PHASE EQUILIBRIA

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Phase Equilibria
1. Introduction
2. Components, Phases, Degrees of Freedom and the Phase Rule
3. One Component Systems
3.1. Variation of chemical potential with temperature
3.2. Effect of pressure on chemical potential vs. temperature curves
3.3. Clausius-Clapeyron Thermodynamic Equation
3.4. Application of Clausius-Clapeyron equation
3.5. Phase diagrams of one-component systems
3.6. Le Chatelier principle and physical equilibria
3.7. Allotropy
3.8. Metastable equilibria
3.9. Liquid Crystals and Anisotropic Liquids
4. Two Component Systems
4.1. Liquid-Liquid Equilibria
4.1.1. Ideal and real liquids
4.1.2. Partially miscible liquids
4.1.3. Completely miscible liquids
4.1.4. Immiscible liquids
4.2. Liquid-Vapor Equilibria
4.2.1. Vapor pressure properties liquids
4.2.2. Raoult’s law
4.2.3. Positive and negative deviations from the Raoult’s law
4.2.4. Zeotropic and Azeotropic liquid mixtures
4.2.5. Distillation of completely miscible liquids
4.2.6. Distillation of partially miscible liquids
4.3. Solid-Liquid Equilibria
4.3.1. Simple eutectic solid-liquid systems
4.3.2. Congruent solid-liquid systems
4.3.3. Incongruent solid-liquid systems
4.4. Miscibility in the solid solutions
4.4.1. Complete miscible solid solutions
4.1.2. Partially miscible solid solutions
5. Three Component Systems
6. Systems with more than three components
7. Practical application of phase equilibria

Index
Selected Bibliography