Introduction to the Course

1. 1887: New Discipline of Physical Chemistry is Announced
   1. van't Hoff
   2. Ostwald
   3. Arrhenius
2. Overview of the History of Physics and Physical Chemistry
   1. Newtonian Mechanics
   2. Start of Modern Chemistry
   3. Confusion about Atoms/Debates about Atomic Weights
   4. Electricity, Magnetism, and Light
   5. Thermodynamics
   6. Kinetic Theory and Statistical Thermodynamics
   7. Early 20th Century Physics

Ch 1: Fundamental Concepts of Thermodynamics

1. Underlying Philosophy
2. System vs. Surroundings
   1. Isolated Systems
   2. Closed Systems
   3. Open Systems
3. Temperature and Thermal Equilibrium
   1. Temperature vs. Heat
   2. Zeroth Law of Thermodynamics
   3. Diathermal vs. Adiabatic Walls
   4. Temperature Scales
4. Ideal Gas Law
   1. Equation of State
   2. Physical Model
   3. Pressure and Partial Pressure
5. Introduction to Real Gases
   1. Physical Expectations
   2. Van der Waals Model

Ch 2: Heat, Work, Internal Energy, Enthalpy, and the First Law of Thermodynamics

1. Statement of the First Law
   1. Conservation of Energy
   2. Formal Statement
2. Work
   1. PV Examples
   2. Other Examples
3. Heat and Heat Capacity
   1. Heat and Internal Energy
   2. Bomb Calorimeter
   3. Heat Capacity
4. Enthalpy
   1. Another State Function
   2. Heat Capacity Revisited
5. Adiabatic Changes

Ch 3: The Importance of State Functions: Internal Energy and Enthalpy

1. Exact vs. Inexact Differentials
   1. Partial Deriviatives
   2. Exact Differentials
2. Relating H and U to Experimental Measures
   1. Internal Energy (closed system, constant composition)
   2. Enthalpy (closed system, constant composition)
3. Some Experimental Measurements
   1. Joule-Thompson Coefficient
   2. Isothermal Compressibility
   3. Volumetric Thermal Expansion Coefficient
   4. More on Heat Capacities

Ch 4: Thermochemistry

1. U and H Associated with Chemical Reactions
   1. Reaction Enthalpies
   2. Using Enthalpies of Formation
2. Hess's Law
   1. Reaction Example
   2. Bond Energy Example
3. Using Calorimetry to Measure Reaction Enthalpies
   1. Bomb Calorimetry
   2. Constant-Pressure Calorimetry
   3. Differential Scanning Calorimetry

Ch 5: Engines and the Second Law of Thermodynamics

1. Energy vs. Entropy
2. Definitions of the Second Law and Entropy
   1. The Second Law of Thermodynamics
   2. A Definition of Entropy
3. The Carnot Cycle
   1. Steps in the Cycle
   2. P-V Diagram
   3. Efficiency
4. Entropy in Thermodynamic Terms
   1. Entropy as a State Function
   2. The Clausius Inequality
5. Sample Problems involving Entropy
   1. Gas Expansion/Compression
   2. Absolute Entropies and the Third Law
   3. Entropy Changes in Chemical Reactions

Ch 6: Equilibrium

1. Free Energies
   1. Helmholtz Energy
   2. Gibbs Energy
2. Useful State Function Equations
   1. Differential Forms
   2. Maxwell Relations
3. Properties of the Gibbs Energy
   1. Pressure Effect
   2. Temperature Effect
   3. Conventional Molar G for a Compound
   4. Change in Composition (Chemical Potential)
4. Ideal Gas Mixtures
   1. Chemical Potential of a Gas within a Mixture
   2. Gibbs Energy for Mixing Ideal Gases
   3. Entropy of Mixing Ideal Gases
5. Chemical Equilibrium
   1. Standard-State Reaction Gibbs Energy
   2. Equilibrium Constants

Ch 7: Fugacity (Section 7.5 only)

Ch 8: Phase Diagrams and the Relative Stability of Solids, Liquids, and Gases

1. Examples of Phases and Phase Changes
   1. Common Examples
   2. Other Examples
   3. Liquid Crystals
2. Phase Diagrams
   1. PVT (3D) Diagrams
   2. PT and PV Projections
   3. Critical Points and Supercritical Fluids
3. Phase Stability and Phase Transitions
   1. Temperature-Tependence of Phase Stability
   2. Pressure and Melting
   3. Capillary Rise
   4. Location of Phase Boundaries
      1. Solid-Liquid
      2. Liquid-Vapor
   5. Phase Interfaces
      1. Surface Tension
      2. Pressure Drop Across Curved Surfaces
      3. Capillary Rise
   Skip section 8.6

   Ch 9: Ideal and Real Solutions

   1. Ideal Solutions
      1. Raoult's Law
      2. Chemical Potential of Ideal Solution Components
      3. Gibbs Energy of Mixing for Ideal Solutions
      4. Dilute Ideal Solutions
   2. Real Solutions and Activities
      1. Solvent
      2. Solute
   3. Partial Molar Quantities
   4. Equilibrium Constants in Solution
   5. Fractional Distillation
   6. Colligative Properties
      1. Boiling Point Elevation
      2. Freezing Point Depression
      3. Osmotic Pressure

   Ch 10: Electrolyte Solutions

   1. Background
      1. Historical Considerations
      2. Physics Basics
   2. Thermodynamics of Ions in Solution
      1. Special Reference State
      2. Mean Activity Coefficients
      3. Equilibrium Constants
      4. Ionic Strength
   3. Debye-Hückel Theory

   Ch 11: Electrochemistry

   1. Electrochemical Cells
      1. Half-Reaction Concept
      2. Classification of Electrochemical Cell Types
   2. Thermodynamics of Electrochemical Cells
      1. Nernst Equation
      2. Electrochemical Potential
      3. Standard Potentials
   Sections 11.11 through 11.16 will not be covered.

   Ch 11: Elementary Chemical Kinetics

   1. Introduction: Thermodynamics vs. Kinetics
   2. Reaction Rates and Rate Constants
   3. Rate Laws and Reaction Order
      1. Definitions and Examples
      2. Integration of Rate Laws
      3. Approach to Equilibrium
   4. Reaction Mechanisms and Chemical Kinetics
   5. Arrhenius Equation
   6. Transition-State Theory
   Sections 18.6, 18.11, 18.12, and 18.13 will not be covered.