Thermodynamics - Gibbs Free Energy Question

[action259]

Homework Statement

I'm having some difficulty with this question, not exactly sure how to start it. Any suggestion would help. Thanks

At 2.02 atm water boils at 121 °C. Calculate the change in the Gibbs free energy
when one mole of steam at 121 °C and one atm condenses to liquid water at the
same temperature and pressure. Is this process possible? Assume that steam
behaves as an ideal gas and that the density of liquid water at 121 °C is constant
at 942 kg m-3.

Homework Equations

I think these equations are useful

dGT=VdP [1]
dΔGT = ΔVdP [2]
ΔGp2 = ΔGp1 + int(ΔVdP) [3]

and since it is an ideal gas

PV=nRT -> V=nRT/P [4]

Now I think subbing [4] into [2] or [3] would help but not sure how to get ΔGp1?

 

[NateD]

The Attempt at a SolutionI think this is what should be done:Substituting [4] into [2]ΔGT = nRT/PdPSubstituting [4] into [3]ΔGp2 = ΔGp1 + nRT/PdPHere I am stuck, not sure how to find out ΔGp1