Question

For a spontaneous reaction the $\Delta$G, equilibrium constant (K) and $E^{\circ}_{cell}$ will be respectively :

• A. $-ve, > 1, -ve$
• B. $-ve, < 1, -ve$
• C. $+ve, > 1, -ve$
• D. $-ve, > 1, +ve$

Answer 1

Answer: (D)

$-ve, > 1, +ve$

Answer 2

$\Delta G^{\circ} = -2.303RT\,log\,K_{eq}$ $\Delta G^{\circ } = -nFE^{\circ}_{cell}$ If a cell reaction is spontaneous (proceeding in forward side), it means $K_{eq} > 1$ and $E^{\circ }_{cell} = +ve$ Thus$\quad\quad\Delta G^{\circ } = - ve$