If the E^{circ}_{cell} for a given reaction h | vedclass

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(A) The relationship between standard Gibbs free energy change $(\Delta G^{\circ})$ and standard cell potential $(E^{\circ}_{cell})$ is given by $\Del

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$\Delta G^{\circ} > 0; K_{eq} < 1$

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(A) The relationship between standard Gibbs free energy change $(\Delta G^{\circ})$ and standard cell potential $(E^{\circ}_{cell})$ is given by $\Delta G^{\circ} = -nFE^{\circ}_{cell}$.If $E^{\circ}_{cell}  0$,which indicates that the reaction is non-spontaneous.Furthermore,the relationship between $E^{\circ}_{cell}$ and the equilibrium constant $(K_{eq})$ is given by $E^{\circ}_{cell} = \frac{RT}{nF} \ln K_{eq}$.If $E^{\circ}_{cell} < 0$,then $\ln K_{eq} < 0$,which implies $K_{eq} < 1$.

If the $E^{\circ}_{cell}$ for a given reaction has a negative value,which of the following gives the correct relationships for the values of $\Delta G^{\circ}$ and $K_{eq}$ ?

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