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

Question

Dr. Abubacker · Accepted Answer

[Solution] $\Delta G^\circ = -nFE^\circ = -2 	imes 96500 	imes 0.24 = -46.32$ kJ $mol^{-1}$. Answer (1).

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

Explanation

Reviewed by Dr. Abubacker

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