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Redox and standard electrode potential: Eduqas A‑Level Chemistry questions

Every Eduqas A-Level Chemistry exam question on PI1.1 Redox and standard electrode potential, 2016–2025, with its mark scheme and examiner’s report.

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1,513 questions

  1. Q12(d)(ii)

    June 2025 · Component 1

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2025 Component 1, question 12(d)(ii): Suitable ligands must be chosen for the reaction to prevent the copper(I) ions precipitating as Cu2O(s) or undergoing disproportionation. State what is meant by

  2. Q12(d)(v)

    June 2025 · Component 1

    4 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2025 Component 1, question 12(d)(v): Copper(I) complexes such as [Cu(CN)2]– can act as reducing agents for other metal ions. Standard electrode potential, E θ / V Pr4+ + e– Pr3+ +3.21 Mn3+ + e– Mn2

  3. Q9(c)(ii)

    June 2024 · Component 1

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 1, question 9(c)(ii): Give the oxidation state of the chlorine atom in this molecule. [1]

  4. Q11(b)(i)

    June 2024 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 1, question 11(b)(i): State what is meant by the term standard electrode potential. [2]

  5. Q11(b)(ii)

    June 2024 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 1, question 11(b)(ii): The table below shows the standard electrode potentials for some metal ions. Standard electrode potential, E θ/ V Co3+ + e– Co2+ +1.82 Mn3+ + e– Mn2+ +1.51 Fe3+

  6. Q12(e)(i)

    June 2024 · Component 1

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 1, question 12(e)(i): Identify the oxidation state of the iron in chukanovite. Give a reason for your answer. [1]

  7. Q2(b)(i)

    June 2024 · Component 3

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 3, question 2(b)(i): Give the half-equation for the reaction occurring at the negative electrode. [1]

  8. Q2(b)(ii)

    June 2024 · Component 3

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 3, question 2(b)(ii): Give the observation at the positive electrode after the cell has been connected for a period of time. [1]

  9. Q2(b)(iii)

    June 2024 · Component 3

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 3, question 2(b)(iii): Give the overall equation for the cell reaction. Identify the oxidising agent and the reducing agent. [2] Equation Oxidising agent Reducing agent

  10. Q2(b)(iv)

    June 2024 · Component 3

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2024 Component 3, question 2(b)(iv): The concentrations of the Cr2+ / Cr3+ and Fe3+ / Fe2+ ions are all 1.0 mol dm–3 State and explain how the value on a high-resistance voltmeter would change if t

  11. Q11(e)

    Autumn 2021 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    Autumn 2021 Component 1, question 11(e): The table below lists the standard electrode potentials for some redox systems. Standard electrode potential, Eθ / V H3PO3 + 2H+ + 2e– s H3PO2 + H2O –0.50 Cu2+

  12. Q12(a)(iii)

    Autumn 2021 · Component 1

    9 marksC2.2 ThermochemistryPI1.1 Redox and standard electrode potential
    The whole paper ↗
    Autumn 2021 Component 1, question 12(a)(iii): The final step is shown below. 2HNO3(aq) + NO(g) ΔHθ = −117 kJ mol–1 3NO2(g) + H2O(l) I. Use oxidation states to show that this is a disproportionation reaction

  13. Q6

    Autumn 2020 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    Autumn 2020 Component 1, question 6: Iron metal reacts with chlorine to form iron(III) chloride and it reacts with iodine to form iron(II) iodide. Use the standard electrode potentials below to exp

  14. Q11(a)

    Autumn 2020 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    Autumn 2020 Component 1, question 11(a): Give one advantage and one disadvantage of the use of fuel cells. [2] Advantage Disadvantage

  15. Q12(c)(i)

    Autumn 2020 · Component 1

    1 markPI1.1 Redox and standard electrode potential
    The whole paper ↗
    Autumn 2020 Component 1, question 12(c)(i): State what is meant by a reducing agent. [1]

  16. Q13(b)(iv)

    June 2019 · Component 1

    4 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2019 Component 1, question 13(b)(iv): Hydrazine can undergo both oxidation and reduction reactions. Electrochemical potentials for both processes are included in the table below. Standard electrode

  17. Q7(b)

    June 2018 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2018 Component 1, question 7(b): Use oxidation states to explain why this is a disproportionation reaction. [2]

  18. Q8

    June 2018 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2018 Component 1, question 8: Standard electrode potentials are measured by comparison with the standard hydrogen electrode. Describe the standard hydrogen electrode. You may include a diagr

  19. Q6

    June 2017 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2017 Component 1, question 6: Carbon monoxide can be used as a reducing agent. Explain why carbon monoxide is a reducing agent and give an equation for a reaction where carbon monoxide acts

  20. Q11(d)(ii)

    June 2017 · Component 1

    2 marksPI1.1 Redox and standard electrode potential
    The whole paper ↗
    June 2017 Component 1, question 11(d)(ii): Sodium can also form an oxide with formula Na2O2. Deduce the oxidation state of the oxygen in this compound, and use it to show that its reaction with water is
All 31 questions on Redox and standard electrode potential, as a list
  1. June 2025, Component 1, Q12(d)(ii) (1 mark): Suitable ligands must be chosen for the reaction to prevent the copper(I) ions precipitating as Cu2O(s) or undergoing disproportionation. State what is meant by
  2. June 2025, Component 1, Q12(d)(v) (4 marks): Copper(I) complexes such as [Cu(CN)2]– can act as reducing agents for other metal ions. Standard electrode potential, E θ / V Pr4+ + e– Pr3+ +3.21 Mn3+ + e– Mn2
  3. June 2024, Component 1, Q9(c)(ii) (1 mark): Give the oxidation state of the chlorine atom in this molecule. [1]
  4. June 2024, Component 1, Q11(b)(i) (2 marks): State what is meant by the term standard electrode potential. [2]
  5. June 2024, Component 1, Q11(b)(ii) (2 marks): The table below shows the standard electrode potentials for some metal ions. Standard electrode potential, E θ/ V Co3+ + e– Co2+ +1.82 Mn3+ + e– Mn2+ +1.51 Fe3+
  6. June 2024, Component 1, Q12(e)(i) (1 mark): Identify the oxidation state of the iron in chukanovite. Give a reason for your answer. [1]
  7. June 2024, Component 3, Q2(b)(i) (1 mark): Give the half-equation for the reaction occurring at the negative electrode. [1]
  8. June 2024, Component 3, Q2(b)(ii) (1 mark): Give the observation at the positive electrode after the cell has been connected for a period of time. [1]
  9. June 2024, Component 3, Q2(b)(iii) (2 marks): Give the overall equation for the cell reaction. Identify the oxidising agent and the reducing agent. [2] Equation Oxidising agent Reducing agent
  10. June 2024, Component 3, Q2(b)(iv) (1 mark): The concentrations of the Cr2+ / Cr3+ and Fe3+ / Fe2+ ions are all 1.0 mol dm–3 State and explain how the value on a high-resistance voltmeter would change if t
  11. Autumn 2021, Component 1, Q11(e) (2 marks): The table below lists the standard electrode potentials for some redox systems. Standard electrode potential, Eθ / V H3PO3 + 2H+ + 2e– s H3PO2 + H2O –0.50 Cu2+
  12. Autumn 2021, Component 1, Q12(a)(iii) (9 marks): The final step is shown below. 2HNO3(aq) + NO(g) ΔHθ = −117 kJ mol–1 3NO2(g) + H2O(l) I. Use oxidation states to show that this is a disproportionation reaction
  13. Autumn 2020, Component 1, Q6 (2 marks): Iron metal reacts with chlorine to form iron(III) chloride and it reacts with iodine to form iron(II) iodide. Use the standard electrode potentials below to exp
  14. Autumn 2020, Component 1, Q11(a) (2 marks): Give one advantage and one disadvantage of the use of fuel cells. [2] Advantage Disadvantage
  15. Autumn 2020, Component 1, Q12(c)(i) (1 mark): State what is meant by a reducing agent. [1]
  16. June 2019, Component 1, Q13(b)(iv) (4 marks): Hydrazine can undergo both oxidation and reduction reactions. Electrochemical potentials for both processes are included in the table below. Standard electrode
  17. June 2018, Component 1, Q7(b) (2 marks): Use oxidation states to explain why this is a disproportionation reaction. [2]
  18. June 2018, Component 1, Q8 (2 marks): Standard electrode potentials are measured by comparison with the standard hydrogen electrode. Describe the standard hydrogen electrode. You may include a diagr
  19. June 2017, Component 1, Q6 (2 marks): Carbon monoxide can be used as a reducing agent. Explain why carbon monoxide is a reducing agent and give an equation for a reaction where carbon monoxide acts
  20. June 2017, Component 1, Q11(d)(ii) (2 marks): Sodium can also form an oxide with formula Na2O2. Deduce the oxidation state of the oxygen in this compound, and use it to show that its reaction with water is
  21. June 2017, Component 1, Q14(a)(i) (1 mark): State the function of the salt bridge. [1]
  22. June 2017, Component 1, Q14(a)(ii) (3 marks): Draw a labelled diagram of the standard hydrogen electrode. [3]
  23. June 2017, Component 1, Q14(a)(iii) (1 mark): When measuring the standard electrode potential for the Zn2+(aq) │ Zn(s) system a piece of zinc metal is placed in an aqueous solution containing Zn2+(aq). Expl
  24. June 2017, Component 1, Q14(b)(i) (1 mark): Give the formula of the strongest reducing agent in the table. [1]
  25. June 2017, Component 1, Q14(b)(ii) (2 marks): Calculate the EMF of the cell formed when the Br2(l) │ Br −(aq) half-cell is connected to the Zn2+(aq) │ Zn(s) half-cell. [2] EMF = V
  26. June 2017, Component 1, Q14(b)(iii) (6 marks): Use the values in the table to explain why the reaction between gaseous iodine and heated iron wire produces iron(II) iodide whilst chlorine gas and iron wire p
  27. June 2017, Component 1, Q15(a) (3 marks): A lithium ion battery can sustain a current over an extended period of time so that a total charge of 1.2 × 104 C has flowed. Calculate the mass of lithium that
  28. June 2017, Component 3, Q3(a) (1 mark): Suggest how the student made the salt bridge. [1]
  29. June 2017, Component 3, Q3(b) (2 marks): Write an equation for the overall cell reaction and calculate the standard cell potential for this cell. [2] Standard cell potential = V
  30. June 2017, Component 3, Q3(c) (2 marks): Describe one observation the student would have made in each half-cell after the cell had been connected for a period of time. [2] Half-cell A Half-cell B
  31. June 2017, Component 3, Q3(d) (1 mark): The student measured the cell potential and found that it was different from the value calculated in (b). Suggest a reason for this. [1]

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