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If the $E_{\text {cell }}^{\circ}$ for a given reaction has a negative value then which of the following gives the correct relationships for the values of $\Delta G^{\circ}$ and $K_{\text {eq }}$ ?
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The correct answer is:
$\Delta G^{\circ}\gt0 ; K_{\text {eq }} \lt 1$
$\Delta G^{\circ}=-n F E^{\circ}$
When $E^{\circ}$ is negative, then $\Delta G^{\circ}\gt0$
$\Delta G^{\circ}=-R T$ in $K_{\mathrm{eq}}$
When, $\Delta G^{\circ}\gt0, K_{\text {eq }}=10^{-x}$ which is less than one, i.e., $K_{\text {eq }} \lt 1$.
When $E^{\circ}$ is negative, then $\Delta G^{\circ}\gt0$
$\Delta G^{\circ}=-R T$ in $K_{\mathrm{eq}}$
When, $\Delta G^{\circ}\gt0, K_{\text {eq }}=10^{-x}$ which is less than one, i.e., $K_{\text {eq }} \lt 1$.
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