Question

For a spontaneous reaction ΔG° and \[\ce{E{^{\circ}_{cell}}}\] will be respectively:

Options

• −ve and +ve

• +ve and −ve

• +ve and +ve

• −ve and −ve

Answer 1

−ve and +ve

Explanation:

For spontaneous reactions, ΔG° should be negative.

The equilibrium constant should be more than one.

ΔG° = −2.303 RT log K_c, If K_c = 1

ΔG° = 0; If K_c > 1 then ΔG° = −ve

Again, \[\ce{\Delta G^\circ = -nFE{^{\circ}_{cell}}}\]

\[\ce{E{^{\circ}_{cell}}}\] must be positive to have ΔG° negative.