CHEM 342: Physical Chemistry II

by Kathryn Davis

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Principles of chemical thermodynamics and statistical thermodynamics, with application to pure substances and mixtures. It also applies the principles of chemical kinetics and dynamic equilibrium theory to a variety of chemical applications, including electrochemistry and spectroscopy.

Description from LibreTexts.

Publisher
Manchester University
Subjects
Chemistry
Licence
CC BY-NC-SA 4.0, as LibreTexts states it. Non-commercial use only.
Who can read
Tweens profiles and older, judged from its title and subjects

Contents

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  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: The First Law of Thermodynamics
  7. 1.1: Overview of Classical Thermodynamics
  8. 1.2: Pressure-Volume Work
  9. 1.3: Work and Heat are not State Functions
  10. 1.4: Energy is a State Function
  11. 1.5: An Adiabatic Process is a Process in which No Energy as Heat is Transferred
  12. 1.6: The Temperature of a Gas Decreases in a Reversible Adiabatic Expansion
  13. 1.7: Enthalpy and Pressure-Volume Work
  14. 1.8: Heat Capacity is a Path Function
  15. 1.9: Relative Enthalpies Can Be Determined from Heat Capacity Data and Heats of Transition
  16. 1.10: Enthalpy Changes for Chemical Equations are Additive
  17. 1.11: Heats of Reactions Can Be Calculated from Tabulated Heats of Formation
  18. 1.12: The Temperature Dependence of ΔH
  19. 1.13: Enthalpy is a State Function
  20. 2: Entropy, Second and Third Laws
  21. 2.1: Energy Does not Determine Spontaneity
  22. 2.2: Nonequilibrium Isolated Systems Evolve in a Direction That Increases Their Energy Dispersal
  23. 2.3: Unlike heat, Entropy is a State Function
  24. 2.4: The Second Law of Thermodynamics
  25. 2.5: The Famous Equation of Statistical Thermodynamics is S=k ln W
  26. 2.6: We Must Always Devise a Reversible Process to Calculate Entropy Changes
  27. 2.7: Thermodynamics Provides Insight into the Conversion of Heat into Work
  28. 2.8: The 3rd Law of Thermodynamics Puts Entropy on an Absolute Scale
  29. 2.9: Entropy Increases with Increasing Temperature
  30. 3: Free Energy and Thermodynamic Potentials
  31. 3.1: Total Differential of a Dependent Variable
  32. 3.2: Total Differential of the Internal Energy
  33. 3.3: Enthalpy, Helmholtz Energy, and Gibbs Energy
  34. 3.4: Closed Systems
  35. 3.5: Surface Work
  36. 3.6: Criteria for Spontaneity
  37. 4: Pure Substances
  38. 4.1: Volume Properties of Pure Substances
  39. 4.2: Internal Pressure
  40. 4.3: U, H, and Cp in Closed Systems
  41. 4.4: Heating at Constant Volume or Pressure
  42. 4.5: Partial Derivatives with Respect to \(T\), \(p\), and \(V\)
  43. 4.6: Standard States of Pure Substances
  44. 4.7: Standard Molar Quantities of a Gas
  45. 4.8: Phase Equilibria
  46. 4.9: Phase Diagrams of Pure Substances
  47. 5: Mixtures
  48. 5.1: Composition Variables
  49. 5.2: Partial Molar Quantities
  50. 5.3: Ideal Solutions obey Raoult's Law
  51. 5.4: Most Solutions are Not Ideal
  52. 5.5: The Activities of Nonvolatile Solutes
  53. 5.6: Colligative Properties Depend only on Number Density
  54. 5.7: Single-ion Quantities
  55. 5.8: Solution of a Symmetrical Electrolyte
  56. 5.9: Electrolytes in General
  57. 5.10: The Debye-Hückel Theory
  58. 5.11: The Gibbs Phase Rule for Multicomponent Systems
  59. 5.12: Phase Diagrams- Binary Systems
  60. 6: Chemical Equilibrium
  61. 6.1: Equilibrium Results when Gibbs Energy is Minimized
  62. 6.2: An Equilibrium Constant is a Function of Temperature Only
  63. 6.3: Gibbs Energy of a Reaction vs. Extent of Reaction is a Minimum at Equilibrium
  64. 6.4: The Sign of ΔG and not ΔG° Determines the Direction of Reaction Spontaneity
  65. 6.5: The van 't Hoff Equation
  66. 7: Kinetics
  67. 7.1: Reaction Rate
  68. 7.2: Rate Laws
  69. 7.3: 0th order Rate Law
  70. 7.4: 1st order rate law
  71. 7.5: 2nd order Rate Laws
  72. 7.6: The Method of Initial Rates
  73. 7.7: Temperature Dependence
  74. 7.8: Collision Theory
  75. 7.9: Transition State Theory
  76. 7.10: Reaction Mechanisms
  77. 7.11: The Connection between Reaction Mechanisms and Reaction Rate Laws
  78. 7.12: The Rate Determining Step Approximation
  79. 7.13: The Steady-State Approximation
  80. 7.14: The Equilibrium Approximation
  81. Back Matter
  82. Index
  83. Glossary
  84. Detailed Licensing
  85. Detailed Licensing