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If the $E_{cell} °$ for a given reaction has a negative value, which of the following gives the correct relationships for the values of $ΔG ° and K_{eq}$ ?

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$ΔG ° > 0; K_{eq} > 1$

$ΔG ° < 0; K_{eq} < 1$

$ΔG ° > 0; K_{eq} < 1$

$ΔG ° < 0; K_{eq} > 1$

answer is A.

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Detailed Solution

$ΔG ° = - {nFE}_{cell} °$

$\begin{array}{l} If E_{eell} ° = - ve then ΔG ° = + ve i.e.; ΔG ° > 0 . \\ ΔG ° = - {nRTlogK}_{eq} \end{array}$

$For Δ G ° = + ve, K_{eq} = - ve i.e., K_{eq} < 1 .$

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