# For the cell reaction $2Fe^{3+}(aq)+2I^{-}(aq)\rightarrow2Fe^{2+}(aq)+I_2(aq)$ $E^{\ominus}_{cell}$ cell E 0.24V at 298 K. The standard Gibbs energy $(\triangle^{\circ}_{r}G^{\ominus})$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 ) $46.32 kJ\; mol^{-1}$