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Physical Chemistry |
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Table of Contents
Thermodynamics |
Statistical Mechanics |
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1. Temperature, Pressure, Molar volume, and Equilibrium |
1. The Fundamental Equations of Statistical Mechanics
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2. The Equation of State |
2. The Physical Interpretation of the Fundamental Equations of Statistical Mechanics
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3. How to Use the Equation of State |
3. Interpretation of the Thermodynamic Quantities
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4. Thermodynamic Transformations |
4. The Partition Function of a System of Independent Particles
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5. Work |
5. The Partition Function of an Ideal Gas of Atoms
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6. Heat |
6. The Thermodynamic Functions of an Ideal Gas of Atoms
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7. Reversible and Irreversible Transformations |
7. The Thermodynamic Properties of an Ideal Gas for which Electronic and Nuclear Contributions are Negligible
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8. Path-Dependent and Path-independent Quantities |
8. A Test of the Theory for a Gas for which Electronic and Nuclear Degrees of Freedom Matter
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9. First and Second Laws |
9. The Statistical Mechanics of a Gas of Diatomic Molecules
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10. Helmholtz and Gibbs Free Energies |
10. A Gas of Diatomic Molecules: Comparison with Experiment
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11. How to Calculate the Change of Entropy in an Equilibrium Transformation |
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12. Enthalpy and Energy Change During a Thermodynamic Transformation |
12. Transition State Theory: The Physical Content
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13. Thermochemistry |
13. Transition State Theory: The Motion of an Adsorbed Atom
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14. The Change of Chemical Potential During an Equilibrium Transformation |
14. Transition State Theory: The Rate Constant
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15. The Chemical Potential of a Compound in a Mixture |
15. Transition State Theory: Calculating the Rate Constant
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16. Mixtures: Partial Molar Quantities and Activities |
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17. Chemical Equilibrium |
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18. Chemical Equilibrium: The Connection between the Equilibrium Constant and Composition |
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19. Chemical Equilibrium: How to Calculate the Equilibrium Constant from Delta G |
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20. Chemical Equilibrium: The Dependence of the Equilibrium Constant on Temperature and Pressure |
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21. Chemical Equilibrium of Coupled Reactions |
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22 Phase Transitions in One-Component Systems: The Phenomena |
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23. Phase Transitions in One-Component Systems: The Equilibrium Conditions |
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24. Phase Transitions in One-Component Systems: How to Use the Equilibrium Conditions |
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25. Phase Equilibria in Binary Systems: The Phenomena |
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26. Equilibrium Conditions for Binary Systems with Two Phases: Application to Vapor-Liquid Equilibrium |
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27. Electrolyte Solutions |
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28. Electrochemistry: Phenomena |
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29. Electrochemistry: Equilibria |
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Appendices 1-9 |
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Kinetics |
Quantum Mechanics |
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1. Generalities about the Rates of Chemical Reactions |
1. Why Quantum Mechanics? |
2. Irreversible First-Order Reactions |
2. Dynamical Variables and Operators |
3. The Temperature Dependence of the Rate Constant: the Arrhenius Formula |
3. The Eigenvalue Problem |
4. Irreversible Second-Order Reactions |
4. What Do We Measure When We Study Quantum Systems? |
5. Reversible First-Order Reactions |
5. Some Results are Certain, Most are Just Probable
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6. Reversible Second-order Reactions |
6. The Physical Interpretation of the Wave Function |
7. Coupled Reactions |
7. Tunneling |
8. An Example of a Complex Reaction: Chain Reactions |
8. Particle in a Box |
9. Enzyme Kinetics |
9. Light Emission and Absorption: the Phenomena |
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10. Light Emission and Absorption: Einstein's Phenomenological Theory |
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11. Light Absorption: A Result of Quantum Theory |
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12. Light Emission and Absorption by a Particle in a Box and a Harmonic Oscillator |
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13. Two-Particle Systems |
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14. Angular Momentum |
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15. Two-Particle Systems: the Radial and Angular Schrödinger Equations |
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16. The Energy Eigenstates of a Diatomic Molecule |
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17. Diatomic Molecule: Its Spectroscopy |
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18. Hydrogen Atom: the Eigenstates |
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19. The Spin of the Electron and its Role in Spectroscopy |
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20. The Hydrogen Molecule |
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21. Nuclear Magnetic Resonance and Electron Spin Resonance |
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Appendices 1-2 |
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