\[ \begin{array}{l} \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \operatorname{Ag}(\m...
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0\[
\begin{array}{l}
\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \operatorname{Ag}(\mathrm{s}) ; \mathrm{E}^{0}=0.80 \mathrm{~V} \\
\mathrm{Co}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Co}(\mathrm{s}) ; \mathrm{E}^{0}=-0.28 \mathrm{~V}
\end{array}
\]
Use the standard reduction potentials to determine the standard potential for the reaction:
\[
\mathrm{Co}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Co}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})
\]
(a) \( 0.52 \mathrm{~V} \)
(b) \( 0.66 \mathrm{~V} \)
(c) \( 1.08 \mathrm{~V} \)
(d) \( 1.88 \mathrm{~V} \)
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