JEE Main · 2005 · 08 May 2005 · Offline · Chemical Thermodynamics

Spontaneity is read off the sign of $\Delta G$, and the other two quantities follow from it. A spontaneous change needs $\Delta G<0$. Through $\Delta G=-RT\ln K$, a negative $\Delta G$ forces $\ln K>0$, so the equilibrium constant exceeds one, $K>1$. And through $\Delta G=-nF{E}_{cell}^{\circ }$, the same negative $\Delta G$ makes $E_{cell}^{\circ }$ positive. So spontaneity pairs a negative $\Delta G$ with $K>1$ and a positive cell potential.