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

Answer 1

Answer: (C)

$\Delta G^o>0;K_{eq}<1$

$\Delta G^0=-nF{E}_{cell}^o=-RTln{K}_{eq}$

As $E_{cell}^{o}is-ve$

$\Delta G=+ve$

Hence,

$\Delta G^o>0;K_{eq}<1$