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Given the half-cell reactions
(i) \( \mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e} \longrightarrow \mathrm{Fe}(\mathrm{s}) ; \quad E^{0}=-0.44 \mathrm{~V} \)
(ii) \( 2 \mathrm{H}^{+}(\mathrm{aq})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})+2 \mathrm{e} \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ; \quad E^{0}=+1.23 \mathrm{~V} \)
\( E^{0} \) for the reaction
\[
\mathrm{Fe}(\mathrm{s})+2 \mathrm{H}^{+}+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})
\]
is
(A) \( +1.67 \mathrm{~V} \)
(B) \( -1.67 \mathrm{~V} \)
(C) \( -0.77 \mathrm{~V} \)
(D) \( +0.77 \mathrm{~V} \)
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