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CHE 371 |
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I: MATHEMATICS REVIEW |
| Functions and Operators |
| Partial Derivatives |
| Multiple Integrals |
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II: GASES |
| The Definition of Pressure |
| Liquid Pressure |
| The Barometer |
| The Manometer |
| Boyle's Law |
| The Two-State Boyle's Law |
| Charles's or Gay-Lussac's Law |
| The Two-State Charles's Law |
| Avogadro's Law |
| The Ideal Gas Law |
| The Two-State Ideal Gas Law |
| Standard Temperature and Pressure (STP) |
| Molar Mass-Ideal Gas Relationship |
| Law of Combining Volumes |
| Dalton's Law of Partial Pressures |
| Mole Fraction |
| Model for the Kinetic Molecular Theory of Gases |
| Molecular Basis of PV=nRT |
| The Speed of Gas Molecules |
| Distribution of Molecular Speeds |
| Translational Kinetic Energy of Gases |
| Effusion of Gases |
| Real Gases |
| The van der Waals Model of Real Gases |
| van der Waals Excluded Volume and Molecular Diameters |
| Boyle Temperature |
| Other Two-Parameter Equations of State |
| Critical Phenomena |
| The Virial Equation of State |
| The van der Waals Constants Can be Related to the Critical Constants |
| Law of Corresponding States |
| van der Waals Equation and the Virial Equation |
| Cubic Expansion Coefficient |
| Isothermal Compressibility |
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III: THE FIRST LAW OF THERMODYNAMICS |
| Definitions |
| Types of Systems |
| Zeroth Law of Thermodynamics |
| Two Different Forms of Energy |
| Joule's Mechanical Equivalent of Heat Experiment |
| Units of Energy |
| State Properties |
| The Total Differential |
| Exact/Inexact Differentials |
| Sign Conventions |
| Endothermic/Exothermic Reactions |
| Thermal/Mechanical Surroundings |
| Heat Capacity |
| Specific Heat |
| Experimental Determination of Specific Heat |
| The Fundamental Equation of Calorimetry |
| The "Coffee Cup'' Calorimeter |
| The Bomb Calorimeter |
| The First Law of Thermodynamics |
An Equation for the Change in Enthalpy ( ) |
vs. |
| Heat Capacities |
| The Interal Energy of an Ideal Gas Does Not Depend on its Volume |
| Joule-Thompson Expansion |
| The Joule-Thompson Expansion is a Constant Enthalpy Process |
| The Joule-Thompson Coefficient |
| Two Conditions for Expansions/Compressions |
| Reversible/Irreversible Processes |
| An Equation for Expansion Work |
| Free Isothermal Expansion of a Gas |
| Free Isothermal (Irreversible) Expansion of a Gas |
| Obtaining Maximum Work by Expansion |
| A Formula for Controlled (Reversible) Isothermal Expansion |
| Adiabatic Expansion of a Gas |
| Reversible Adiabatic Expansion of a Gas |
| Irreversible Adiabatic Expansion of a Gas |
| What is Enthalpy? |
| Values of with Special Names |
| Rules of Thermochemistry |
| Standard Conditions |
| Standard Molar Enthalpies of Formation |
| Standard Molar Enthalpies of Formation for Ions in Aqueous Solutions |
| Bond Energies |
| Using Bond Energies to Estimate
for a Reaction |
| Temperature Dependence of |
| Temperature Dependence of the Heat Capacity |
Using  Tables to Calculate  |
The Connection Between 
and  |
| Other useful relations |
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IV: THE SECOND AND THIRD LAWS OF THERMODYNAMICS |
| The Second Law of Thermodynamics |
| Spontaneous/Non-spontaneous Processes |
| Heat Engines |
| Efficiency of a Heat Engine |
| The Carnot Cycle |
| The Efficiency of the Carnot Cycle and the Thermodynamic Temperature Scale |
| Calculations for the Ideal Gas Carnot Cycle |
| Entropy |
| The Clausius Inequality |
| Mathematical Demonstration that Entropy is a State Function |
| Irreversible Processes are Accompanied by an Increase in Entropy |
| Criteria for Spontaneity |
| The Fundamental Equation for a Closed System |
| Heat Transfer |
 for
Typical Processes |
| Molar Entropy of an Ideal Gas as a Function of Temperature and Pressure |
| Entropy of Mixing |
| Molecular Interpretation of Entropy |
| Aside on Statitical Thermodynamics |
| The Third Law of Thermodynamics |
The Standard Reaction Entropy,
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How Do We Calculate 
for a Chemical Reaction? |
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V: GIBBS ENERGY |
| Proof that Rev. Work is Maximum Work |
| Gibbs Free Energy |
| Maximum Useful Work |
 gives the Maximum Non-Expansion Work |
| Equilibrium Criteria Under Various Conditions |
| When is < 0 and a Reaction is Spontaneous? |
| Fundamental Relationships for Closed Systems |
| Determining from the Defining
Equation |
| Determining
from the Standard Gibbs Free Energy of Formation |
| for an Isothermal Expansion of an Ideal Gas |
| for Normal Boiling |
| Pressure Dependence of |
| Temperature Dependence of |
| Thermodynamic Definition of an Ideal Gas |
| Thermodynamic Equations of State |
What is  for a Real Gas? |
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| Fugacity |
| The Standard State of Fugacity |
| Calculating the Fugacity of Real Gases |
| Calculating the Fugacity of a van der Waals Gas |
| The Fugacity Coefficient |
| The Chemical Potential |
| Partial Molar Quantities |
| The Gibbs-Duhem Equation |
| Determining the Partial Molar Volume of a Solute |
| Mixing of Two Ideal Gases |
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VI. CHEMICAL EQUILIBRIUM |
| The Gibbs Energy Minimum and Equilibrium |
| Reaction Gibbs Energy at Arbitrary Concentrations |
| Standard Free Energies for Ideal Gases |
| Standard Free Energies for Ideal Gases: Mixtures |
| The Reaction Quotient, Q |
| The Equilibrium Constant: Ideal Gas Reactions |
| On Equilibrium Constants |
| Activity |
| Reactions at Equilibrium |
| Examples |
| LeChatelier's Principle |
| The Effect of Temperature on the Equilibrium Constant |
| The Effect of Pressure on the Equilibrium Constant |
| The Equilibrium Constant Expressed in Concentrations |
| The Equilibrium Constant: Real Gas Reactions |
The Connection Between  and
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VII: PHASE DIAGRAMS AND EQUILIBRIUM |
| Vapor Pressure |
| Phase Equilibria: Definitions |
| Phase Transitions and Phase Diagrams |
| Criteria of Equilibrium between Phases: The Chemical Potential |
| Gibbs Phase Rule |
| One-Component Phase Diagrams |
| The Clapeyron Equation |
| The Clausius-Clapeyron Equation |
| Measures of Concentration |
| Raoult's Law |
| Raoult's Law Written in Terms of Fugacities |
| Ideal Solutions and Vapor Pressure Curves |
| Henry's Law |
| If Henry's Law is Obeyed, Then Raoult's Law is Obeyed |
| Ideal-Dilute Solutions and Vapor Pressure Curves |
| Vapor Pressure Lowering |
| Freezing Point Depression |
| Boiling Point Elevation |
| Osmotic Pressure |
| Phase Diagrams for Binary Mixtures |
| Mixtures of Volatile Liquids |
| Fractional Distillation |
| Tie Lines |
| The Lever Rule |
| Highly Non-Ideal Mixtures |
| Liquid-Liquid Phase Diagrams |
| Liquid-Solid Phase Diagrams |
| Cooling Curves |
| Congruently Melting Compounds |
| Enthalpy of Solution |
Mixing of Ideal Solutions:
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Mixing of Ideal Solutions:
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Mixing of Ideal Solutions:
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Mixing of Ideal Solutions:
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| Activity, Again |
| Standard Reference States: Gases, Solids, and Liquids |
| Activity for the Solvent |
Activity of Solutes:  -Scale |
Activity of Solutes:  -Scale |
| The Equilibrium constant Written in Terms of Activities |
| Vapor Pressure can be an Equilibrium Constant |
| Activities and Activity Coefficients of the Solvent are Experimentally Determined |
| Activities and Activity Coefficients of the Solute are Experimentally Determined |
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VIII: ELECTROCHEMISTRY |
| A Review of Oxidation-Reduction Reactions |
| Rules for Assigning Oxidation Numbers |
| Rules for Balancing Oxidation-Reduction Reactions |
| Oxidation Numbers Revisited |
| Formal Charges |
| Electrical Units and Constants |
| Types of Electrochemical Cells |
| Examples of Electrochemical Cells |
| Cell Reaction and Half-Reactions |
| Cell Notation |
| ReDox Couples |
| Varieties of Electrochemical Cells |
| Half-Cells |
| Concentration Cells |
| Liquid-Junction Potentials |
| Cell Potential |
| Standard Voltage |
| Nernst Equation |
| The Standard Hydrogen Electrode (SHE) |
| Standard Reduction Potentials |
| Defining a Standard State for a Strong Electrolyte |
| Activity of a Uni-Univalent (1:1) Electrolyte Solution |
| Multi-valent Electrolyte |
| Ionic Strength |
| Debye-Huckel Theory |
| Determination of the Activity Coefficient of HCl |
| Ksp from Standard Reduction Potentials |
| The Electrochemical Series |
| Variation of E with pH |
| Relationship to Other Thermodynamic Functions |
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IX: OTHER STUFF |
| Conductivities of Electrolytic Solutions |
| Kohlrausch's Law |
| Nernst Distribution Law |