The standard reduction potential of the electrode is . Calculate the reduction electrode potential ( — Electrochemistry Chemistry Question
Question
The standard reduction potential of the $Cu^{2+}/Cu$ electrode is $+0.34\text{ V}$. Calculate the reduction electrode potential (in Volts) of a half-cell containing a $0.01\text{ M}$ aqueous solution of $Cu^{2+}$ ions at $298\text{ K}$. (Take $\frac{2.303RT}{F} = 0.0591\text{ V}$)
Answer: 0.2809
💡 Solution & Explanation
According to the Nernst equation for the half-reaction $Cu^{2+} + 2e^- \rightarrow Cu$, $E = E^\circ - \frac{0.0591}{n} \log \frac{1}{[Cu^{2+}]}$. Plugging in the values: $E = 0.34 - \frac{0.0591}{2} \log \frac{1}{0.01} = 0.34 - \frac{0.0591}{2} \log(100) = 0.34 - 0.0591 = 0.2809\text{ V}$.
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