Kelvi

For the cell reaction $\\ {2Fe}^{3+} (aq) + 2I^{-} (aq) \rightarrow 2Fe^{2+} (aq) + I_2 (s) \\$ The standard Gibbs energy $(\Delta G^\circ)$ of the cell reaction is: $\\$ (Given: $E^\circ_{cell} = 0.24$ V at $298$ K)

medium

Electrochemistry

2019

chemistry

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

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

Explanation

To solve this problem, we will use the relationship between the standard Gibbs energy change and the standard cell potential. $\\$ The formula to calculate the standard Gibbs energy change $(\Delta G^\circ)$ is: $\\ \Delta G^\circ = -nFE^\circ_{cell} \\$

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