First we explain the physical transformation of a pure substance and equilibrium relations by introducing chemical potential, and then, the derivation of the phase boundary line of gas-liquid, liquid-solid, and gas-solid systems. Moreover, we give a description of the thermodynamic properties of simple mixtures in gas or liquid systems using chemical potential. We finally explain the phase rule of Gibbs which is the most important law of phase equilibrium in chemistry, and the interpretation of the phase diagram for the steam-liquid, liquid-liquid or liquid-liquid-solid coexisting systems using the phase rule.
Understanding of thermodynamic equilibrium and phase diagrams
By the end of this course, students will be able to understand:
1) Physical transformations and phase diagrams of pure substances
2) Thermodynamic description of mixtures
3) Thermodynamics of mixing
4) Chemical potential and activities
5) Colligative properties
6) The phase rule and phase diagrams of simple mixtures
Phase stability, Phase boundary, Partial molar quantities, Thermodynamics of mixing, Chemical potential, Colligative properties, Activity, Phase rule, Phase diagram
|✔ Specialist skills||Intercultural skills||Communication skills||✔ Critical thinking skills||✔ Practical and/or problem-solving skills|
At the beginning or the end of each class, solutions to exercise problems that were assigned during the previous or present class are reviewed. To prepare for class, students should read the course schedule section and check what topics will be covered. Required learning should be completed outside of the classroom for preparation and review purposes.
|Course schedule||Required learning|
|Class 1||Physical transformations of pure substances and equilibrium in chemistry||Understanding of the phase diagram indicating the physical transformation of a pure substance|
|Class 2||Physical transformations of pure substances and thermodynamic criterion of equilibrium||Understanding of the thermodynamic meaning of the phase stability and phase transitions, and derivation of the phase boundary equations|
|Class 3||Thermodynamic description of simple mixtures||Understanding of partial molar quantity and the thermodynamic function in the mixture of the perfect gas|
|Class 4||Chemical potential of liquids and thermodynamics of mixing||Understanding of the chemical potential of liquid and thermodynamic function in the liquid mixtures.Understanding of colligative properties.|
|Class 5||Phase diagram of binary system||Understanding of the phase rule, vapour pressure and temperature–composition diagrams|
|Class 6||Phase diagram of ternary system and activity||Understanding of phase diagram, solvent, solute and ion activities|
|Class 7||Final examination|
To enhance effective learning, students are encouraged to spend approximately 100 minutes preparing for class and another 100 minutes reviewing class content afterwards (including assignments) for each class.
They should do so by referring to textbooks and other course material.
Peter Atkins & Julio de Paula, Physical Chemistry, Tenth edition, Oxford, ISBN: 978-0199697403
We distribute a document at the start of lecture as needed and give a commentary using PowerPoint. The PowerPoint file to be used for lecture is made available beforehand through OCW
We evaluate students' comprehension by the results of practice exercises in classes and the final exam.
Students must have successfully completed both Basic Chemical Thermodynamics I (LAS.C107) and Physical chemistry I (CAB.B216) or have equivalent knowledge.
Classes A and B are for the students with an odd and even student ID numbers, respectively.