Chemistry 0620/42 February/March 2021: question paper and mark scheme

Question

The table shows the numbers of protons, neutrons and electrons in particles A to I. particle protons neutrons electrons A 1 0 0 B 6 6 6 C 6 8 6 D 10 10 10 E 16 16 18 F 17 18 17 G 18 22 18 H 19 20 19 I 20 20 18 Answer the following questions about particles A to I. Each letter may be used once, more than once or not at all. (a) State which of the particles A to I: (i) is an anion …… [1] (ii) are cations …… and …… [2] (iii) are noble gas atoms …… and …… [2] (iv) is a halogen atom …… [1] (v) is a Group I atom …… [1] (vi) have the same nucleon number …… and …… [1] (vii) causes acidity in aqueous solutions …… [1] (viii) is used to define the relative atomic mass of elements…… [1] (b) Explain why B and C are isotopes of the same element. . …… . …… [2] [Total: 12]

Question

The elements shown are gases at room temperature and pressure. hydrogen nitrogen oxygen chlorine (a) State which one of these gases is green. . …… [1] (b) The gases shown exist as diatomic molecules. State the name of another element which has diatomic molecules and is a gas at room temperature and pressure. . …… [1] (c) When separate samples of each of these gases are placed in a container they will diffuse. (i) Describe why these gases diffuse. . …… [1] (ii) State which of these four gases has the highest rate of diffusion. Explain your answer. gas . …… explanation …… . …… [2] (d) Nitrogen, oxygen and other substances are found in clean, dry air. (i) State the percentage of nitrogen in clean, dry air. . …… [1] (ii) Other than nitrogen and oxygen, identify another element found in clean, dry air. . …… [1] (iii) Identify a compound found in clean, dry air. . …… [1] (iv) Nitrogen and oxygen can be separated from liquid air. State the name of this process. . …… [2] [Total: 10]

Question

This question is about ammonia. (a) Nitrogen reacts with hydrogen to form ammonia in an industrial process. N2(g) + 3H2(g) 2NH3(g) (i) Name this industrial process. . …… [1] (ii) State the meaning of the symbol . . …… [1] (iii) State the conditions used in this industrial process. Include units. temperature …… pressure . …… [2] (iv) Name the catalyst used in this industrial process. . …… [1] (v) If the pressure is increased, the yield of ammonia increases. Explain why, in terms of equilibrium. . …… . …… . …… [2] (vi) If the temperature is increased, the rate of reaction increases. Explain why, in terms of particles. . …… . …… . …… . …… . …… [3] (b) Ammonia reacts with sulfuric acid to make a compound which is used as a fertiliser. Write the chemical equation for the reaction between ammonia and sulfuric acid. . …… [2] [Total: 12]

Question

A student wanted to make some zinc chloride crystals. The student followed the procedure shown. step 1 Add excess zinc powder to dilute hydrochloric acid to form aqueous zinc chloride. step 2 Remove unreacted zinc powder from the aqueous zinc chloride. step 3 Heat the solution until it is saturated. step 4 Allow the saturated solution to cool and remove the crystals that form. (a) Write the equation for the reaction in step 1. Include state symbols. . …… [3] (b) Explain why excess zinc powder is added in step 1. . …… [1] (c) Suggest how unreacted zinc powder is removed in step 2. . …… [1] (d) A saturated solution is formed in step 3. Suggest what is meant by the term saturated solution. . …… . …… [2] (e) Explain why crystals form as the solution cools in step 4. . …… [1] (f) Name two zinc compounds which react with dilute hydrochloric acid to form zinc chloride. . …… . …… [2] (g) If excess calcium metal is used instead of excess zinc powder in step 1, pure calcium chloride crystals do not form. Explain why. . …… . …… [1] (h) Some salts can be made by titration. In a titration experiment, 20.0 cm3 of aqueous sodium hydroxide reacts exactly with 25.0 cm3 of 0.100 mol / dm3 dilute sulfuric acid to make sodium sulfate. 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) (i) Circle the name of the type of reaction that takes place. decomposition neutralisation precipitation reduction [1] (ii) Calculate the concentration of the aqueous sodium hydroxide in g / dm3 using the following steps. ● Calculate the number of moles of dilute sulfuric acid used. …… mol ● Determine the number of moles of sodium hydroxide which react with the dilute sulfuric acid. …… mol ● Calculate the concentration of the aqueous sodium hydroxide in mol / dm3. …… mol / dm3 ● Calculate the concentration of the aqueous sodium hydroxide in g / dm3. …… g / dm3 [5] [Total: 17] QUESTION 5 STARTS ON THE NEXT PAGE.

Question

The table shows the names or structures of organic compounds P to U. P Q R H H H H C C C H propanoic acid but-1-ene H H H S T U H H H propan-1-ol methyl butanoate C C C H H H (a) Give the letters of the organic compounds, P to U, that are unsaturated hydrocarbons. . …… [2] (b) Describe the test for an unsaturated hydrocarbon. test . …… observations …… [2] (c) But-1-ene is an unbranched molecule. (i) Name the unbranched isomer of but-1-ene. . …… [1] (ii) Draw the structure of a branched isomer of but-1-ene. Show all of the atoms and all of the bonds. [1] (d) Dodecane is an alkane with 12 carbon atoms. Dodecane can be cracked. (i) Write the formula of dodecane. . …… [1] (ii) Give the letters of all the organic compounds, P to U, that can be formed when dodecane is cracked. . …… [2] (e) Name the reagent and suggest the conditions needed to convert organic compound U into organic compound S. reagent …… conditions …… [3] (f) Organic compound S can be converted to organic compound Q by reaction with an acidified reagent. (i) Name the type of chemical change that happens to organic compound S. . …… [1] (ii) Name the acidified reagent added to organic compound S. . …… [1] (g) Organic compound T is made by reacting two compounds together. (i) Name the homologous series that organic compound T belongs to. . …… [1] (ii) Name the two compounds which react together to make organic compound T. Draw the structures of each compound you have named. Show all of the atoms and all of the bonds. name . …… structure name . …… structure [4] (iii) Deduce the molecular formula of organic compound T. . …… [1] [Total: 20]

Question

Polymers are large molecules built up from small molecules. (a) State the name given to the small molecules from which polymers are made. . …… [1] (b) The formula of a polymer is shown. H H C C CH3 CH3 n (i) Draw the structure of the small molecule from which this polymer is made. Show all of the atoms and all of the bonds. [2] (ii) State the type of polymerisation used to make this polymer. . …… [1] (c) Three amino acids are shown. They combine to form part of a natural polymer. H 2N COOH H 2N COOH H 2N COOH (i) Name the type of natural polymer formed when amino acids combine. . …… [1] (ii) Complete the diagram to show part of the structure of the natural polymer that forms when these three amino acids combine. Show all of the bonds in the linkages. [3] (iii) Name the type of chemical reaction that takes place when this natural polymer is converted back to amino acids. . …… [1] [Total: 9] 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 12 85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131 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.).