Thermodynamics and Chemistry

by Howard DeVoe

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Thermodynamics and Chemistry is designed primarily as a textbook for a one-semester course in classical chemical thermodynamics at the graduate or undergraduate level.

Description from LibreTexts.

Publisher
University of Maryland
Subjects
Chemistry, Physical and Theoretical Chemistry Textbook Maps
Licence
CC BY 4.0, as LibreTexts states it
Who can read
Tweens profiles and older, judged from its title and subjects

Contents

LibreTexts writes equations in TeX, and here they show as TeX; the PDF has them typeset.

  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: Introduction
  7. 1.1: Units
  8. 1.2: Quantity Calculus
  9. 1.3: Dimensional Analysis
  10. 1.4: Chapter 1 Problem
  11. 2: Systems and Their Properties
  12. 2.1: The System, Surroundings, and Boundary
  13. 2.2: Phases and Physical States of Matter
  14. 2.3: Some Basic Properties and Their Measurement
  15. 2.4: The State of the System
  16. 2.5: Processes and Paths
  17. 2.6: The Energy of the System
  18. 2.7: Chapter 2 Problems
  19. 3: The First Law
  20. 3.1: Heat, Work, and the First Law
  21. 3.2: Spontaneous, Reversible, and Irreversible Processes
  22. 3.3: Heat Transfer
  23. 3.4: Deformation Work
  24. 3.5: Applications of Expansion Work
  25. 3.6: Work in a Gravitational Field
  26. 3.7: Shaft Work
  27. 3.8: Electrical Work
  28. 3.9: Irreversible Work and Internal Friction
  29. 3.10: Reversible and Irreversible Processes- Generalities
  30. 3.11: Chapter 3 Problems
  31. 4: The Second Law
  32. 4.1: Types of Processes
  33. 4.2: Statements of the Second Law
  34. 4.3: Concepts Developed with Carnot Engines
  35. 4.4: Derivation of the Mathematical Statement of the Second Law
  36. 4.5: Irreversible Processes
  37. 4.6: Applications
  38. 4.7: Summary
  39. 4.8: The Statistical Interpretation of Entropy
  40. 4.9: Chapter 4 Problems
  41. 5: Thermodynamic Potentials
  42. 5.1: Total Differential of a Dependent Variable
  43. 5.2: Total Differential of the Internal Energy
  44. 5.3: Enthalpy, Helmholtz Energy, and Gibbs Energy
  45. 5.4: Closed Systems
  46. 5.5: Open Systems
  47. 5.6: Expressions for Heat Capacity
  48. 5.7: Surface Work
  49. 5.8: Criteria for Spontaneity
  50. 5.9: Chapter 5 Problems
  51. 6: The Third Law and Cryogenics
  52. 6.1: The Zero of Entropy
  53. 6.2: Molar Entropies
  54. 6.3: Cryogenics
  55. 6.4: Chapter 6 Problem
  56. 7: Pure Substances in Single Phases
  57. 7.1: Volume Properties
  58. 7.2: Internal Pressure
  59. 7.3: Thermal Properties
  60. 7.4: Heating at Constant Volume or Pressure
  61. 7.5: Partial Derivatives with Respect to \(T\), \(p\), and \(V\)
  62. 7.6: Isothermal Pressure Changes
  63. 7.7: Standard States of Pure Substances
  64. 7.8: Chemical Potential and Fugacity
  65. 7.9: Standard Molar Quantities of a Gas
  66. 7.10: Chapter 7 Problems
  67. 8: Phase Transitions and Equilibria of Pure Substances
  68. 8.1: Phase Equilibria
  69. 8.2: Phase Diagrams of Pure Substances
  70. 8.3: Phase Transitions
  71. 8.4: Coexistence Curves
  72. 8.5: Chapter 8 Problems
  73. 9: Mixtures
  74. 9.1: Composition Variables
  75. 9.2: Partial Molar Quantities
  76. 9.3: Gas Mixtures
  77. 9.4: Liquid and Solid Mixtures of Nonelectrolytes
  78. 9.5: Activity Coefficients in Mixtures of Nonelectrolytes
  79. 9.6: Evaluation of Activity Coefficients
  80. 9.7: Activity of an Uncharged Species
  81. 9.8: Mixtures in Gravitational and Centrifugal Fields
  82. 9.9: Chapter 9 Problems
  83. 10: Electrolyte Solutions
  84. 10.1: Single-ion Quantities
  85. 10.2: Solution of a Symmetrical Electrolyte
  86. 10.3: Electrolytes in General
  87. 10.4: The Debye-Hückel Theory
  88. 10.5: Derivation of the Debye-Hückel Theory
  89. 10.6: Mean Ionic Activity Coefficients from Osmotic Coefficients
  90. 10.7: Chapter 10 Problems
  91. 11: Reactions and Other Chemical Processes
  92. 11.1: Mixing Processes
  93. 11.2: The Advancement and Molar Reaction Quantities
  94. 11.3: Molar Reaction Enthalpy
  95. 11.4: Enthalpies of Solution and Dilution
  96. 11.5: Reaction Calorimetry
  97. 11.6: Adiabatic Flame Temperature
  98. 11.7: Gibbs Energy and Reaction Equilibrium
  99. 11.8: The Thermodynamic Equilibrium Constant
  100. 11.9: Effects of Temperature and Pressure on Equilibrium Position
  101. 11.10: Chapter 11 Problems
  102. 12: Equilibrium Conditions in Multicomponent Systems
  103. 12.1: Effects of Temperature
  104. 12.2: Solvent Chemical Potentials from Phase Equilibria
  105. 12.3: Binary Mixture in Equilibrium with a Pure Phase
  106. 12.4: Colligative Properties of a Dilute Solution
  107. 12.5: Solid-Liquid Equilibria
  108. 12.6: Liquid-Liquid Equilibria
  109. 12.7: Membrane Equilibria
  110. 12.8: Liquid-Gas Equilibria
  111. 12.9: Reaction Equilibria
  112. 12.10: Evaluation of Standard Molar Quantities
  113. 12.11: Chapter 12 Problems
  114. 13: The Phase Rule and Phase Diagrams
  115. 13.1: The Gibbs Phase Rule for Multicomponent Systems
  116. 13.2: Phase Diagrams- Binary Systems
  117. 13.3: Phase Diagrams- Ternary Systems
  118. 13.4: Chapter 13 Problems
  119. 14: Galvanic Cells
  120. 14.1: Cell Diagrams and Cell Reactions
  121. 14.2: Electric Potentials in the Cell
  122. 14.3: Molar Reaction Quantities of the Cell Reaction
  123. 14.4: The Nernst Equation
  124. 14.5: Evaluation of the Standard Cell Potential
  125. 14.6: Standard Electrode Potentials
  126. 14.7: Chapter 14 Problems
  127. 15: Appendices
  128. 15.1: Appendix A- Definitions of the SI Base Units
  129. 15.2: Appendix B- Physical Constants
  130. 15.3: Appendix C- Symbols for Physical Quantities
  131. 15.4: Appendix D- Miscellaneous Abbreviations and Symbols
  132. 15.5: Appendix E- Calculus Review
  133. 15.6: Appendix F- Mathematical Properties of State Functions
  134. 15.7: Appendix G- Forces, Energy, and Work
  135. 15.8: Appendix H- Standard Molar Thermodynamic Properties
  136. 15.9: Appendix I- Answers to Selected Problems
  137. Back Matter
  138. Index
  139. Glossary
  140. Detailed Licensing