For the cell reaction 2Fe3+(aq) + 2I– (aq) $ \to $ 2Fe2+(aq) + I2(aq) ${E_{cell}^\Theta }$ = 0.24 V at 298 K. The standard Gibbs energy ($\Delta $rGo) of the cell reaction is : [Given that Faraday constant F = 96500 C mol–1]

Question

For the cell reaction
2Fe³⁺(aq) + 2I^– (aq) $ \to $ 2Fe²⁺(aq) + I₂(aq)
${E_{cell}^\Theta }$ = 0.24 V at 298 K. The standard Gibbs energy ($\Delta $_rG^o) of the cell reaction is :
[Given that Faraday constant F = 96500 C mol^–1]

46.32 kJ mol^–1

23.16 kJ mol^–1

–46.32 kJ mol^–1

–23.16 kJ mol^–1

Solution

Please login to view the detailed solution steps...

Go to DASH