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CHM 312: Physical Chemistry II

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CHM 312: Physical Chemistry II

Chemistry
Author
Anderson Marsh
Publisher
Lebanon Valley College
Source
LibreTexts
License
CC BY
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 138 sections
  1. 01: Gases and Equations of State
  2. 1.01: The Average Translational Kinetic Energy of a Gas
  3. 1.02: The Gaussian Distribution of One Component of the Molecular Velocity
  4. 1.03: The Distribution of Molecular Speeds is Given by the Maxwell-Boltzmann Distribution
  5. 1.04: The Maxwell-Boltzmann Distribution Has Been Verified Experimentally
  6. 1.05: The Frequency of Collisions with a Wall
  7. 1.06: Collisions with Other Molecules
  8. 1.07: Mean Free Path
  9. 1.08: The meaning and measurement of temperature
  10. 1.09: The variables of state pressure units and the ideal gas law
  11. 1.10: Ideal vs. real gases and the van der Waals equation
  12. 1.11: Another way of dealing with real gases- the virial equation
  13. 1.12: Connecting the van der Waals and the viral equations- the Boyle temperature
  14. 1.13: The ideal gas law functions and derivatives
  15. 1.14: Functions of Two Independent Variables
  16. 1.15: The Equation of State
  17. 1.16: Compressibility and Expansivity
  18. 1.17: The Total Differential
  19. 1.18: Exact and Inexact Differentials
  20. 02: Work Heat and the First Law
  21. 2.01: Overview of Classical Thermodynamics
  22. 2.02: Pressure-Volume Work
  23. 2.03: Work and Heat are not State Functions
  24. 2.04: Thermodynamic Systems
  25. 2.05: Internal Energy
  26. 2.06: The Joule Experiment
  27. 2.07: Enthalpy
  28. 2.08: Thermochemistry
  29. 2.09: Reaction Enthalpies
  30. 2.10: Lattice Energy and the Born-Haber Cycle
  31. 2.11: Energy Basics
  32. 2.12: Measuring Heat
  33. 2.13: Temperature Dependence of Enthalpy
  34. 2.14: The Joule-Thomson Effect
  35. 2.15: Adiabatic Changes
  36. 03: Entropy and the Second and Third Laws
  37. 3.01: Energy Does not Determine Spontaneity
  38. 3.02: Introduction to the Second Law
  39. 3.03: Heat Engines and the Carnot Cycle
  40. 3.04: Entropy
  41. 3.05: Nonequilibrium Isolated Systems Evolve in a Direction That Increases Their Energy Dispersal
  42. 3.06: Calculating Entropy Changes
  43. 3.07: We Must Always Devise a Reversible Process to Calculate Entropy Changes
  44. 3.08: Comparing the System and the Surroundings
  45. 3.09: Heat Capacity as a Function of Temperature
  46. 3.10: The Third Law
  47. 3.11: Absolute Entropy
  48. 3.12: Evaluating Entropy Changes Using Thermochemical Cycles
  49. 04: State Functions in Thermodynamics
  50. 4.01: Free Energy Functions
  51. 4.02: A G and Maximum Work
  52. 4.03: Gibbs Energy Determines the Direction of Spontaneity at Constant Pressure and Temperature
  53. 4.04: The Maxwell Relations
  54. 4.05: Volume Dependence of Helmholtz Energy
  55. 4.06: Pressure Dependence of Gibbs Energy
  56. 4.07: Temperature Dependence of A and G
  57. 4.08: The Enthalpy of an Ideal Gas is Independent of Pressure
  58. 4.09: When Two Variables Change at Once
  59. 05: Single Component Phase Equilibrium
  60. 5.01: Gibbs Energies and Phase Diagrams
  61. 5.02: Chemical Potential and Fugacity
  62. 5.03: The Gibbs-Duhem Equation
  63. 5.04: Criterion for Phase Equilibrium
  64. 5.05: Phase Diagrams for Pure Substances
  65. 5.06: Gibbs Phase Rule
  66. 5.07: The Clapeyron Equation
  67. 5.08: The Clausius-Clapeyron Equation
  68. 06: Multiple Component Phase Equilibrium
  69. 6.01: Thermodynamics of Mixing
  70. 6.02: Partial Molar Volume
  71. 6.03: Chemical Potential
  72. 6.04: Non-ideality in Gases - Fugacity
  73. 6.05: A Mixture is a Combination of Two or More Substances
  74. 6.06: The Gibbs-Duhem Equation Relates Chemical Potential and Composition at Equilibrium
  75. 6.07: Chemical Potential of Each Component Has the Same Value in Each Phase in Which the Component Appears
  76. 6.08: Raoults Law and Phase Diagrams of Ideal Solutions
  77. 6.09: Fractional Distillation of Ideal Mixtures
  78. 6.10: Most Solutions are Not Ideal
  79. 6.11: Phase Diagrams of Non-Ideal Solutions
  80. 6.12: Fractional Distillation of Non-ideal Mixtures (Azeotropes)
  81. 6.13: Activity
  82. 6.14: Colligative Properties
  83. 6.15: Osmotic Pressure can Determine Molecular Masses
  84. 07: Chemical Equilibrium
  85. 7.01: Equilibrium Results when Gibbs Energy is Minimized
  86. 7.02: Reaction Quotient and Equilibrium Constant
  87. 7.03: An Equilibrium Constant is a Function of Temperature Only
  88. 7.04: Pressure Dependence of Kp - Le Chatelier's Principle
  89. 7.05: Degree of Dissociation
  90. 7.06: The Dumas Bulb Method for Measuring Decomposition Equilibrium
  91. 7.07: Gibbs Energy of a Reaction vs. Extent of Reaction is a Minimum at Equilibrium
  92. 7.08: The Sign of G and not G Determines the Direction of Reaction Spontaneity
  93. 7.09: Reaction Quotient and Equilibrium Constant Ratio Determines Reaction Direction
  94. 7.10: The van 't Hoff Equation
  95. 08: Electrochemistry
  96. 8.01: Electrolytes Solutions are Nonideal at Low Concentrations
  97. 8.02: The Debye-Huckel Theory
  98. 8.03: Extending Debye-Huckel Theory to Higher Concentrations
  99. 8.04: Electricity
  100. 8.05: The connection to G
  101. 8.06: Half Cells and Standard Reduction Potentials
  102. 8.07: Entropy of Electrochemical Cells
  103. 8.08: The Nernst Equation
  104. 8.09: Evaluation of the Standard Cell Potential
  105. 09: Chemical Kinetics
  106. 9.01: The Time Dependence of a Chemical Reaction is Described by a Rate Law
  107. 9.02: The Method of Initial Rates
  108. 9.03: Rate Laws Must Be Determined Experimentally
  109. 9.04: First-Order Reactions Show an Exponential Decay of Reactant Concentration with Time
  110. 9.05: Different Rate Laws Predict Different Kinetics
  111. 9.06: The Method of Half-Lives
  112. 9.07: Complex Rate Laws
  113. 9.08: Reaction Mechanisms
  114. 9.09: The Connection between Reaction Mechanisms and Reaction Rate Laws
  115. 9.10: The Rate Determining Step Approximation
  116. 9.11: The Steady-State Approximation
  117. 9.12: The Equilibrium Approximation
  118. 9.13: Arrhenius Equation
  119. 9.14: The Rate of Bimolecular Gas-Phase Reaction Can Be Estimated Using Hard-Sphere Collision Theory and an Energy-Dependent Reaction Cross Section
  120. 9.15: A Reaction Cross Section Depends Upon the Impact Parameter
  121. 9.16: The Rate Constant for a Gas-Phase Chemical Reaction May Depend on the Orientations of the Colliding Molecules
  122. 9.17: Kinetics of Reactions in Solution
  123. 9.18: Diffusion-controlled Reactions
  124. 9.19: Diffusion-Limited Reactions
  125. 9.20: Basics of Reaction Profiles
  126. 9.21: RK3. Activation Barriers
  127. 9.22: Eyring equation
  128. 10: Complex Reaction Mechanisms
  129. 10.01: The Lindemann Mechanism
  130. 10.02: Some Reaction Mechanisms Involve Chain Reactions
  131. 10.03: Catalysis
  132. 10.04: The Michaelis-Menten Mechanism
  133. 10.05: Isotherms are Plots of Surface Coverage as a Function of Gas Pressure at Constant Temperature
  134. 10.06: Atoms and Molecules can Physisorb or Chemisorb to a Surface
  135. 10.07: Using Langmuir Isotherms to Derive Rate Laws for Surface-Catalyzed Gas-Phase Reactions
  136. 10.08: The Structure of a Surface is Different from that of a Bulk Solid
  137. 10.09: The Haber-Bosch Reaction Can Be Surface Catalyzed
  138. 10.10: Fluorescence