography is correct? A A solvent is needed to dissolve the paper. B Paper chromatography separates mixtures of solvents. C The solvent should cover the baseline. D The baseline should be drawn in pencil.

Question

Element X has 7 protons. Element Y has 8 more protons than X. Which statement about element Y is correct? A Y has more electron shells than X. B Y has more electrons in its outer shell than X. C Y is in a different group of the Periodic Table from X. D Y is in the same period of the Periodic Table as X.

Question

A covalent molecule Q contains only six shared electrons. What is Q? A ammonia, NH3 B chlorine, Cl 2 C methane, CH4 D water, H2O

Question

Which piece of apparatus is used to measure exactly 25.00 cm3 of hydrochloric acid? A beaker B measuring cylinder C pipette D balance

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Which statement about isotopes of the same element is correct? A They have different numbers of electrons. B They have different numbers of neutrons. C They have different numbers of protons. D They have the same mass number.

Question

Potassium reacts with iodine to form an ionic compound. 2K + I2 → 2KI Which statements describe what happens when potassium reacts with iodine? 1 Each potassium atom loses two electrons. 2 Each potassium atom loses one electron. 3 Each iodine atom gains one electron. 4 Each iodine atom gains two electrons. A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Question

What is the relative formula mass of magnesium nitrate, Mg(NO3)2? A 74 B 86 C 134 D 148

Question

In separate experiments, electricity was passed through concentrated aqueous sodium chloride and molten lead(II) bromide. What would happen in both experiments? A A halogen would be formed at the anode. B A metal would be formed at the cathode. C Hydrogen would be formed at the anode. D Hydrogen would be formed at the cathode.

Question

The equation for the decomposition of calcium carbonate is shown. CaCO3 → CaO + CO2 What mass of calcium oxide is produced when 10 g of calcium carbonate is heated? A 4.4 g B 5.0 g C 5.6 g D 10.0 g

Question

Heat energy transfer during chemical reactions can be described using energy level diagrams. In which row is the description correct? energy level diagram description energy 1 exothermic progress of reaction energy heat energy absorbed 2 from environment progress of reaction energy heat energy released 3 to environment progress of reaction energy 4 endothermic progress of reaction A 1 and 2 B 1 and 3 only C 1, 3 and 4 D 2 and 4

Question

The equations for two reactions are shown. 1 CH4 + 2O2 → CO2 + 2H2O 2 2H2 + O2 → 2H2O Which statement about the reactions is correct? A Heat energy is released during both these reactions. B Heat energy is absorbed during both these reactions. C Heat energy is released during reaction 1 but absorbed during reaction 2. D Heat energy is released during reaction 2 but absorbed during reaction 1.

Question

When sulfur is heated it undergoes a ……1…… change as it melts. Further heating causes the sulfur to undergo a ……2…… change and form sulfur dioxide. Which words complete gaps 1 and 2? 1 2 A chemical chemical B chemical physical C physical chemical D physical physical

Question

Copper(II) carbonate reacts with dilute sulfuric acid. Which conditions produce the fastest rate of reaction? form of temperature of dilute copper(II) carbonate sulfuric acid / °C A large lumps 37 B large lumps 70 C powder 37 D powder 70

Question

Hydrated copper(II) sulfate is blue. When it is heated it forms white anhydrous copper(II) sulfate. How is a sample of anhydrous copper(II) sulfate changed into hydrated copper(II) sulfate? A Water is added. B It is cooled down. C It is heated up. D Water is removed.

Question

Copper(II) oxide reacts with iron. The equation for the reaction is shown. 3CuO + 2Fe → 3Cu + Fe2O3 Why can this reaction be described as the reduction of copper(II) oxide? A Iron gains oxygen. B The copper(II) oxide loses oxygen. C The copper(II) oxide weighs less after the reaction than before. D There are fewer substances on the right of the equation.

Question

Element X forms an oxide, XO, that neutralises sulfuric acid. Which row describes X and XO? element X nature of oxide, XO A metal acidic B metal basic C non-metal acidic D non-metal basic

Question

Which methods of salt preparation are suitable for copper(II) chloride? 1 Add copper(II) carbonate to dilute hydrochloric acid. 2 Add copper to dilute hydrochloric acid. 3 Warm copper(II) oxide with dilute hydrochloric acid. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

A white solid, J, is tested and the observations are shown. test observations flame test red flame acidify with nitric acid then white precipitate add aqueous silver nitrate What is J? A lithium bromide B lithium chloride C sodium bromide D sodium chloride

Question

Which statement about the Periodic Table is not correct? A Elements in the same period have similar properties. B It can be used to predict the properties of elements. C Non-metals are found on the right side of the table. D There are more metals than non-metals.

Question

Bromine and iodine are elements in Group VII of the Periodic Table. Which statement about these elements is correct? A Iodine displaces bromide ions from solution. B Bromine is a lighter colour than iodine. C Bromine is more dense than iodine. D Bromine is less reactive than iodine.

Question

Helium and neon exist as monoatomic gases at room temperature and pressure. statement 1 Helium and neon have eight electrons in their outer shell. statement 2 Helium and neon are unreactive. Which option is correct? A Statement 1 and statement 2 are incorrect. B Statement 1 is correct and explains statement 2. C Statement 1 is correct, but does not explain statement 2. D Statement 1 is incorrect, but statement 2 is correct.

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An element melts at 1455 °C, has a density of 8.90 g / cm3 and forms a green chloride. Where in the Periodic Table is this element found? A B C D

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Which statement about the reactivity of metals is correct? A Iron is more reactive than magnesium. B Copper reacts with dilute hydrochloric acid. C Potassium reacts with cold water. D Calcium oxide is reduced more easily than iron oxide.

Question

Iron from a blast furnace is treated with oxygen and with calcium oxide to make steel. Which substances in the iron are removed? oxygen calcium oxide removes removes A carbon acidic oxides B carbon basic oxides C iron acidic oxides D iron basic oxides

Question

Water is removed from reservoirs and undergoes several stages of treatment to make it suitable for drinking. Which statements about the stages are correct? 1 Chlorine is added to the water to kill harmful bacteria. 2 Water is heated to remove dissolved oxygen gas. 3 Water is filtered to remove solids. A 1 only B 1 and 2 C 1 and 3 D 2 and 3

Question

Which gas is an air pollutant that causes acid rain? A argon B carbon monoxide C methane D nitrogen dioxide

Question

An NPK fertiliser is made by mixing two compounds. The first compound has the formula (NH4)2HPO4. What is the formula of the second compound? A CaCO3 B KNO3 C NaCl D (NH4)2SO4

Question

Which reaction does not occur during the extraction of iron from hematite in a blast furnace? A C + O2 → CO2 B CaO + SiO2 → CaSiO3 C CO2 + C → 2CO D 4Fe + 3O2 → 2Fe2O3

Question

Which row describes the uses of sulfur and sulfur dioxide? sulfur sulfur dioxide A extraction of aluminium food preservative B extraction of aluminium manufacture of cement C manufacture of sulfuric acid food preservative D manufacture of sulfuric acid manufacture of cement

Question

Metal X is a good conductor of electricity and is used for electrical wiring. Metal Y is used to make an alloy which is resistant to corrosion and is used to make cutlery. Metal Z is light and strong and is used in the manufacture of aircraft. What are X, Y and Z? X Y Z A aluminium iron copper B copper iron aluminium C aluminium copper iron D copper aluminium iron

Question

Which statement about calcium carbonate is correct? A It is made by the thermal decomposition of limestone. B It is used to neutralise alkaline soils. C It is a reactant in the test for carbon dioxide. D It is used to remove impurities in iron extraction.

Question

What is the main constituent of natural gas? A hydrogen B methane C nitrogen D oxygen

Question

Which compounds belong to the same homologous series? A ethane and propane B ethanoic acid and ethanol C methane and ethene D propene and ethanoic acid

Question

Which statement about alkanes is correct? A They burn in oxygen. B They contain carbon, hydrogen and oxygen atoms. C They contain double bonds. D They contain ionic bonds.

Question

P, Q, R and S are organic compounds. P is formed by reacting ethene with steam. Q decolourises bromine water. R is a hydrocarbon; all of its bonds are single covalent bonds. S is a waste product from digestion in animals. Which compounds are alkanes? A P and Q B P and S C Q and R D R and S

Question

Which row describes how ethanol is used? fuel solvent A no no B no yes C yes no D yes yes

Question

Which diagram shows the conversion of ethene into ethanol? A B H H H H H H H H C C H C C H C C H C C O H H H H H H H H H C D H H H H H H H H H C C H C C H C C H H C C O H H H H H H H H H

Question

Which substance is a natural polymer? A ethene B Terylene C nylon D protein 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.).