Q. Which of the following expression is correct?
A) $\Delta G{^\circ}\ = \ - \ nFE_{cell}^{{^\circ}}$
B) $\Delta G{^\circ}\ = \ + \ nFE_{cell}^{{^\circ}}$
C) $\Delta G{^\circ}\ = \ - 2.303\ RT\ \ nFE_{cell}^{{^\circ}}$
D) $\Delta G{^\circ}\ = \ - nF\ \log\ K_{c}\$
Explanation
(a)
The correct relation of $E_{cell}^{{^\circ}}$ with free energy of cell reaction and equilibrium constant are as follows
$\ \ \ \ \ \ \ \Delta G{^\circ}\ = \ \ nFE_{cell}^{{^\circ}}$
and $\Delta G{^\circ}\ = \ - 2.303\ RT\ \log\ K_{eq}$
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.