If the enthalpy change for the transition of liquid water to steam is 30 kJ mol^$$-$$1 at 27^oC, the entropy change for the process would be

Match List I (Equations) with List II (Type of processes) and select the correct option.

List I		List II
Equations		Type of processes
A.	Kp > Q	(i)	Non- spontaneous
B.	$$\Delta $$Go < RT ln Q	(ii)	Equilibrium
C.	Kp = Q	(iii)	Spontaneous and endothermic
D.	T > $${{\Delta H} \over {\Delta S}}$$	(iv)	Spontaneous

Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be

For vaporization of water at 1 atmospheric pressure, the values of $$\Delta $$H and $$\Delta $$S are 40.63 kJ mol^$$-$$1 and 108.8 J K^$$-$$1 mol^$$-$$1, respectively. The temperature when Gibb's energy change ($$\Delta $$G) for this transformation will be zero, is