The relation between Delta G and E for a cell | vedclass

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Question

(D) For a spontaneous reaction,the Gibbs free energy change $\Delta G$ must be negative. Given the relation $\Delta G = -nFE$,where $n$ is the number

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$E$ is positive

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(D) For a spontaneous reaction,the Gibbs free energy change $\Delta G$ must be negative. Given the relation $\Delta G = -nFE$,where $n$ is the number of moles of electrons transferred,$F$ is the Faraday constant,and $E$ is the cell potential. For $\Delta G$ to be negative,the value of $E$ must be positive,because $-nFE$ will result in a negative value when $E > 0$. Therefore,the cell reaction is spontaneous if $E$ is positive.

The relation between $\Delta G$ and $E$ for a cell is $\Delta G = -nFE$. The cell reaction will be spontaneous if:

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