Lesson 14.1.1

14.1.1 Standard electrode potentials and the hydrogen electrode Quiz: Pearson Edexcel Chemistry, Unit 14

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 14.1.1, Standard electrode potentials and the hydrogen electrode: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 14: Redox II, written with Revision Ninja.

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The 20 questions

  1. What is the assigned standard electrode potential of the standard hydrogen electrode?

    • +1.00 V
    • +0.10 V
    • -1.00 V
    • 0.00 V

  2. Why must standard electrode potentials be measured relative to a reference electrode?

    • Voltage changes rapidly
    • Hydrogen is reactive
    • Current flow varies
    • Absolute values impossible

  3. What standard pressure is used when measuring standard electrode potentials?

    • 1 kPa
    • 100 kPa
    • 101 kPa
    • 100 atm

  4. Against which reference electrode are standard electrode potentials measured?

    • Standard zinc electrode
    • Standard hydrogen electrode
    • Standard calomel electrode
    • Standard copper electrode

  5. What does a more negative standard electrode potential indicate about a species?

    • Less easily oxidised
    • Stronger oxidising agent
    • Stronger reducing agent
    • Weaker reducing agent

  6. Which metal is the strongest reducing agent: Mg (E° = -2.37 V), Zn (-0.76 V), or Cu (+0.34 V)?

    • Zinc
    • Magnesium
    • Hydrogen
    • Copper

  7. What is the standard electrode potential of the standard hydrogen electrode?

    • -0.76 V, the Zn2+/Zn value
    • 0.00 V, by definition
    • +1.00 V, a concentration reference
    • +0.34 V, the Cu2+/Cu value

  8. What is the standard cell emf for a Zn/Zn2+ half-cell (E-zero -0.76 V) connected to a Cu2+/Cu half-cell (E-zero +0.34 V), with Cu2+ reduced?

    • +0.42 V
    • +1.10 V
    • +0.76 V
    • -1.10 V

  9. What is E°cell for chlorine oxidising Fe²⁺ to Fe³⁺ (E° Cl₂/Cl⁻ = +1.36 V, Fe³⁺/Fe²⁺ = +0.77 V)?

    • +0.59 V
    • +2.13 V
    • -0.59 V
    • -2.13 V

  10. Which standard cell diagram represents a cell formed from Zn²⁺/Zn and Cu²⁺/Cu electrodes?

    • Zn(s)|Zn²⁺(aq)||Cu²⁺(aq)|Cu(s)
    • Cu²⁺(aq)|Cu(s)||Zn(s)|Zn²⁺(aq)
    • Cu(s)|Cu²⁺(aq)||Zn²⁺(aq)|Zn(s)
    • Zn²⁺(aq)|Zn(s)||Cu(s)|Cu²⁺(aq)

  11. Using E-zero Mg2+/Mg = -2.37 V and Ag+/Ag = +0.80 V, what is the standard emf of Mg + 2Ag+ gives Mg2+ + 2Ag?

    • -1.57 V
    • +3.17 V
    • -3.17 V
    • +1.57 V

  12. Why might a reaction with a positive E°cell value fail to occur at a measurable rate?

    • High activation energy
    • Endothermic reaction
    • Low reactant concentration
    • Negative cell potential

  13. How does increasing the concentration of Zn2+ ions affect the electrode potential of a Zn2+/Zn half-cell?

    • More positive
    • No effect
    • Zero potential
    • More negative

  14. Which metal can displace iron from an aqueous Fe2+ solution given E°(Fe2+/Fe) = -0.44 V?

    • Lead
    • Copper
    • Silver
    • Zinc

  15. What is the standard emf of a Zn/Zn2+ half-cell (E-zero -0.76 V) connected to Ag+/Ag (E-zero +0.80 V)?

    • +1.56 V
    • +0.04 V
    • +0.76 V
    • -1.56 V

  16. What role does platinum play in the standard hydrogen electrode?

    • Inert electrode conductor
    • Decreases pH value
    • Acts as oxidant
    • Reacts with hydrogen

  17. What is E°cell for Sn | Sn2+ || Pb2+ | Pb given E°(Sn2+/Sn) = -0.14 V and E°(Pb2+/Pb) = -0.13 V?

    • -0.27 V
    • -0.01 V
    • +0.27 V
    • +0.01 V

  18. What is the standard aqueous ion concentration required for measuring standard electrode potentials?

    • 0.50 mol dm-3
    • 0.10 mol dm-3
    • 2.00 mol dm-3
    • 1.00 mol dm-3

  19. By convention, how are standard electrode potential half-equations always written?

    • Redox reactions
    • Neutralisation equations
    • Oxidation half-equations
    • Reduction half-equations

  20. What is the standard emf for Mg (anode, E-zero -2.37 V) and Zn2+/Zn (cathode, -0.76 V) with the magnesium oxidised?

    • +1.61 V
    • +3.13 V
    • -1.61 V
    • +0.61 V

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