Chemical Thermodynamics Classical, Statistical And Irreversible

Cover
Dedication
Contents
Preface
List of Symbols
Chapter 1 : Introduction
	1.a. Scope and Limitations of Thermodynamics
	1.b. The Language and Methods of Thermodynamics
	1.c. Thermodynamic Equilibrium
	1.d. Thermodynamic Processes and Paths
	1.e. State Functions
	1.f. Thermometry
		1.g.1. Heat
		1.g.2. Work
		1.g.3. Energy
		1.h.1. Work of Expansion
		1.h.2. Reversible and Irreversible Processes—Maximum Work
		1.h.3. Maximum Work in a Reversible Isothermal Expansion of an Ideal Gas
		Questions
Chapter 2 : The First Law of Thermodynamics
	2.a. Principle of Conservation of Energy
		2.b.1. Mathematical Formulation of the First Law
		2.b.2. Heat Changes at Constant Volume and Constant Pressure
	2.c. Heat Capacity
		2.d.1. Energy Content of an Ideal Gas
		2.d.2. The Joule–Thomson Effect
	2.e. Some Relations Between Cp and Cv
	2.f. Calculation of ΔU, ΔH, q and w for Ideal Gases
		2.g.1. Temperature Changes in Reversible Adiabatic Processes
		2.g.2. Pressure–Volume Relationships in Reversible Adiabatic Changes
		2.g.3. Relationship Between Pressure and Temperature in Reversible Adiabatic Changes
	2.h. Comparison of Isothermal and Adiabatic Processes
	2.i. Adiabatic Irreversible Expansion
		2.j.1. Calculation of Thermodynamic Quantities for Real Gases
		2.j.2. Isothermal Changes of Real Gases
		2.j.3. Adiabatic Reversible Expansion of a Real Gas
		2.j.4. Irreversible Isothermal Expansion of a Real Gas
		2.j.5. Adiabatic Irreversible Expansion
		Questions
Chapter 3 : Thermochemistry
	3.a. Heat Changes in Chemical Reactions
	3.b. Standard States and Conventions
		3.c.1. Heat (Enthalpy) of Formation
		3.c.2. Heat (Enthalpy) of Combustion
		3.c.3. Thermochemical Laws
		3.c.4. Phase Changes
		3.c.5. Heat (Enthalpy) of Solution
		3.c.6. Heat (Enthalpy) of Neutralisation
		3.c.7. Heats (Enthalpies) of Formation of Atoms and Ions
		3.c.8. Born–Haber Cycle
		3.c.9. Bond Energy (Enthalpy)
	3.d. Kirchhoff’s Equation
	3.e. Explosions and Flames
		Questions
Chapter 4 : The Second Law of Thermodynamics
	4.a. The Need for a Second Law
		4.b.1. Statements
		4.b.2. The Efficiency of a Heat Engine
	4.c. Heat Pump and Refrigerator
	4.d. The Thermodynamic Scale of Temperature
		4.e.1. Entropy
		4.e.2. The Evaluation of Entropy Changes
	4.f. Dependence of Entropy on Variables of a System
	4.g. ΔS for Phase Changes
	4.h. Temperature–Entropy Diagram
	4.i. Irreversible Processes
	4.j. Entropy of Mixing
		4.k.1. The Significance of Entropy
		4.k.2. Degradation of Energy
		4.k.3. Entropy as a Measure of Disorder
		4.k.4 Entropy of the Universe
		Questions
Chapter 5 : Free Energy and Work Function
	5.a.1. Entropy as a Criterion for Spontaneity
	5.a.2. Definition of New State Functions
	5.b. Variation in A and G with Volume, Temperature and Pressure
	5.c. Conditions for Equilibrium and Spontaneity
	5.d. Thermodynamic Formulae—Maxwell Relations
	5.e. Thermodynamic Equations of State
	5.f. Standard Free Energies
	5.g. The Gibbs–Helmholtz Equation
		Questions
Chapter 6 : The Third Law of Thermodynamics
	6.a. The Nernst Heat Theorem
	6.b. Calculation of Entropy
	6.c. Entropy of Real Gases
	6.d. Applications of the Third Law
	6.e. Entropy Changes in Chemical Reactions
		Questions
Chapter 7 : Statistical Thermodynamics
	7.a. The Statistical Method
	7.b. The Language of Statistical Thermodynamics
	7.c. Statistical Thermodynamic Formulation of the Boltzmann Equation
	7.d. Negative Temperature
		7.e.1. Partition Function and Thermodynamic Functions
		7.e.2. Molar Partition Function
	7.f. Entropy and the Third Law
		7.g.1. Separation of the Partition Function According to Forms of Energy
		7.g.2. Kinetic Theory of Gases and the Translational Kinetic Energy
		7.g.3. Molar Entropy of an Ideal Monoatomic Gas (Translational Entropy)
		7.g.4. Diatomic Molecules—Rotational Partition Function
		7.g.5. Partition Function and Vibrational Energy
		7.g.6. Electronic Partition Function
		7.g.7. Total or Combined Partition Function
	7.h. Calculation of Equilibrium Constants by Using Partition Functions
		7.i.1. Heat Capacity
		7.i.2. Equipartition of Energy
		7.i.3. Heat Capacities from the Classical Theory
		7.i.4. Quantum Statistical Theory of Specific Heat
		7.i.5. Diatomic Molecules
		7.i.6. Rotational Heat Capacity for the Hydrogen Molecule
		7.i.7. Vibrational Contribution
	7.j. Heat Capacity of Solids
		7.k.1. Quantum Statistics
		7.k.2. Fermi–Dirac Statistics
		7.k.3. Bose–Einstein Statistics
		Questions
Chapter 8 : Partial Molar Properties
	8.a. Systems of Variable Composition
		8.b.1. Molarity and Mol Fraction
		8.b.2. Molality and Mol Fraction
	8.c. Partial Molar Quantities
		8.d.1. Chemical Potential (μ) and the Gibbs–Duhem Equations
		8.d.2. Mixtures of Gases
	8.e. Alternative Definitions of Chemical Potential
	8.f. Variation of Chemical Potential with T and P
	8.g. Determination of Partial Molar Properties
	8.h. Differential and Integral Heats (Enthalpies) of Solution
	8.i. Determination of Partial Molar Properties from Apparent Molar Properties
		Questions
Chapter 9 : Phase Equilibria
	9.a. Chemical Potential and Phase Equilibria
	9.b. Single Component Systems
	9.c. The Clausius–Clapeyron Equation
	9.d. Thermodynamic Derivation of the Phase Rule
	9.e. Applications of the Phase Rule to a Few Systems
		Questions
Chapter 10 : Fugacity and Activity
	10.a. Fugacity
		10.b.1. Methods of Determining the Fugacity of a Real Gas
		10.b.2. Variation of Fugacity with Pressure
		10.b.3. Variation of Fugacity with Temperature
	10.c. Ideal Solutions and Raoult’s Law
	10.d. Thermodynamics of Mixing
		10.e.1. Dilute Solutions
		10.e.2. Composition of the Vapour in Equilibrium with a Liquid
		10.e.3. Deviations from Raoult’s Law
		10.e.4. Henry’s Law and the Solubility of Gases
	10.f. Nernst Distribution Law
		10.g.1. Colligative Properties
		10.g.2. Lowering of Vapour Pressure
		10.g.3. Elevation of the Boiling Point
		10.g.4. Depression of the Freezing Point
		10.g.5. Osmosis and Osmotic Pressure
		10.g.6. Association and Dissociation in Solution
		10.h.1. Activity
		10.h.2. Choice of Standard States
		10.h.3. Dependence of Activity on Temperature and Pressure
		10.h.4. The Activity Coefficient
		10.h.5. Determination of Activity and Activity Coefficients of Non-electrolytes
		10.h.6. Determination of the Activity of One Component from That of the Other
		Questions
Chapter 11 : Chemical Equilibrium
	11.a. The Law of Mass Action
	11.b. Free Energy Criterion and Reversible Reactions
	11.c. Free Energy and the Equilibrium Constant
	11.d. Equilibrium in Ideal Gas Systems
	11.e. Significance of the Equilibrium Constant
		11.f.1. Application of the Law of Mass Action to a Few Chemical Equilibria
		11.f.2. Homogeneous Equilibria
		11.f.3. Heterogeneous Equilibria
		11.g.1. Effect of External Factors on Chemical Equilibria
		11.g.2. Effect of Pressure on Chemical Equilibria
		11.g.3. Effect of Temperature on Chemical Equilibria
	11.h. The Reaction Isotherm
		Questions
Chapter 12 : Aqueous Solutions of Electrolytes
	12.a. Fugacity and Activity of Electrolytes
		12.b.1. Mean Ionic Activity
		12.b.2. Mean Ionic Activity Coefficient
		12.b.3. Determination of the Activities and Activity Coefficients of Strong Electrolytes
	12.c. Ionic Strength
		12.d.1. Activity Coefficients from Solubility Measurements
		12.d.2. Results of Activity Coefficient Measurements
		12.d.3. Activity Coefficients from Debye–Huckel Theory
		12.e.1. Applications of the Debye–Huckel Limiting Law
		12.e.2. Verification of the Limiting Law
	12.f. Thermodynamics of Ions in Solution
		Questions
Appendix A :  Thermodynamic Properties of Systems Under the Influence of Various Fields
Appendix B : Non-equilibrium Thermodynamics or Thermodynamics of Irreversible Processes
Appendix C : A Molecular Approach to Internal Energy and Enthalpy
Appendix D : A Few Applications of Quantum Statistics
Appendix E : Tables : List of tables A to H
Bibliography
Index