I got some confusion going on with this explanation of Raoult's Law.
This is what my book say:
Because the ideal solution has a higher entropy than the pure solvent, the energy of a vapor increases as its molecules expand into a larger volume, that is, if they are at a lower pressure. Thus, solutes in a solution reduce the vapor pressure of the solvent.
Also, I should mention both solutions have the same $\Delta S$ based on the same $\frac{\Delta H}{T}$.
The point is I am confused about the last part of this explanation about how molecules expand. First off, this is all in a closed container, otherwise there's no vapor pressure. If so, the volume should be the same there is no larger or smaller volume.
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