Calculate the cell potential of the galvanic cell: Zn(s) | Zn²⁺ (0.01 M) || Cu²⁺ (0.1 M) | Cu(s) at 25 °C. Use the standard electrode potentials: Zn²⁺/Zn = –0.76 V and Cu²⁺/Cu = +0.34 V.

Step-by-step solution

1. Identify the half‑reactions: Zn(s) → Zn²⁺ + 2e⁻ (E° = –0.76 V) and Cu²⁺ + 2e⁻ → Cu(s) (E° = +0.34 V).
2. Write the overall cell reaction: Zn(s) + Cu²⁺ → Zn²⁺ + Cu(s).
3. Calculate the standard cell potential: E°cell = E°cathode – E°anode = +0.34 V – (–0.76 V) = +1.10 V.
4. Write the Nernst equation for the cell: E = E°cell – (0.0592/2) log(Q).
5. Determine the reaction quotient: Q = [Zn²⁺]/[Cu²⁺] = 0.01/0.1 = 0.1.
6. Substitute the values: E = 1.10 V – (0.0592/2) log(0.1) = 1.10 V – 0.0296 × (–1) = 1.10 V + 0.0296 V = 1.1296 V.
7. Round to two decimal places: E ≈ 1.13 V.

Concept tested: Cell potential calculation using Nernst equation

Published 1 September 2026 · How this solution was prepared and checked

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