Given electrode potentials: \( \begin{array}{ll}\mathrm{Fe}^{3+}+\mathrm{e} \rightarrow \mathrm{...

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Given electrode potentials:
\( \begin{array}{ll}\mathrm{Fe}^{3+}+\mathrm{e} \rightarrow \mathrm{Fe}^{2+} & \mathrm{E}^{\circ}=0.771 \text { volts } \\ \mathrm{I}_{2}+2 \mathrm{e} \rightarrow 2 \mathrm{I}^{-} & \mathrm{E}^{\circ}=0.536 \text { volts }\end{array} \)
\( \mathrm{E}^{\circ} \) cell for the cell reaction \( 2 \mathrm{Fe}^{3+}+2 \mathrm{I}^{-} \rightarrow 2 \mathrm{Fe}^{2+}+ \)\( \mathrm{I}_{2} \) is:
(A) \( (2 \times 0.771-0.836)=1.006 \) math xmlns=http://www.w3.org/1998/Math/MathML class=wrs_chemistrymivolts/mi/math
(B) \( (0.771-0.5 \times 0.536)=0.503 \) math xmlns=http://www.w3.org/1998/Math/MathML class=wrs_chemistrymivolts/mi/math
(C) \( 0.771-0.536=0.235 \) math xmlns=http://www.w3.org/1998/Math/MathML class=wrs_chemistrymivolts/mi/math
(D) \( 0.536-0.771=-0.235 \) math xmlns=http://www.w3.org/1998/Math/MathML class=wrs_chemistrymivolts/mi/math
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