Question

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 $K_{eq}$ ?

• A. $\Delta G^{\circ} > 0 ; K_{eq} < 1$
• B. $\Delta G^{\circ} > 0 ; K_{eq} > 1$
• C. $\Delta G^{\circ} < 0 ; K_{eq} > 1$
• D. $\Delta G^{\circ} < 0 ; K_{eq} < 1$

Answer 1

Answer: (A)

$\Delta G ^{\circ}=- nFE ^{\circ}$
$E ^{o}$ is negative
So $\Delta G^{\circ}=+v e$
$\Delta G ^{\circ}=-2.303 RT \log K$
$\therefore K _{ eq } < 1$