Paper 1-style (Higher)
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Paper 1-style practice paper: Higher — question paper

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GCSE (9–1) · GCSE Chemistry (Higher)

Paper 1-style practice paper

Higher

Duration: 105 minutes
Total: 100 marks
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READ THESE INSTRUCTIONS FIRST

  • Answer all questions.
  • Section A contains ten multiple-choice questions. Choose one answer, A, B, C or D, for each.
  • Section B contains structured questions. Write your answers in the spaces provided.
  • You may use a calculator. Values of relative atomic/formula mass and bond energies are given where needed.
  • The number of marks is given in brackets [ ] at the end of each question or part question.
  • The total mark for this paper is 100.

Original practice material written for the MOE GCSE Chemistry syllabus. It is not an official MOE or school examination paper. Foundation and Higher content of chapters 1–11: atomic structure and the periodic table, bonding and ionic equations, allotropes and nanoparticles, moles and molar gas volume, acids and titrations in mol/dm³, electrolysis half equations, reactivity and extraction, bond energy calculations, cells and fuel cells.

For Examiner’s Use
Section A/ 10
Section B/ 90
Total/ 100

Section A: Multiple-choice questions[10 marks]

Choose one answer for each question. Each question is worth 1 mark.

  1. 1

    The relative charge of an electron is

    1. A+1
    2. B−1
    3. C0
    4. D+2
    ( )
  2. 2

    The isotopes ³⁵Cl and ³⁷Cl differ in their number of

    1. Aprotons
    2. Belectrons
    3. Cneutrons
    4. Dbonds
    ( )
  3. 3

    In the balanced equation 2Mg + O₂ → 2MgO, the coefficient of MgO is

    1. A1
    2. B2
    3. C3
    4. D4
    ( )
  4. 4

    The number of moles in 8 g of methane (Mr = 16) is

    1. A0.25
    2. B2
    3. C1
    4. D0.5
    ( )
  5. 5

    The molar gas volume at room temperature and pressure is

    1. A24 dm³ per mole
    2. B24 cm³ per mole
    3. C2.4 dm³ per mole
    4. D1 dm³ per mole
    ( )
  6. 6

    The ionic equation for neutralisation is

    1. AH⁺ + Cl⁻ → HCl
    2. BNa⁺ + OH⁻ → NaOH
    3. CH⁺ + OH⁻ → H₂O
    4. DH₂ + O₂ → H₂O
    ( )
  7. 7

    0.1 mol of solute in 250 cm³ of solution has a concentration of

    1. A0.4 mol/dm³
    2. B0.025 mol/dm³
    3. C4 mol/dm³
    4. D25 mol/dm³
    ( )
  8. 8

    At the cathode during electrolysis of molten PbBr₂, the half equation is

    1. APb²⁺ → Pb + 2e⁻
    2. B2Br⁻ → Br₂ + 2e⁻
    3. CPb + 2e⁻ → Pb²⁺
    4. DPb²⁺ + 2e⁻ → Pb
    ( )
  9. 9

    Using bond energies (H–H 436, Cl–Cl 242, H–Cl 431 kJ/mol), ΔH for H₂ + Cl₂ → 2HCl is

    1. A−184 kJ/mol
    2. B+184 kJ/mol
    3. C−678 kJ/mol
    4. D−862 kJ/mol
    ( )
  10. 10

    The overall equation for a hydrogen–oxygen fuel cell is

    1. AH₂ → 2H⁺ + 2e⁻
    2. B2H₂O → 2H₂ + O₂
    3. C2H₂ + O₂ → 2H₂O
    4. DH₂ + O₂ → H₂O₂
    ( )

Section B: Structured questions[90 marks]

Answer all questions in the spaces provided.

  1. 11

    This question is about the periodic table.

    1. (a)

      Explain why the reactivity of Group 1 metals increases down the group.

      [3]
    2. (b)

      Write the balanced equation, with state symbols, for potassium reacting with water.

      [3]
    3. (c)

      Bromine is added to solutions of potassium chloride and potassium iodide. State and explain what happens in each.

      [2]
  2. 12

    This question is about bonding and equations.

    1. (a)

      Describe, in terms of electrons, the formation of magnesium chloride from magnesium atoms and chlorine atoms.

      [3]
    2. (b)

      Write the ionic equation, with state symbols, for the precipitation of silver chloride when silver nitrate solution is added to sodium chloride solution.

      [2]
    3. (c)

      Give three limitations of the particle models used for atoms and molecules.

      [3]
  3. 13

    This question is about nanoparticles. A cube has sides of 0.1 cm.

    1. (a)

      Calculate the surface area to volume ratio of a 1 cm cube.

      [2]
    2. (b)

      Calculate the surface area to volume ratio of a 0.1 cm cube.

      [3]
    3. (c)

      Use your answers to explain one use of nanoparticles and one possible risk.

      [3]
  4. 14

    This question is about quantitative chemistry. (Mr: CaCO₃ = 100, CO₂ = 44)

    1. (a)

      Write the balanced equation, with state symbols, for calcium carbonate reacting with hydrochloric acid.

      [3]
    2. (b)

      Write the ionic equation for the reaction of any carbonate with dilute acid.

      [2]
    3. (c)

      In a reaction between two solutions in an open beaker, the recorded mass falls by 0.44 g. Explain the observation.

      [3]
  5. 15

    This question is about the mole. (Ar: Na = 23, Cl = 35.5, H = 1; molar gas volume = 24 dm³ at RTP; Avogadro constant = 6.02 × 10²³)

    1. (a)

      Calculate the number of moles in 8 g of sodium hydroxide (Mr = 40).

      [2]
    2. (b)

      4.6 g of sodium burns in chlorine to make sodium chloride (Mr = 58.5): 2Na + Cl₂ → 2NaCl. Calculate the mass of sodium chloride formed.

      [4]
    3. (c)

      Calculate the volume of 0.25 mol of hydrogen gas at RTP.

      [2]
    4. (d)

      Calculate the number of atoms in 0.2 mol of sodium.

      [1]
  6. 16

    This question is about titrations. 25.0 cm³ of sodium hydroxide solution is neutralised by 20.0 cm³ of 0.50 mol/dm³ hydrochloric acid.

    1. (a)

      Describe the titration technique, including the choice of indicator.

      [4]
    2. (b)

      Calculate the number of moles of hydrochloric acid used.

      [2]
    3. (c)

      Calculate the concentration of the sodium hydroxide in mol/dm³ (HCl + NaOH → NaCl + H₂O).

      [2]
  7. 17

    This question is about electrolysis.

    1. (a)

      Write the half equations for the electrodes during electrolysis of molten lead bromide.

      [4]
    2. (b)

      Explain why hydrogen, not sodium, is produced at the cathode during electrolysis of concentrated aqueous sodium chloride.

      [2]
    3. (c)

      Write the half equation for the oxygen formed at the anode from hydroxide ions.

      [2]
  8. 18

    This question is about energy changes. Bond energies: H–H 436, Cl–Cl 242, H–Cl 431 kJ/mol.

    1. (a)

      Sketch or describe the reaction profile of an exothermic reaction, labelling ΔH and the activation energy.

      [3]
    2. (b)

      Calculate ΔH for H₂ + Cl₂ → 2HCl using the bond energies given.

      [4]
    3. (c)

      Explain, in terms of bonds, why the reaction is exothermic.

      [2]
  9. 19

    This question is about metals and their extraction.

    1. (a)

      Zinc displaces copper from copper sulfate solution. Write the ionic equation for this reaction and identify the species that is oxidised.

      [3]
    2. (b)

      Explain why potassium cannot be extracted from its ore by reduction with carbon.

      [2]
    3. (c)

      Give two advantages and one disadvantage of using bacteria (bioleaching/phytomining) to extract copper from low-grade ores.

      [3]
    4. (d)

      Explain why a metal’s conductivity increases when it is pure but its hardness increases when it is alloyed.

      [4]
  10. 20

    This question is about making and using chemicals.

    1. (a)

      Describe how to make a pure, dry sample of the insoluble salt lead sulfate from lead nitrate solution and sodium sulfate solution.

      [4]
    2. (b)

      0.2 mol of sodium contains how many atoms? Show your working.

      [2]
    3. (c)

      Explain why solid sodium chloride does not conduct electricity but molten sodium chloride does.

      [3]
    4. (d)

      A hydrogen–oxygen fuel cell is used in a bus. Write the two half equations (acidic electrolyte) and explain one advantage of the fuel cell over a petrol engine.

      [3]

— End of paper —