4. Why is the free energy of an ideal liquid mixture less than the free energy of the pure liquid? How does this lead to freezing point depression, with the assumption that the coexisting solid is pure?

4. Why is the free energy of an ideal liquid mixture less than the free energy of the pure liquid? How does this lead to freezing point depression, with the assumption that the coexisting solid is pure?

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.50E

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4. Why is the free energy of an ideal liquid mixture less than the free energy of the pure liquid?
How does this lead to freezing point depression, with the assumption that the coexisting solid is
pure?

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