Question

The $\Delta G^{\circ}$ for the Daniell cell has been found to be $-212.3\, kJ$ at $25^{\circ} C$. Calculate the equilibrium constant for the cell reaction.

• A. $ 11.64\times {{10}^{30}} $
• B. $ 1.64\times {{10}^{37}} $
• C. $ 0.1064\times {{10}^{35}} $
• D. $ 21.64\times {{10}^{39}} $

Answer 1

Answer: (B)

$\Delta G^{\circ}=-R T \ln K_{c}$
$-212300\, J=-\left(8.314 \,J K^{-1}\, mol ^{-1}\right)(298 \,K)$
$\ln K_{c}=\frac{212300}{8.314 \times 293}=85.69$
$K_{c}=1.64 \times 10^{37}$