0620 Chemistry November 2025 Question Paper 42

1 The three states of matter are solid, liquid and gas.

(a) Complete Table 1.1 to describe the structures of solids, liquids and gases in terms of particle separation, particle arrangement and particle motion. Table 1.1 state of matter particle separation particle arrangement particle motion solid touching liquid gas random random

[3]

(b) Substances can physically change.

Name each physical change: • solid to liquid • gas to liquid • solid to aqueous [3]

(c) Gases diffuse.

(i) Describe, in terms of particles, why gases diffuse [1]

(ii) State what determines the relative rate of diffusion of gases at constant temperature [1]

(d) Gaseous oxides of nitrogen are atmospheric pollutants. One adverse effect of oxides of nitrogen is the formation of acid rain.

State two other adverse effects of oxides of nitrogen. 1 2 [2] , ,

(e) In a catalytic converter, oxides of nitrogen are removed by reaction with the toxic gaseous product of the incomplete combustion of hydrocarbon fuels. Two non-toxic gases are formed in this reaction.

(i) Name the toxic gaseous product of the incomplete combustion of hydrocarbon fuels [1]

(ii) Name the two non-toxic gases formed in the catalytic converter. 1 2 [2]

[Total: 13] , ,

2 Iron is extracted from iron ore in a blast furnace.

(a) The iron compound in the main iron ore used in the blast furnace is iron(III) oxide.

(i) State the name of the main iron ore used in the blast furnace [1]

(ii) State how the main source of heat is provided in the blast furnace [1]

(iii) Name the gaseous reducing agent in the blast furnace [1]

(iv) Write a symbol equation for the reduction of iron(III) oxide by the gaseous reducing agent in (a)(iii) [2]

(v) The main impurity in iron ore is silicon(IV) oxide.

Write two symbol equations to show the role of limestone in removing silicon(IV) oxide from iron ore. 1 2 [2]

(b) Table 2.1 shows four different isotopes of iron, A, B, C and D. Table 2.1 A B C D 54Fe 56Fe 57Fe 58Fe

Explain why A, B, C and D are isotopes of iron [2] , ,

(c) Iron can form two different ions, Fe2+ and Fe3+.

(i) Complete Table 2.2 to show the number of protons, neutrons and electrons in the two iron ions shown. Table 2.2 54Fe2+ 58Fe3+ protons neutrons electrons

[3]

(ii) Describe a test for aqueous Fe2+ ions. test observations [2]

(d) An oxidising agent converts Fe2+ ions to Fe3+ ions.

(i) Define the term oxidising agent [2]

(ii) Explain why the conversion of Fe2+ ions to Fe3+ ions is described as oxidation [1]

(iii) The oxidising agent for the conversion of Fe2+ ions to Fe3+ ions is aqueous potassium manganate(VII).

State one condition needed for the oxidation to take place [1]

(e) Iodide ions, I– , reduce Fe3+ ions to Fe2+ ions in aqueous solution.

Suggest the identity of the other product formed in this reaction [1]

[Total: 19] , ,

3 A student prepares a sample of the insoluble salt barium sulfate, BaSO4.

The student adds aqueous sodium sulfate, Na2SO4(aq), to aqueous barium chloride, BaCl 2(aq).

The student carries out the following steps.

step 1 Dissolve 0.100 moles of solid BaCl 2 in 100 cm3 of distilled water in a beaker to form BaCl 2(aq).

step 2 Add an aqueous solution which contains 0.100 moles of Na2SO4(aq) to the beaker containing the BaCl 2(aq) from step 1.

step 3 Stir the mixture and then filter it.

step 4 Dry the solid left in the filter paper.

(a) Complete the symbol equation for the reaction. Include state symbols. BaCl 2(aq) + Na2SO4(aq) BaSO4( ) + ( )

[2]

(b) Calculate the mass of solid BaCl 2 dissolved in step 1.

mass = g [2]

(c) The concentration of Na2SO4(aq) in step 2 is 1.25 mol / dm3.

Calculate the volume, in cm3, of 1.25 mol / dm3 Na2SO4(aq) added in step 2 which contains 0.100 moles of Na2SO4 .

volume = cm3 [1]

(d) State the colour of the solid formed in step 2 [1]

(e) The mixture is filtered in step 3.

State the general term given to a solid left in the filter paper after filtration [1] , ,

(f) The actual mass of dry BaSO4 collected in step 4 is greater than the expected mass. This is because the student should do an additional step between step 3 and step 4.

Suggest what the student should do in this additional step, and explain why the actual mass collected is greater than the expected mass [2]

(g) State the name of this method of salt preparation [1]

(h) State the name of a different: • barium salt that can be used in place of BaCl 2 • sulfate salt that can be used in place of Na2SO4 • barium salt that can be made by this method [3]

[Total: 13] , ,

4 Nitric acid, HNO3 , and sulfuric acid, H2SO4 , are strong acids. Ethanoic acid, CH3COOH, is a weak acid.

(a) One mole of each acid is added separately to 1000 cm3 of distilled water to form a dilute solution. All three acids dissociate in distilled water.

(i) State the formula of the common cation produced when each of the three acids dissociates in water [1]

(ii) Explain, in terms of dissociation, why: • nitric acid is described as a strong acid • ethanoic acid is described as a weak acid [2]

(iii) State which of the three dilute acids will have the highest pH value [1]

(iv) State the colour of thymolphthalein in all three dilute acids [1]

(v) Give the formula of the anion formed when: • sulfuric acid dissociates in water • ethanoic acid dissociates in water [2]

(vi) Name the two gaseous products formed during the electrolysis of dilute sulfuric acid using inert electrodes and [2]

(vii) Name the salt formed when calcium reacts with ethanoic acid [1] , ,

(b) Aluminium nitrate, Al (NO3)3 , is made when dilute nitric acid reacts with aluminium hydroxide, Al (OH)3 .

(i) Al (OH)3 acts as a base in this reaction.

Define the term base [1]

(ii) Al (OH)3 is not an alkali.

State what this tells you about the solubility of Al (OH)3 [1]

(iii) Name one other compound which forms aluminium nitrate when added to dilute nitric acid [1]

(iv) The oxidation number of the O atoms in Al (NO3)3 is –2.

The formula of the aluminium ion in Al (NO3)3 is Al 3+.

Determine the oxidation number of the N atoms in Al (NO3)3.

Show your working.

oxidation number of N = [2]

[Total: 15] , ,

5 This question is about the homologous series of alkanes.

Three general characteristics of alkanes are: • they are generally unreactive because they do not have a functional group • they show trends in their physical properties, such as melting points and boiling points • they have similar chemical properties.

(a) Describe two other general characteristics of the homologous series of alkanes. 1 2 [2]

(b) (i) State the trend in the boiling points of the alkanes as the carbon chain length increases [1]

(ii) Name one other physical property of alkanes that shows a trend, other than melting points and boiling points.

Describe this trend as the carbon chain length of alkanes increases. name description [2]

(c) State why alkanes are described as saturated [1] , ,

(d) Propane has the structural formula CH3CH2CH3 .

When propane undergoes a monosubstitution reaction with chlorine at room temperature, two organic products can be formed.

(i) State one condition needed for this substitution reaction to take place [1]

(ii) Give the structural formula and state the name of each organic product formed. • structural formula of product 1 name of product 1 • structural formula of product 2 name of product 2 [4]

(iii) The two products formed are structural isomers of each other.

Define the term structural isomers [1]

[Total: 12] , ,

6 Compound E shown in Fig. 6.1 is an ester. CH3 CH2 CH2 CH2 CH3 O O C Fig. 6.1

(a) On Fig. 6.1, draw a circle around all the atoms which make up the ester linkage. [1]

(b) Name compound E [1]

(c) Deduce the empirical formula of compound E [1]

(d) Compound E is produced when two different compounds react together in the presence of a catalyst.

(i) Name the two compounds that react together to produce compound E. 1 2 [2]

(ii) Suggest a suitable catalyst for this reaction [1]

(e) Determine the number of unbranched esters which have the molecular formula C5H10O2 [1]

(f) All unbranched esters with the molecular formula C5H10O2 combust completely to form carbon dioxide and water only.

Write the symbol equation for the complete combustion of C5H10O2 [1]

[Total: 8] , , Group The Periodic Table of Elements 1 H hydrogen 1 2 He helium 4 I II III IV V VI VII VIII 3 Li lithium 7 4 Be beryllium 9 atomic number atomic symbol Key name relative atomic mass 11 Na sodium 23 12 Mg magnesium 24 19 K potassium 39 20 Ca calcium 40 37 Rb rubidium 85 38 Sr strontium 88 55 Cs caesium 133 56 Ba barium 137 87 Fr francium – 88 Ra radium – 5 B boron 11 13 Al aluminium 27 31 Ga gallium 70 49 In indium 115 81 Tl thallium 204 113 Nh nihonium – 6 C carbon 12 14 Si silicon 28 32 Ge germanium 73 50 Sn tin 119 82 Pb lead 207 22 Ti titanium 48 40 Zr zirconium 91 72 Hf hafnium 178 104 Rf rutherfordium – 23 V vanadium 51 41 Nb niobium 93 73 Ta tantalum 181 105 Db dubnium – 24 Cr chromium 52 42 Mo molybdenum 96 74 W tungsten 184 106 Sg seaborgium – 25 Mn manganese 55 43 Tc technetium – 75 Re rhenium 186 107 Bh bohrium – 26 Fe iron 56 44 Ru ruthenium 101 76 Os osmium 190 108 Hs hassium – 27 Co cobalt 59 45 Rh rhodium 103 77 Ir iridium 192 109 Mt meitnerium – 28 Ni nickel 59 46 Pd palladium 106 78 Pt platinum 195 110 Ds darmstadtium – 29 Cu copper 64 47 Ag silver 108 79 Au gold 197 111 Rg roentgenium – 30 Zn zinc 65 48 Cd cadmium 112 80 Hg mercury 201 112 Cn copernicium – 114 Fl flerovium – 116 Lv livermorium – 7 N nitrogen 14 15 P phosphorus 31 33 As arsenic 75 51 Sb antimony 122 83 Bi bismuth 209 115 Mc moscovium – 8 O oxygen 16 16 S sulfur 32 34 Se selenium 79 52 Te tellurium 128 84 Po polonium – 9 F fluorine 19 17 Cl chlorine 35.5 35 Br bromine 80 53 I iodine 127 85 At astatine – 117 Ts tennessine – 10 Ne neon 20 18 Ar argon 40 36 Kr krypton 84 54 Xe xenon 131 86 Rn radon – 118 Og oganesson – 21 Sc scandium 45 39 Y yttrium 89 57–71 lanthanoids 89–103 actinoids 57 La lanthanum 139 89 Ac lanthanoids actinoids The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.). actinium – 58 Ce cerium 140 90 Th thorium 232 59 Pr praseodymium 141 91 Pa protactinium 231 60 Nd neodymium 144 92 U uranium 238 61 Pm promethium – 93 Np neptunium – 62 Sm samarium 150 94 Pu plutonium – 63 Eu europium 152 95 Am americium – 64 Gd gadolinium 157 96 Cm curium – 65 Tb terbium 159 97 Bk berkelium – 66 Dy dysprosium 163 98 Cf californium – 67 Ho holmium 165 99 Es einsteinium – 68 Er erbium 167 100 Fm fermium – 69 Tm thulium 169 101 Md mendelevium – 70 Yb ytterbium 173 102 No nobelium – 71 Lu lutetium 175 103 Lr lawrencium – , ,