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Physical chemistry / Keith J. Laidler, John H. Meiser

Main Author Laidler, Keith J. Coauthor Meiser, John H. Country Estados Unidos. Edition 2nd ed Publication Boston : Houghton Mifflin Company, cop. 1995 Description XVII, 988 p. : il. ; 24 cm ISBN 0-395-64153-5 CDU 541.1
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Item type Current location Call number Status Date due Barcode Item holds Course reserves
Monografia Biblioteca Geral da Universidade do Minho
BGUMD 110753 Available 156491

Licenciatura em Química Química Física 2º semestre

Licenciatura em Física Química Física 2º semestre

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Enhanced descriptions from Syndetics:

After explaining the experimental and theoretical reasoning behind fundamental concepts of physical chemistry, this text moves into a discussion of the concept itself. This narrative approach, which incorporates historical vignettes, aims to give a greater understanding of the material, and brief biographies of famous physical chemists are provided to help students to see how theories have developed and to add interest to the course. Problems, worked-out examples and suggested readings are included.

Table of contents provided by Syndetics

  • Note: Each chaper concludes with Key Equations, Problems, and Suggested Reading
  • 1 The Nature of Physical Chemistry and the Kinetic Theory of Gases
  • 1.1 The Nature of Physical Chemistry
  • 1.2 Some Concepts from Classical Mechanics
  • 1.3 Systems, States, and Equilibrium
  • 1.4 Thermal Equilibrium
  • 1.5 Pressure and Boyle's Law Biography: Robert Boyle
  • 1.6 Gay-Lussac's (Charles's) Law
  • 1.7 The Ideal Gas Thermometer
  • 1.8 The Equation of State for an Ideal Gas
  • 1.9 The Kinetic-Molecular Theory of Ideal Gases
  • 1.10 The Barometric Distribution Law
  • 1.11 The Maxwell Distribution of Molecular Speeds and Translational Energies
  • 1.12 Real Gases
  • 1.13 Equations of State
  • 1.14 The Virial Equation Appendix: Some Definite and Indefinite Integrals Often Used in Physical Chemistry
  • 2 The First Law of Thermodynamics
  • 2.1 Origins of the First Law
  • 2.2 States and State Functions
  • 2.3 Equilibrium States and Reversibility
  • 2.4 Energy, Heat, and Work
  • 2.5 Thermochemistry
  • 2.6 Ideal Gas Relationships
  • 2.7 Real Gases
  • 3 The Second and Third Laws of Thermodynamics Biography: Rudolph Julius Emmanuel Clausius
  • 3.1 The Carnot Cycle
  • 3.2 Irreversible Processes
  • 3.3 Molecular Interpretation of Entropy
  • 3.4 The Calculation of Entropy Changes
  • 3.5 The Third Law of Thermodynamics
  • 3.6 Conditions for Equilibrium
  • 3.7 The Gibbs Energy
  • 3.8 Some Thermodynamic Relationships
  • 3.9 The Gibbs-Helmholtz Equation
  • 3.10 Thermodynamic Limitations to Energy Conversion
  • 4 Chemical Equilibrium Biography: Jacobus Henricus van't Hoff
  • 4.1 Chemical Equilibrium Involving Ideal Gases
  • 4.2 Equilibrium in Nonideal Gaseous Systems
  • 4.3 Chemical Equilibrium in Solution
  • 4.4 Heterogeneous Equilibrium
  • 4.5 Tests for Chemical Equilibrium
  • 4.6 Shifts of Equilibrium at Constant Temperature
  • 4.7 Coupling of Reactions
  • 4.8 Temperature Dependence of Equilibrium Constants
  • 4.9 Pressure Dependence of Equilibrium Constants
  • 5 Phases and Solutions
  • 5.1 Phase Recognition
  • 5.2 Vaporization and Vapor Pressure
  • 5.3 Classification of Transitions in Single-Component Systems
  • 5.4 Ideal Solutions: Raoult's and Henry's Laws
  • 5.5 Partial Molar Quantities
  • 5.6 The Chemical Potential
  • 5.7 Thermodynamics of Solutions
  • 5.8 The Colligative Properties
  • 6 Phase Equilibria
  • 6.1 Equilibrium Between Phases
  • 6.2 One-Component Systems
  • 6.3 Binary Systems Involving Vapor
  • 6.4 Condensed Binary Systems
  • 6.5 Thermal Analysis
  • 6.6 More Complicated Binary Systems
  • 6.7 Crystal Solubility: The Krafft Boundary and Krafft Eutectic
  • 6.8 Ternary Systems
  • 7 Solutions of Electrolytes
  • 7.1 Faraday's Laws of Electrolysis Biography: Michael Faraday
  • 7.2 Molar Conductivity
  • 7.3 Weak Electrolytes: The Arrhenius Theory Biography: Svante August Arrhenius
  • 7.4 Strong Electrolytes
  • 7.5 Independent Migration of Ions
  • 7.6 Transport Numbers
  • 7.7 Ion Conductivities
  • 7.8 Thermodynamics of Ions
  • 7.9 Theories of Ions in Solution
  • 7.10 Activity Coefficients
  • 7.11 Ionic Equilibria
  • 7.12 Ionization of Water
  • 7.13 The Donnan Equilibrium
  • 8 Electrochemical Cells
  • 8.1 The Daniell Cell
  • 8.2 Standard Electrode Potentials
  • 8.3 Thermodynamics of Electrochemical Cells
  • 8.4 Types of Electrochemical Cells
  • 8.5 Applications of emf Measurements
  • 8.6 Fuel Cells
  • 8.7 Photogalvanic Cells
  • 8.8 Batteries, Old and New
  • 9 Chemical Kinetics
  • I The Basic Ideas
  • 9.1 Rates of Consumption and Formation
  • 9.2 Rate of Reaction
  • 9.3 Empirical Rate Equations
  • 9.4 Analysis of Kinetic Results
  • 9.5 Techniques for Very Fast Reactions
  • 9.6 Molecular Kinetics
  • 9.7 The Arrhenius Equation
  • 9.8 Potential-Energy Surfaces
  • 9.9 The Preexponential Factor Biography: Henry Eyring
  • 9.10 Reactions in Solution
  • 9.11 Reaction Dynamics
  • 10 Chemical Kinetics
  • II Composite Mechanisms
  • 10.1 Evidence for a Composite Mechanism
  • 10.2 Types of Composite Reactions
  • 10.3 Rate Equations for Composite Mechanisms
  • 10.4 Rate Constants, Rate Coefficients, and Equilibrium Constants
  • 10.5 Free-Radical Reactions
  • 10.6 Photochemical Reactions
  • 10.7 Radiation-Chemical Reactions
  • 10.8 Explosions
  • 10.9 Catalysis
  • 10.10 Reactions in Solution: Some Special Features
  • 10.11 Mechanisms of Polymerization in Macromolecules
  • 10.12 Kinetics of Polymerization
  • 10.13 Induction Periods, Oscillations, and Chaos
  • 10.14 Electrochemical Dynamics
  • 11 Quantum Mechanics and Atomic Structure
  • 11.1 Electromagnetic Radiation and the Old Quantum Theory
  • 11.2 Bohr's Atomic Theory
  • 11.3 The Foundations of Quantum Mechanics
  • 11.4 Schrouml;dinger's Wave Mechanics
  • 11.5 Quantum-Mechanical Postulates
  • 11.6 Quantum Mechanics of Some Simple Systems
  • 11.7 Quantum Mechanics of Hydrogenlike Atoms
  • 11.8 Physical Significance of the Orbital Quantum Numbers
  • 11.9 Angular Momentum and Magnetic Moment
  • 11.10 The Rigid Linear Rotor
  • 11.11 Spin Quantum Numbers
  • 11.12 Many-Electron Atoms
  • 11.13 Approximate Methods in Quantum Mechanics
  • 12 The Chemical Bond Biography: Gilbert Newton Lewis
  • 12.1 The Hydrogen Molecular-Ion, H2+ 12.2
  • 12.3 Huuml;ckel Theory for More Complex Molecules
  • 12.4 Valence-Bond Theory for More Complex Molecules
  • 12.5 Symmetry in Chemistry
  • 12.6 Symmetry of Molecular Orbitals Appendix: Character Tables
  • 13 Foundations of Chemical Spectroscopy
  • 13.1 Emission and Absorption Spectra
  • 13.2 Atomic Spectra Biography: Gerhard Herzberg
  • 13.3 Pure Rotational Spectra of Molecules
  • 13.4 Vibrational-Rotational Spectra of Molecules
  • 13.5 Raman Spectra
  • 13.6 Electronic Spectra of Molecules
  • Appendix: Symmetry Species Corresponding to Infrared and Raman Spectra
  • 14 Some Modern Applications of Spectroscopy
  • 14.1 Laser Spectroscopy
  • 14.2 Spectral Line Widths
  • 14.3 Types of Lasers
  • 14.4 Laser Techniques for Chemistry
  • 14.5 Magnetic Spectroscopy
  • 14.6 Nuclear Magnetic Spectroscopy
  • 14.7 Electron Magnetic Resonance (EMR)
  • 14.8 Mouml;ssbauer Spectroscopy
  • 14.9 Photoelectron Spectroscopy
  • 14.10 Photoacoustic Spectroscopy
  • 14.11 Chiroptical Methods
  • 14.12 Mass Spectrometry
  • 15 Statistical Mechanics
  • 15.1 Forms of Molecular Energy Biography: Ludwig Boltzmann
  • 15.2 Principles of Statistical Mechanics
  • 15.3 The Partition Function
  • 15.4 Thermodynamic Quantities from Partition Functions
  • 15.5 The Partition Function for Some Special Cases
  • 15.6 The Internal Energy, Enthalpy, and Gibbs Energy Functions
  • 15.7 The Calculation of Equilibrium Constants
  • 15.8 Transition-State Theory
  • 15.9 The Approach to Equilibrium
  • 15.10 The Canonical Ensemble
  • 16 The Solid State
  • 16.1 Crystal Forms and Crystal Lattices
  • 16.2 X-Ray Crystallography
  • 16.3 Experimental Methods Biography: Dorothy Crowfoot Hodgkin
  • 16.4 Theories of Solids
  • 16.5 Statistical Thermodynamics of Crystals: Theories of Heat Capacities
  • 16.6 Electrical Conductivity in Solids
  • 16.7 Optical Properties of Solids
  • 17 The Liquid State
  • 17.1 Liquids Compared with Dense Gases
  • 17.2 Liquids Compared with Solids
  • 17.3 Intermolecular Forces
  • 17.4 Theories and Models of Liquids
  • 17.5 Water, the Incomparable Liquid
  • 17.6 The Hydrophobic Effect
  • 18 Surface Chemistry and Colloids
  • 18.1 Adsorption
  • 18.2 Adsorption Isotherms
  • 18.3 Thermodynamics and Statistical Mechanics of Adsorption
  • 18.4 Chemical Reactions on Surfaces
  • 18.5 Surface Heterogeneity
  • 18.6 The Structure of Solid Surfaces and of Adsorbed Layers
  • 18.7 Surface Tension and Capillarity
  • 18.8 Liquid Films on Surfaces Biography: Agnes Pockels
  • 18.9 Colloidal Systems
  • 19 Transport Properties
  • 19.1 Viscos

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