Electrochemistry

The standard cell potential of the following cell \(\mathrm{Zn}\left|\mathrm{Zn}^{2+}(\mathrm{aq})\right| \mathrm{Fe}^{2+}(\mathrm{aq}) \mid \mathrm{Fe}\) is \(0.32 \mathrm{~V}\). Calculate the standard Gibbs energy change for the reaction:

\(\mathrm{Zn}(\mathrm{s})+\mathrm{Fe}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Fe}(\mathrm{s})\)

(Given : \(1 \mathrm{~F}=96487 \mathrm{C}\))