For the cell reaction

2Fe^{3+}(aq)+ 2I^{-}(aq) \rightarrow 2Fe^{2+}(aq) + I_2(aq)

E^0_{cell} = 0.24V at 298K. The standard Gibbs energy (\Delta_r G^0) of the cell reaction is:

[Given that Faraday constant F = 96500 C mol-1]

  • Option 1)

    -46.32 kJ mol-1

  • Option 2)

    -23.16 kJ mol-1

  • Option 3)

    46.32 kJ mol-1

  • Option 4)

    23.16 kJ mol-1

Answers (1)

We know that 

    \Delta G^0 = -nFE^0_{cell}

\Rightarrow \Delta G^0 = -2\times 96500\times 0.24

\Rightarrow \Delta G^0 = -46.32 kJ mol^{-1}

Option 1 is correct


Option 1)

-46.32 kJ mol-1

Option 2)

-23.16 kJ mol-1

Option 3)

46.32 kJ mol-1

Option 4)

23.16 kJ mol-1

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