Question
For a spontaneous reaction the $$\Delta G,$$ equilibrium constant $$(K)$$ and $$E_{cell}^ \circ $$ will be respectively
A.
$$-ve, >1, -ve$$
B.
$$-ve, <1, -ve$$
C.
$$+ve, >1, -ve$$
D.
$$-ve, >1, +ve$$
Answer :
$$-ve, >1, +ve$$
Solution :
NOTE : For spontaneous reaction $$\Delta G$$ should be negative. Equilibrium constant should be more than one
$$\left( {\Delta G = - 2.303\,RT\log \,{K_c},\,{\text{If}}\,{K_c} = 1\,{\text{then}}\,\Delta G = 0\,;\,{\text{If}}\,{K_c} < 1\,{\text{then}}\,\Delta G = + ve} \right).$$ Again $$\Delta G = - nFE_{cell}^ \circ .$$
$$E_{cell}^ \circ $$ must be $$+ve$$ to have $$\Delta G - ve.$$