Chemical Thermodynamics

Autor Leo Lue
ISBN 978-87-7681-497-7
1. Edition
90 Seiten

Beschreibung

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1. Introduction
1.1 Basic concepts
1.1.1 State function versus path function
1.1.2 Intensive property versus extensive property
1.2 Brief review of thermodynamics
1.2.1 The first law of thermodynamics
1.2.2 The second law of thermodynamics
1.3 The fundamental equation of thermodynamics
1.4 The calculus of thermodynamics
1.5 Open systems
1.6 Legendre transforms and free energies

2. Single component systems
2.1 General phase behavior
2.2 Conditions for phase equilibrium
2.3 The Clapeyron equation

3. Multicomponent systems
3.1 Thermodynamics of multicomponent systems
3.1.1 The fundamental equation of thermodynamics
3.1.2 Phase equilibria
3.1.3 Gibbs phase rule
3.2 Binary mixtures
3.2.1 Vapor-liquid equilibrium
3.2.2 Liquid-liquid equilibria
3.2.3 Vapor-liquid-liquid equilibria
3.3 Ternary mixtures

4. The ideal solution model
4.1 Definition of the ideal solution model
4.2 Derivation of Raoult’s law

5. Partial molar properties
5.1 Definition
5.2 Relationship between total properties and partial molar properties
5.3 Properties changes on mixing
5.4 Graphical representation for binary systems

6. Nonideal solutions
6.1 Deviations from Raoult’s law and the activity coefficient
6.2 Modified Raoult’s law
6.3 Empirical activity coefficient models
6.4 The Gibbs-Duhem equation
6.5 Azeotropic systems

7. Stability
7.1 Introduction
7.2 Liquid-liquid equilibrium

8. Solid-liquid equilibrium
8.1 Introduction
8.2 Phase behavior
8.3 Conditions for equilibrium

9. Gas solubility and Henry’s law
9.1 Henry’s law
9.2 Activity coefficients

10. Equations of state
10.1 The principle of corresponding states
10.2 The van der Waals equation and cubic equations of state
10.3 Equations of state for mixtures

11. Thermodynamics from equations of state
11.1 The residual Helmholtz free energy
11.2 Fugacity
11.3 Vapor-liquid equilibrium with a non-ideal vapor phase

12. Chemical reaction equilibria
12.1 Conditions for equilibrium
12.2 The phase rule for chemically reacting systems
12.3 Gas phase reactions
12.4 The standard Gibbs free energy of formation
12.5 The influence of temperature
12.6 Liquid phase reactions