Given: (i) \( \mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu} ; \mathrm{E}^{\circ}=0.3...
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0Given:
(i) \( \mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu} ; \mathrm{E}^{\circ}=0.337 \mathrm{~V} \)
(ii) \( \mathrm{Cu}^{2+}+\mathrm{e}^{-} \rightarrow \mathrm{Cu}^{+} ; \mathrm{E}^{\circ}=0.153 \mathrm{~V} \)
Standard electrode potential \( \left(\mathrm{E}^{\circ}\right) \) for the reaction, \( \mathrm{Cu}^{+}+\mathrm{e}^{-} \rightarrow \mathrm{Cu} \), will be:
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