Question

If the $E_{cell}^0$ for a given reaction has a negative value, which of the following gives the correct relationships for the values of $\Delta G^0$ 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

The correct option is A $\Delta G^{\circ }>0;K_{eq}<1$

$\Delta G^{\circ }=-nF{E}_{cell}^{\circ }$
If $E_{cell}^{\circ }=-ve$ then $\Delta G^{\circ }=+ve$ i.e.; $\Delta G^{\circ }>0$
$\Delta G^{\circ }=-nRTlog{K}_{eq}$
For $\Delta G^{\circ }=+ve,K_{eq}=-vei.e.,K_{eq}<1$