by Howard DeVoe, Associate Professor Emeritus, University of Maryland


Chapter 1. Introduction
Physical Quantities, Units, and Symbols; Quantity Calculus; Dimensional Analysis; Problem

Chapter 2. Systems and Their Properties
The System, Surroundings, and Boundary; Phases and Physical States of Matter; Some Basic Properties and Their Measurement; The State of the System; Processes and Paths; The Energy of the System; Problems

Chapter 3. The First Law
Heat, Work, and the First Law; Spontaneous, Reversible, and Irreversible Processes; Heat Transfer; Deformation Work; Applications of Expansion Work; Work in a Gravitational Field; Shaft Work; Electrical Work; Irreversible Work and Internal Friction; Reversible and Irreversible Processes: Generalities; Problems

Chapter 4. The Second Law
Types of Processes; Statements of the Second Law; Concepts Developed with Carnot Engines; The Second Law for Reversible Processes; The Second Law for Irreversible Processes; Applications; Summary; The Statistical Interpretation of Entropy; Problems

Chapter 5. Thermodynamic Potentials
Total Differential of a Dependent Variable; Total Differential of the Internal Energy; Enthalpy, Helmholtz Energy, and Gibbs Energy; Closed Systems; Open Systems; Expressions for Heat Capacity; Surface Work; Criteria for Spontaneity; Problems

Chapter 6. The Third Law and Cryogenics
The Zero of Entropy; Molar Entropies; Cryogenics; Problem

Chapter 7. Pure Substances in Single Phases
Volume Properties; Internal Pressure; Thermal Properties; Heating at Constant Volume or Pressure; Partial Derivatives with Respect to T, p, and V; Isothermal Pressure Changes; Standard States of Pure Substances; Chemical Potential and Fugacity; Standard Molar Quantities of a Gas; Problems

Chapter 8. Phase Transitions and Equilibria of Pure Substances
Phase Equilibria; Phase Diagrams of Pure Substances; Phase Transitions; Coexistence Curves; Problems

Chapter 9. Mixtures
Composition Variables; Partial Molar Quantities; Gas Mixtures; Liquid and Solid Mixtures of Nonelectrolytes; Activity Coefficients in Mixtures of Nonelectrolytes; Evaluation of Activity Coefficients; Activity of an Uncharged Species; Mixtures in Gravitational and Centrifugal Fields; Problems

Chapter 10. Electrolyte Solutions
Single-ion Quantities; Solution of a Symmetrical Electrolyte; Electrolytes in General; The Debye-Huckel Theory; Derivation of the Debye-Huckel Equation; Mean Ionic Activity Coefficients from Osmotic Coefficients; Problems

Chapter 11. Reactions and Other Chemical Processes
Mixing Processes; The Advancement and Molar Reaction Quantities; Molar Reaction Enthalpy; Enthalpies of Solution and Dilution; Reaction Calorimetry; Adiabatic Flame Temperature; Gibbs Energy and Reaction Equilibrium; The Thermodynamic Equilibrium Constant; Effects of Temperature and Pressure on Equilibrium Position; Problems

Chapter 12. Equilibrium Conditions in Multicomponent Systems
Effects of Temperature; Solvent Chemical Potentials from Phase Equilibria; Binary Mixture in Equilibrium with a Pure Phase; Colligative Properties of a Dilute Solution; Solid-Liquid Equilibria; Liquid-Liquid Equilibria; Membrane Equilibria; Liquid-Gas Equilibria; Reaction Equilibria; Evaluation of Standard Molar Quantities; Problems

Chapter 13. The Phase Rule and Phase Diagrams
The Gibbs Phase Rule for Multicomponent Systems; Phase Diagrams: Binary Systems; Phase Diagrams: Ternary Systems; Problems

Chapter 14. Galvanic Cells
Cell Diagrams and Cell Reactions; Electric Potentials in the Cell; Molar Reaction Quantities of the Cell Reaction; The Nernst Equation; Evaluation of the Standard Cell Potential; Standard Electrode Potentials; Problems

Appendix A. Definitions of the SI Base Units

Appendix B. Physical Constants

Appendix C. Symbols for Physical Quantities

Appendix D. Miscellaneous Abbreviations and Symbols

Appendix E. Calculus Review

Appendix F. Mathematical Properties of State Functions

Appendix G. Forces, Energy, and Work

Appendix H. Standard Molar Thermodynamic Properties

Appendix I. Answers to Selected Problems