Question

Given the standard half-cell potentials \(\left(\mathrm{E}^{\circ}\right)\) of the following as
$$
\begin{array}{ll}
\mathrm{Zn}=\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} & \mathrm{E}^{0}=+0.76 \mathrm{~V} \\
\mathrm{Fe}=\mathrm{Fe}^{2+}+2 \mathrm{e}^{-} & \mathrm{E}^{0}=0.41 \mathrm{~V}
\end{array}
$$
Then the standard e.m.f. of the cell with the reaction \(\mathrm{Fe}^{2+}+\mathrm{Zn} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Fe}\) is
(A) \(-0.35 \mathrm{~V}\)
(B) \(+0.35 \mathrm{~V}\)
(C) \(+1.17 \mathrm{~V}\)
(D) \(-1.17 \mathrm{~V}\)

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