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Thermodynamics and Chemistry, 2nd Edition, Howard DeVoe
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An accessible, straightforward presentation of classical thermodynamics, focusing on derivations of basic relations, starting with thermodynamic laws and various applications of interest to chemical engineers. Written in a clear, rigorous, and understandable manner, the book extends applications of fundamental concepts by presenting topics relevant to chemistry, but which are often omitted from thermodynamics books. It indicates the conditions under which a particular equation is valid. And, it incorporates modern symbols and nomenclature, such as the notation recommended by the International Union of Pure and Applied Chemistry. A valuable reference on thermodynamics for chemical engineers. 目录： Chapter 1. Introduction Units; 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; Derivation of the Mathematical Statement of the Second Law; 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; Activities; 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 Theory; 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; Effect 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 Bibliography Index |
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