Assumed a cell with the following reaction: \( \mathrm{Cu}_{(\mathrm{s})}+2 \mathrm{Ag}^{+} \) \...

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Assumed a cell with the following reaction: \( \mathrm{Cu}_{(\mathrm{s})}+2 \mathrm{Ag}^{+} \) \( \left(1 \times 10^{-3} \mathrm{M}\right) \rightarrow \mathrm{Cu}^{2+}(0.250 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s}) ; \mathrm{E}_{\text {cell }}^{\mathrm{o}}=2.97 \mathrm{~V} \).
\( \mathrm{E}_{\text {cell }} \) for the above reaction is \( \mathrm{V} \). (nearest integer) [Given: \( \log 2.5=0.3979, \mathrm{~T}=298 \mathrm{~K} \) ]
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