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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?