Lesson 14.1.2

14.1.2 Cell emf and cell diagrams Quiz: Pearson Edexcel Chemistry, Unit 14

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 14.1.2, Cell emf and cell diagrams: 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. By convention, which half-cell reaction is written on the left side of a cell diagram?

    • Neutralisation
    • Precipitation
    • Oxidation
    • Reduction

  2. What feature does a single vertical line represent in a standard electrochemical cell diagram?

    • Gaseous state
    • Liquid junction
    • Salt bridge
    • Phase boundary

  3. What feature does a double vertical line represent in a standard electrochemical cell diagram?

    • Phase boundary
    • Salt bridge
    • Platinum electrode
    • Wire connection

  4. Which expression calculates the standard emf of an electrochemical cell from half-cell potentials?

    • E°cathode + E°anode
    • E°anode × E°cathode
    • E°anode - E°cathode
    • E°cathode - E°anode

  5. Which electrode in an electrochemical cell acts as the cathode?

    • Leftmost electrode
    • More positive E°
    • More negative E°
    • Zero electrode potential

  6. What sign must the standard cell emf have for a reaction to be thermodynamically feasible?

    • Negative
    • Neutral
    • Zero
    • Positive

  7. What is the primary function of a salt bridge in an electrochemical cell?

    • Transfers hydrogen gas
    • Measures cell emf
    • Allows ion flow
    • Allows electron flow

  8. Using Ni2+/Ni (E-zero -0.25 V) and Ag+/Ag (E-zero +0.80 V), what is the standard emf of the cell Ni | Ni2+ || Ag+ | Ag?

    • +1.05 V
    • -1.05 V
    • +0.25 V
    • +0.55 V

  9. Which cell diagram represents the reaction where Ni is oxidised and Ag+ is reduced?

    • Ni2+|Ni||Ag|Ag+
    • Ag+|Ag||Ni|Ni2+
    • Ag|Ag+||Ni2+|Ni
    • Ni|Ni2+||Ag+|Ag

  10. Using E-zero Fe2+/Fe = -0.44 V and E-zero Cu2+/Cu = +0.34 V, what is the emf of the cell Fe | Fe2+ || Cu2+ | Cu?

    • +0.10 V
    • +0.78 V
    • +0.34 V
    • -0.78 V

  11. What is ΔG° for a two-electron cell reaction with E°cell = +0.78 V?

    • +151 kJ mol-1
    • -75 kJ mol-1
    • +75 kJ mol-1
    • -151 kJ mol-1

  12. What does a negative E°cell value indicate about the forward reaction?

    • At equilibrium
    • Extremely fast
    • Feasible
    • Non-feasible

  13. In the cell Zn | Zn²⁺ || Cu²⁺ | Cu, which electrode acts as the negative terminal?

    • Zinc ion
    • Zinc
    • Copper
    • Copper ion

  14. What is the cell emf of a cell constructed from two identical half-cells?

    • -1.10 V
    • +0.50 V
    • +1.10 V
    • 0.00 V

  15. In the cell Zn | Zn²⁺ || Cu²⁺ | Cu, which process occurs at the cathode?

    • Reduction of Zn²⁺
    • Oxidation of Cu
    • Oxidation of Zn
    • Reduction of Cu²⁺

  16. Using the half-cells MnO4-/Mn2+ (E-zero +1.51 V) as cathode and Fe3+/Fe2+ (E-zero +0.77 V) as anode, what is the standard emf?

    • +0.23 V
    • +2.28 V
    • +0.74 V
    • -0.74 V

  17. Which equation relates standard cell potential (E°cell) to the equilibrium constant (K)?

    • ln K = nFE° / RT
    • ln K = -nFE° / RT
    • ln K = RT / nFE°
    • K = nFE° / RT

  18. For a two-electron cell with E-zero cell = +0.50 V at 298 K, what is K approximately?

    • About 1 x 10^2
    • About 0.50
    • About 39
    • About 8 x 10^16

  19. Why does measuring a cell under non-standard concentrations alter its cell potential?

    • Electrode mass changes
    • Concentration changes potentials
    • Activation energy changes
    • Equilibrium constant changes

  20. What is the cell potential when a cell reaction reaches chemical equilibrium?

    • +1.10 V
    • -1.10 V
    • 0 V
    • Maximum positive value

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