Question

The cell in which the following reaction occurs:

$2\text{F}{\text{e}}^{\text{3 +}}\left(\text{aq}\right)+2{\text{I}}^{\text{-}}\left(\text{aq}\right)\to 2\text{F}{\text{e}}^{\text{2 +}}\left(\text{aq}\right)+{\text{I}}_{\text{2}}\left(\text{s}\right)\text{has}{\text{E}}_{\left(\text{cell}\right)}^{\odot }=0.236\text{V}$ at 298 K.

Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Answer 1

$\Delta G=nF{E}^{\circ }$

$=-2\times 96500\times 0.236=-45.548kJ$

$logK=\frac{nF{E}^{\circ }}{2.303RT}=\frac{2\times 0.236}{0.0591}=7.986$

$K={\left(10\right)}^{7.986}=96827785.6$

$=9.68\times {10}^7$