Nguồn ngoài

General Physical Chemistry I

CHEM 351 is an-unit upper-division course titled Physical Chemistry I: Thermodynamics and Kinetics. It focuses on the quantitative interpretation of macroscopic matter, covering chemical thermodynamics, kinetics, and the laws governing energy, enthalpy, entropy, and reaction rates.

Chemistry

Tác giả: Nancy Gerber
Nhà xuất bản: San Francisco State University
Nguồn: LibreTexts
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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Mục lục· 148 mục

01: The Properties of Gases
1.01: Properties of Gas
1.02: All Dilute Gases Behave Ideally
1.03: van der Waals and Redlich-Kwong Equations of State
1.04: A Cubic Equation of State
1.05: The Law of Corresponding States
1.06: The Second Virial Coefficient
1.07: The Repulsive Term in the Lennard-Jones Potential
1.08: Van der Waals Constants in Terms of Molecular Parameters
1.E: The Properties of Gases (Exercises)
02: The Kinetic Theory of Gases
2.01: Basics of Kinetic Molecular Theory
2.02: Common Ideal Gas Difficulties
2.03: Connecting Gas Properties to Kinetic Theory of Gases
2.04: Kinetic Molecular Theory of Gases
2.05: Real Gases
2.06: The Average Translational Kinetic Energy of a Gas
2.07: The Gaussian Distribution of One Component of the Molecular Velocity
2.08: The Distribution of Molecular Speeds is Given by the Maxwell-Boltzmann Distribution
2.09: The Frequency of Collisions with a Wall
2.10: The Maxwell-Boltzmann Distribution Has Been Verified Experimentally
2.11: Mean Free Path
2.12: Rates of Gas-Phase Chemical Reactions
2.E: The Kinetic Theory of Gases (Exercises)
03: Properties of Liquids
3.01: Capillary Action
3.02: Cohesive and Adhesive Forces
3.03: Contact Angles
3.04: Surface Tension
3.05: Unusual Properties of Water
3.06: Vapor Pressure
3.07: Viscosity
3.08: Wetting Agents
04: The First Law of Thermodynamics
4.01: Overview of Classical Thermodynamics
4.02: Pressure-Volume Work
4.03: Work and Heat are not State Functions
4.04: Energy is a State Function
4.05: An Adiabatic Process is a Process in which No Energy as Heat is Transferred
4.06: The Temperature of a Gas Decreases in a Reversible Adiabatic Expansion
4.07: Work and Heat Have a Simple Molecular Interpretation
4.08: Pressure-Volume Work
4.09: Heat Capacity is a Path Function
4.10: Relative Enthalpies Can Be Determined from Heat Capacity Data and Heats of Transition
4.11: Enthalpy Changes for Chemical Equations are Additive
4.12: Heats of Reactions Can Be Calculated from Tabulated Heats of Formation
4.13: The Temperature Dependence of H
4.14: Enthalpy is a State Function
4.E: The First Law of Thermodynamics (Exercises)
05: Entropy and The Second Law of Thermodynamics
5.01: Energy Does not Determine Spontaneity
5.02: Nonequilibrium Isolated Systems Evolve in a Direction That Increases Their Energy Dispersal
5.03: Unlike heat Entropy is a State Function
5.04: The Second Law of Thermodynamics
5.05: The Famous Equation of Statistical Thermodynamics is Sk ln W
5.06: We Must Always Devise a Reversible Process to Calculate Entropy Changes
5.07: Thermodynamics Provides Insight into the Conversion of Heat into Work
5.08: Entropy Can Be Expressed in Terms of a Partition Function
5.09: The Statistical Definition of Entropy is Analogous to the Thermodynamic Definition
5.E: Entropy and The Second Law of Thermodynamics (Exercises)
06: Entropy and the Third Law of Thermodynamics
6.01: Entropy Increases With Increasing Temperature
6.02: The 3rd Law of Thermodynamics Puts Entropy on an Absolute Scale
6.03: The Entropy of a Phase Transition can be Calculated from the Enthalpy of the Phase Transition
6.04: The Debye Function is Used to Calculate the Heat Capacity at Low Temperatures
6.05: Practical Absolute Entropies Can Be Determined Calorimetrically
6.06: Practical Absolute Entropies of Gases Can Be Calculated from Partition Functions
6.07: Standard Entropies Depend Upon Molecular Mass and Structure
6.08: Spectroscopic Entropies sometimes disgree with Calorimetric Entropies
6.09: Standard Entropies Can Be Used to Calculate Entropy Changes of Chemical Reactions
6.E: Entropy and the Third Law of Thermodynamics (Exercises)
07: Helmholtz and Gibbs Energies
7.01: Helmholtz Energy
7.02: Gibbs Energy Determines the Direction of Spontaneity at Constant Pressure and Temperature
7.03: The Maxwell Relations
7.04: The Enthalpy of an Ideal Gas is Independent of Pressure
7.05: Thermodynamic Functions have Natural Variables
7.06: The Standard State for a Gas is an Ideal Gas at 1 Bar
7.07: The Gibbs-Helmholtz Equation
7.08: Fugacity Measures Nonideality of a Gas
7.E: Helmholtz and Gibbs Energies (Exercises)
08: Phase Equilibria
8.01: A Phase Diagram Summarizes the Solid-Liquid-Gas Behavior of a Substance
8.02: Gibbs Energies and Phase Diagrams
8.03: The Chemical Potentials of a Pure Substance in Two Phases in Equilibrium
8.04: The Clausius-Clapeyron Equation
8.05: Chemical Potential Can be Evaluated From a Partition Function
8.E: Phase Equilibria (Exercises)
09: Solutions
9.01: Partial Molar Quantities in Solutions
9.02: The Gibbs-Duhem Equation
9.03: Chemical Potential of Each Component Has the Same Value in Each Phase in Which the Component Appears
9.04: Ideal Solutions obey Raoult's Law
9.05: Most Solutions are Not Ideal
9.06: Vapor Pressures of Volatile Binary Solutions
9.07: Activities of Nonideal Solutions
9.08: Activities are Calculated with Respect to Standard States
9.09: Gibbs Energy of Mixing of Binary Solutions in Terms of the Activity Coefficient
9.E: Solutions I- Liquid-Liquid Solutions (Exercises)
10: Chemical Equilibrium
10.01: Equilibrium Results when Gibbs Energy is Minimized
10.02: An Equilibrium Constant is a Function of Temperature Only
10.03: Standard Gibbs Energies of Formation Can Be Used to Calculate Equilibrium Constants
10.04: Gibbs Energy of a Reaction vs. Extent of Reaction is a Minimum at Equilibrium
10.05: Reaction Quotient and Equilibrium Constant Ratio Determines Reaction Direction
10.06: The Sign of G and not G Determines the Direction of Reaction Spontaneity
10.07: The van 't Hoff Equation
10.08: Equilibrium Constants in Terms of Partition Functions
10.09: Molecular Partition Functions and Related Thermodynamic Data Are Extensively Tabulated
10.10: Real Gases Are Expressed in Terms of Partial Fugacities
10.11: Thermodynamic Equilibrium Constants Are Expressed in Terms of Activities
10.12: Activities are Important for Ionic Species
10.13: Homework Problems
11: Chemical Kinetics I - Rate Laws
11.01: The Time Dependence of a Chemical Reaction is Described by a Rate Law
11.02: Rate Laws Must Be Determined Experimentally
11.03: First-Order Reactions Show an Exponential Decay of Reactant Concentration with Time
11.04: Different Rate Laws Predict Different Kinetics
11.05: Reactions can also be Reversible
11.06: The Rate Constants of a Reversible Reaction Can Be Determined Using Relaxation Techniques
11.07: Rate Constants Are Usually Strongly Temperature Dependent
11.08: Transition-State Theory Can Be Used to Estimate Reaction Rate Constants
11.E: Chemical Kinetics I - Rate Laws (Exercises)
12: Chemical Kinetics II- Reaction Mechanisms
12.01: A Mechanism is a Sequence of Elementary Reactions
12.02: The Principle of Detailed Balance
12.03: Multiple Mechanisms are often Indistinguishable
12.04: The Steady-State Approximation
12.05: Rate Laws Do Not Imply Unique Mechanism
12.06: The Lindemann Mechanism
12.07: Some Reaction Mechanisms Involve Chain Reactions
12.08: A Catalyst Affects the Mechanism and Activation Energy
12.09: The Michaelis-Menten Mechanism for Enzyme Catalysis
12.E: Chemical Kinetics II- Reaction Mechanisms (Exercises)
13: Math Chapters
13.01: Complex Numbers
13.02: Probability and Statistics
13.03: Vectors
13.04: Spherical Coordinates
13.05: Determinants
13.06: Matrices
13.07: Numerical Methods
13.08: Partial Differentiation
13.09: Series and Limits
13.10: Fourier Analysis
13.10.01: Fourier Analysis in Matlab
13.10.02: Fourier Synthesis of Periodic Waveforms
13.11: The Binomial Distribution and Stirling's Appromixation