For the cell reaction
$$2Fe^{3+} (aq) + 2I^-(aq) \rightarrow 2Fe^+ (aq) + I_2(aq)$$
$$E_{cell}^\ominus = 0.24 V$$ at 298 K. The standard Gibbs energy $$(\triangle_rG^\ominus)$$ of the cell reaction is:
[Given that Faraday constant $$F = 96500 C mol^{-1}]$$

A

$$-23.16 kJ mol^{-1}$$

B

$$46.32 kJ mol^{-1}$$

C

$$23.16 kJ mol^{-1}$$

D

$$-46.32 kJ mol^{-1}$$