Question

If the $E_{cell}^o$ for a given reaction has a negative value, then which of the following gives the correct relationships for the values of $\Delta G^o$ and $K_{eq}$?

• A. $△G^o<0;K_{eq}>1$
• B. $△G^o<0;K_{eq}<1$
• C. $△G^o>0;K_{eq}<1$
• D. $△G^o>0;K_{eq}>1$

Answer 1

The correct option is C $△G^o>0;K_{eq}<1$

We have $E_{cell}^o$ negative.

$\because △G^o=-nF{E}_{cell}^o$

$△G^o=+ve\Rightarrow △G>0$

Also, $△G^o=-2.303RT\times log{K}_{eq}$

$\therefore K_{eq}<1$

Hence, option C is correct.