Lesson 14.1.3

14.1.3 Feasibility, limitations and the electrochemical series Quiz: Pearson Edexcel Chemistry, Unit 14

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 14.1.3, Feasibility, limitations and the electrochemical series: 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. How are standard electrode potentials arranged in the electrochemical series?

    • Most positive to negative
    • Most negative to positive
    • Highest mass to lowest
    • Random order

  2. Where in the electrochemical series is the strongest reducing agent located?

    • E° value of zero
    • Most positive E° value
    • Middle of series
    • Most negative E° value

  3. Where in the electrochemical series is the strongest oxidising agent located?

    • Middle of series
    • Most positive E° value
    • E° value of zero
    • Most negative E° value

  4. Metal A displaces metal B from solution if metal A has what property?

    • More positive E° value
    • Higher electrode mass
    • More negative E° value
    • Equal E° value

  5. What happens to an element during a disproportionation reaction?

    • Oxidised and reduced
    • Only oxidised
    • Only reduced
    • Neither oxidised nor reduced

  6. Why might a thermodynamically feasible reaction fail to occur at a noticeable rate?

    • Zero activation energy
    • High activation energy
    • Negative cell potential
    • Low activation energy

  7. Which standard condition is violated if aqueous ion concentrations are not 1.00 mol dm⁻³?

    • Standard temperature
    • Standard state
    • Standard concentration
    • Standard pressure

  8. Given E°(Cu⁺/Cu) = +0.52 V and E°(Cu²⁺/Cu⁺) = +0.15 V, calculate E°cell for Cu⁺ disproportionation.

    • +0.37 V
    • -0.67 V
    • +0.67 V
    • -0.37 V

  9. Which species is the strongest oxidising agent given these standard electrode potentials?

    • Zn
    • Cu2+
    • Ag+
    • Zn2+

  10. Which species is the stronger oxidising agent: Cr2O72- (+1.33 V) or Fe3+ (+0.77 V)?

    • Cr2O72-
    • Fe3+
    • Cr3+
    • Fe2+

  11. What is the E cell value for chlorine oxidising bromide ions under standard conditions?

    • Yes, +2.43 V
    • Yes, +0.29 V
    • No, -0.29 V
    • No, -2.43 V

  12. What is E cell for bromine oxidising iodide ions under standard conditions?

    • -1.61 V
    • -0.53 V
    • +0.53 V
    • +1.61 V

  13. What is the calculated standard cell potential for the decomposition of hydrogen peroxide?

    • +2.45 V
    • -2.45 V
    • -1.09 V
    • +1.09 V

  14. Which ion is most easily reduced given standard electrode potentials: Fe3+ (+0.77 V) or Sn2+ (-0.14 V)?

    • Fe3+
    • Fe2+
    • Sn
    • Sn2+

  15. Which metal can displace hydrogen gas from dilute acid under standard conditions?

    • Copper
    • Gold
    • Silver
    • Zinc

  16. Why might a reaction with a positive cell potential not occur at a measurable rate?

    • Low concentration
    • Negative enthalpy change
    • High activation energy
    • Low equilibrium constant

  17. How does decreasing reactant concentration affect the measured electrode potential of a half-cell?

    • It stays constant
    • It becomes zero
    • It decreases
    • It increases

  18. Using E-zero(O2/H2O) = +1.23 V in acid and E-zero(Fe3+/Fe2+) = +0.77 V, what is the E-zero cell for O2 oxidising Fe2+?

    • +0.46 V
    • -0.46 V
    • +2.00 V
    • +0.20 V

  19. What is E cell for metal X (-0.20 V) displacing Y from Y2+ (-0.40 V)?

    • +0.20 V
    • -0.20 V
    • -0.60 V
    • +0.60 V

  20. What process occurs when a single species acts as both oxidising and reducing agent?

    • Neutralisation
    • Disproportionation
    • Precipitation
    • Thermal decomposition

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