Given the electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.771 \ V$
$I_2 + 2e^- \to 2I^{-}; E^o = 0.536 \ V$
The $E^o_{\text{cell}}$ for the cell reaction $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$ is:
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.771 \ V$
$I_2 + 2e^- \to 2I^{-}; E^o = 0.536 \ V$
The $E^o_{\text{cell}}$ for the cell reaction $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$ is:
- A$(2 \times 0.771 - 0.536) = 1.006 \ V$
- B$(0.771 - 0.5 \times 0.536) = 0.503 \ V$
- C$(0.771 - 0.536) = 0.235 \ V$
- D$(0.536 - 0.771) = -0.235 \ V$
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