Question

If the $E_{cell}^{\circ }$ 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

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

$\because E_{cell}^0=-ve\therefore \Delta G^0=-nF{E}_{cell}^0\Delta G^0=+ve\Rightarrow \Delta G>0\because \Delta G^0=-2.303RTlog{K}_{eq}\therefore K_{eq}<1$