1. The problem statement, all variables and given/known data 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. 2. Relevant equations I think these equations are useful dGT=VdP  dΔGT = ΔVdP  ΔGp2 = ΔGp1 + int(ΔVdP)  and since it is an ideal gas PV=nRT -> V=nRT/P  Now I think subbing  into  or  would help but not sure how to get ΔGp1?