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JOHN: This figure plots the change in Gibbs free energy versus mole fraction for a non-ideal solution. When we mix two liquids together, the Gibbs free energy decreases, and if it were an ideal solution, the kind of solution that we use in Raoults law, for an ideal solution, the change in Gibbs free energy, IS, indicate ideal solution, is the sum of mole fractions, log of mole fractions. And this, of course, comes from the entropy term for entropy of mixing. Its in the Gibbs free energy because delta H for an ideal solution is zero. So if we look at this figure, change in Gibbs free energy, we can see that the change is negative, that when we mix the different concentrations, the Gibbs free energy always decreases. Now, what were interested in is a case where we have positive deviations from Raoults law. So what this means is if xi gamma i, where gamma i is the activity coefficient, Pi sat, YiP, this is the modified Raoults Law. So when we talk about positive deviations, we mean