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Answer: \(E \approx 0.287\) V

Electrode reaction: Cu\(^{2+}\) + 2e\(^-\) → Cu(s), \(n = 2\). Nernst equation at 298 K:

\[E = E^\circ - \frac{0.0592}{n}\log_{10}\frac{1}{[\text{Cu}^{2+}]} = 0.337 - \frac{0.0592}{2}\log_{10}\frac{1}{0.02}\]\[E = 0.337 - 0.0296\times\log_{10}50 = 0.337 - 0.0296\times1.699 = 0.337 - 0.0503 = 0.2867\ \text{V}\]
Doubtly AI · 27 Oct 2026 AI-verified · Oct 2026 Report
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