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Chemistry Question on types of cells

For the cell reaction
2Fe3++2I(aq)−→2Fe2++I2(aq)2Fe^{3+}+2I^{-}_{(aq)}\rightarrow2Fe^{2+}+I_2{(aq)}
Ecell⊖=0.24 V at 298k.E^{\ominus}_{cell}=0.24\ V \ at \ 298 k.The standard Gibbs energy (ΔrG⊖)(\Delta_rG^{\ominus}) of the cell reaction is:
[Given that Faraday constant F=96500 C mol−1] F=96500 \ C\ mol^{-1}]

A

−46.32 kjmol−1-46.32 \ kjmol{-1}

B

−23.16 kjmol−1-23.16 \ kjmol{-1}

C

46.32 kjmol−146.32 \ kjmol{-1}

D

23.16 kjmol−123.16\ kjmol{-1}

Answer

−46.32 kjmol−1-46.32 \ kjmol{-1}

Explanation

Solution

The correct option is (A) :−46.32 kjmol−1-46.32 \ kjmol{-1}