External

CHM 363: Physical Chemistry 1

This text is an introduction to physical chemistry that emphasizes experimental and theoretical aspects of chemical thermodynamics, chemical and physical equilibrium, and kinetics.

Chemistry

Author: Elaine Marzluff
Publisher: Grinnell College
Source: LibreTexts
Language: EN
Category: Basic Sciences

Read online Download PDF (open licence)

Contents· 112 sections

01: Energy Levels and Spectroscopy
1.01: Electromagnetic Radiation
1.02: The Wave Theory of Light
1.03: Bohr's Theory of the Hydrogen Emission Spectrum
1.04: Hydrogen's Atomic Emission Spectrum
1.05: The Schrodinger Wave Equation
1.06: Particle in a One-Dimensional Box
1.07: Electronic Spectroscopy
1.08: The Harmonic Oscillator Approximates Molecular Vibrations
1.09: The Harmonic Oscillator and Infrared Spectra
1.10: Microwave Spectroscopy
02: Atomic Structure
2.01: The Schrodinger Wave Equation for the Hydrogen Atom
2.02: Many-Electron Atoms and the Periodic Table
2.03: Quantum-Mechanical Tunneling
03: Chemical Bond
3.01: Lewis Structures
3.02: Valence Bond Theory
3.03: Hybridization of Atomic Orbitals
3.04: Molecular Orbital Theory
3.05: Diatomic Molecules
3.06: Electronegativity and Dipole Moment
3.07: Photoelectron Spectroscopy
04: Gases
4.01: The Perfect Gas
4.02: Real Gases (Deviations From Ideal Behavior)
4.03: van der Waals and Redlich-Kwong Equations of State
4.04: The Law of Corresponding States
4.05: The Repulsive Term in the Lennard-Jones Potential
05: Boltzmann
5.01: The Boltzmann Factor is used to Approximate the Fraction of Particles in a Large System
5.02: The Boltzmann Distribution represents a Thermally Equilibrated Distribution
5.03: The Average Ensemble Energy is Equal to the Observed Energy of a System
5.04: Heat Capacity at Constant Volume is the Change in Internal Energy with Temperature
5.05: Partition Functions can be Decomposed into Partition Functions of Each Degree of Freedom
5.06: Translational Partition Functions of Monotonic Gases
5.07: Most Atoms are in the Ground Electronic State
5.08: The Energy of a Diatomic Polyatomic Molecule Can Be Approximated as a Sum of Separate Terms
5.09: Most Molecules are in the Ground Vibrational State
5.10: Most Molecules are Rotationally Excited at Ordinary Temperatures
5.11: Rotational Partition Functions of Diatomic Gases Contain a Symmetry Number
06: The First Law
6.01: Internal Energy
6.02: Enthalpy
6.03: Thermochemistry
6.04: State Functions and Exact Differentials
6.05: Adiabatic Changes
07: Entropy and The Second Law of Thermodynamics
7.01: Energy Does not Determine Spontaneity
7.02: The Second Law of Thermodynamics
7.03: We Must Always Devise a Reversible Process to Calculate Entropy Changes
7.04: The Famous Equation of Statistical Thermodynamics is Sk ln W
7.05: Entropy Can Be Expressed in Terms of a Partition Function
7.06: The Statistical Definition of Entropy is Analogous to the Thermodynamic Definition
7.07: Thermodynamics Provides Insight into the Conversion of Heat into Work
08: The Third Law Absolute Entropy and the Gibbs Free Energy of Formation
8.01: Heat Capacity as a Function of Temperature
8.02: The Third Law
8.03: Absolute Entropy
8.04: Evaluating Entropy Changes Using Thermochemical Cycles
09: Helmholtz and Gibbs Energies
9.01: Helmholtz Energy
9.02: Gibbs Energy Determines the Direction of Spontaneity at Constant Pressure and Temperature
9.03: The Maxwell Relations
9.04: Thermodynamic Functions have Natural Variables
9.05: The Enthalpy of an Ideal Gas is Independent of Pressure
9.06: The Gibbs-Helmholtz Equation
10: Phase Equilibria
10.01: A Phase Diagram Summarizes the Solid-Liquid-Gas Behavior of a Substance
10.02: Gibbs Energies and Phase Diagrams
10.03: The Chemical Potentials of a Pure Substance in Two Phases in Equilibrium
10.04: The Clausius-Clapeyron Equation
11: Solutions Liquid Liquid
11.01: A Mixture is a Combination of Two or More Substances
11.02: The Gibbs-Duhem Equation Relates Chemical Potential and Composition at Equilibrium
11.03: Chemical Potential of Each Component Has the Same Value in Each Phase in Which the Component Appears
11.04: Ideal Solutions obey Raoult's Law
11.05: Most Solutions are Not Ideal
11.06: Vapor Pressures of Volatile Binary Solutions
11.07: Activities of Nonideal Solutions
12: Chemical Equilibrium
12.01: Reaction Quotient and Equilibrium Constant
12.02: Equilibrium Results when Gibbs Energy is Minimized
12.03: The Equilibrium Constant
12.04: An Equilibrium Constant is a Function of Temperature Only
12.05: Reaction Quotient and Equilibrium Constant Ratio Determines Reaction Direction
12.06: The Sign of G and not G Determines the Direction of Reaction Spontaneity
12.07: The van 't Hoff Equation
12.08: Equilibrium Constants in Terms of Partition Functions
13: The Kinetic Theory of Gases
13.01: The Average Translational Kinetic Energy of a Gas
13.02: The Distribution of Molecular Speeds is Given by the Maxwell-Boltzmann Distribution
13.03: Mean Free Path
13.04: Rates of Gas-Phase Chemical Reactions
14: Chemical Kinetics I - Rate Laws
14.01: The Time Dependence of a Chemical Reaction is Described by a Rate Law
14.02: First-Order Reactions Show an Exponential Decay of Reactant Concentration with Time
14.03: Different Rate Laws Predict Different Kinetics
14.04: Arrhenius Equation
14.05: Eyring equation
15: Chemical Kinetics II- Reaction Mechanisms
15.01: A Mechanism is a Sequence of Elementary Reactions
15.02: The Steady-State Approximation
15.03: Rate Laws Do Not Imply Unique Mechanism
15.04: The Lindemann Mechanism
15.05: Some Reaction Mechanisms Involve Chain Reactions
15.06: A Catalyst Affects the Mechanism and Activation Energy
15.07: The Michaelis-Menten Mechanism for Enzyme Catalysis
16: Math Chapters
16.01: Probability and Statistics
16.02: Spherical Coordinates
16.03: Partial Differentiation