A galvanic cell is constructed as follows: Zn(s) | Zn^{2+}(0.010\,M) || Cu^{2+}(0.10\,M) | Cu(s). Standard reduction potentials at 298\,K are:
$$
\text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \quad E^\circ = -0.76\ \text{V}
$$
$$
\text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \quad E^\circ = +0.34\ \text{V}
$$
Calculate:
(i) the standard cell potential $E^\circ_{\text{cell}}$,
(ii) the cell potential $E_{\text{cell}}$ under the given concentrations using the Nernst equation,
(iii) state whether the cell will operate spontaneously in the direction written, and
(iv) the equilibrium constant $K$ for the overall cell reaction.

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(i) $E^\circ_{\text{cell}} = 1.10\ \text{V}$\n(ii) $E_{\text{cell}} \approx 1.13\ \text{V}$\n(iii) Yes, the cell is spontaneous in the written direction.\n(iv) $K \approx 1.5\times10^{37}$.

Gce Model Questions Vol1 2021 Chemistry Question 32

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