Preface 1. INTRODUCTION AND DEFINITION OF TERMS Introduction The
Concept of State Simple Equilibrium The Equation of State of an
Ideal Gas The Units of Energy and Work Extensive and Intensive
Properties Phase Diagrams and Thermodynamic Components 2. THE FIRST
LAW OF THERMODYNAMICS 2.1 Introduction 2.2 The Relationship between
Heat and Work 2.3 Internal Energy and the First Law of
Thermodynamics 2.4 Constant-Volume Processes 2.5 Constant-Pressure
Processes and the Enthalpy H 2.6 Heat Capacity 2.7 Reversible
Adiabatic Processes 2.8 Reversible Isothermal Pressure or Volume
Changes of an Ideal Gas 2.9 Summary 2.10 Numerical Examples
Problems 3. THE SECOND LAW OF THERMODYNAMICS 3.1 Introduction 3.2
Spontaneous or Natural Processes 3.3 Entropy and the Quantification
of Irreversibility 3.4 Reversible Processes 3.5 An Illustration of
Irreversible and Reversible Processes 3.6 Entropy and Reversible
Heat 3.7 The Reversible Isothermal Compression of an Ideal Gas 3.8
The Reversible Adiabatic Expansion of an Ideal Gas 3.9 Summary
Statements 3.10 The Properties of Heat Engines 3.11 The
Thermodynamic Temperature Scale 3.12 The Second Law of
Thermodynamics 3.13 Maximum Work 3.14 Entropy and the Criterion for
Equilibrium 3.15 The Combined Statement of the First and Second
Laws of Thermodynamics 3.16 Summary 3.17 Numerical Examples
Problems 4. THE STATISTICAL INTERPRETATION OF ENTROPY 4.1
Introduction 4.2 Entropy and Disorder on an Atomic Scale 4.3 The
Concept of Microstate 4.4 Determination of the Most Probable
Microstate 4.5 The Influence of Temperature 4.6 Thermal Equilibrium
and the Boltzmann Equation 4.7 Heat Flow and the Production of
Entropy 4.8 Configurational Entropy and Thermal Entropy 4.9 Summary
4.10 Numerical Examples Problems 5. AUXILIARY FUNCTIONS 5.1
Introduction 5.2 The Enthalpy H 5.3 The Helmholtz Free Energy A 5.4
The Gibbs Free Energy G 5.5 Summary of the Equations for a Closed
System 5.6 The Variation of the Composition and Size of the System
5.7 The Chemical Potential 5.8 Thermodynamic Relations 5.9
Maxwell's Equations 5.10 The Upstairs-Downstairs-Inside-Out Formula
5.11 The Gibbs-Helmholtz Equation 5.12 Summary 5.13 Example of the
Use of the Thermodynamic Relations Problems 6. HEAT CAPACITY,
ENTHALPY, ENTROPY, AND THE THIRD LAW OF THERMODYNAMICS 6.1
Introduction 6.2 Theoretical Calculation of the Heat Capacity 6.3
The Empirical Representation of Heat Capacities 6.4 Enthalpy as a
Function of Temperature and Composition 6.5 The Dependence of
Entropy on Temperature and the Third Law of Thermodynamics 6.6
Experimental Verification of the Third Law 6.7 The Influence of
Pressure on Enthalpy and Entropy 6.8 Summary 6.9 Numerical Examples
Problems 7. PHASE EQUILIBRIUM IN A ONE-COMPONENT SYSTEM 7.1
Introduction 7.2 The Variation of Gibbs Free Energy with
Temperature at Constant Pressure 7.3 The Variation of Gibbs Free
Energy with Pressure at Constant Temperature 7.4 Gibbs Free Energy
as a Function of Temperature and Pressure 7.5 Equilibrium between
the Vapor Phase and a Condensed Phase 7.6 Graphical Representation
of Phase Equilibria in a One-Component System 7.7 Solid-Solid
Equilibria 7.8 Summary 7.9 Numerical Examples Problems 8. THE
BEHAVIOR OF GASES 8.1 Introduction 8.2 The P-V-T Relationships of
Gases 8.3 Deviations from Ideality and Equations of State for Real
Gases 8.4 The van der Waals Gas 8.5 Other Equations of State for
Nonideal Gases 8.6 The Thermodynamic Properties of Ideal Gases and
Mixtures of Ideal Gases 8.7 The Thermodynamic Treatment of Nonideal
Gases 8.8 Summary 8.9 Numerical Examples Problems 9. THE BEHAVIOR
OF SOLUTIONS 9.1 Introduction 9.2 Raoult's Law and Henry's Law 9.3
The Thermodynamic Activity of a Component in Solution 9.4 The
Gibbs-Duhem Equation 9.5 The Gibbs Free Energy of Formation of a
Solution 9.6 The Properties of Raoultian Ideal Solutions 9.7
Nonideal Solutions 9.8 Application of the Gibbs-Duhem Relation to
the Determination of Activity 9.9 Regular Solutions 9.10 A
Statistical Model of Solutions 9.11 Subregular Solutions 9.12
Summary 9.13 Numerical Examples Problems 10. GIBBS FREE
ENERGY-COMPOSITION AND PHASE DIAGRAMS OF BINARY SYSTEMS 10.1
Introduction 10.2 Gibbs Free Energy and Thermodynamic Activity 10.3
The Gibbs Free Energy of Formation of Regular Solutions 10.4
Criteria for Phase Stability in Regular Solutions 10.5 Liquid and
Solid Standard States 10.6 Phase Diagrams, Gibbs Free Energy, and
Thermodynamic Activity 10.7 The Phase Diagrams of Binary Systems
That Exhibit Regular Solution Behavior in the Liquid and Solid
States 10.8 Summary 10.9 Numerical Example Problems 11. REACTIONS
INVOLVING GASES 11.1 Introduction 11.2 Reaction Equilibrium in a
Gas Mixture and the Equilibrium Constant 11.3 The Effect of
Temperature on the Equilibrium Constant 11.4 The Effect of Pressure
on the Equilibrium Constant 11.5 Reaction Equilibrium as a
Compromise between Enthalpy and Entropy 11.6 Reaction Equilibrium
in the System SO2(g)-SO3(g)-O2(g) 11.7 Equilibrium in H2O-H2 and
CO2-CO Mixtures 11.8 Summary 11.9 Numerical Examples Problems 12.
REACTIONS INVOLVING PURE CONSENSED PHASES AND A GASEOUS PHASE 12.1
Introduction 12.2 Reaction Equilibrium in a System Containing Pure
Condensed Phases and a Gas Phase 12.3 The Variation of the Standard
Gibbs Free Energy Change with Temperature 12.4 Ellingham Diagrams
12.5 The Effect of Phase Transformations 12.6 The Oxides of Carbon
12.7 Graphical Representation of Equilibria in the System
Methal-Carbon-Oxygen 12.8 Summary 12.9 Numerical Examples Problems
13. REACTION EQUILIBRIA IN SYSTEMS CONTAINING COMPONENTS IN
CONDENSED SOLUTIONS 13.1 Introduction 13.2 The Criteria for
Reaction Equilibrium in Systems Containing Components in Condensed
Solution 13.3 Alternative Standard States 13.4 The Gibbs Phase Rule
13.5 Binary Systems Containing Compounds 13.6 Graphical
Representation of Phase Equilibria 13.7 The Formation of Oxide
Phases of Variable Composition 13.8 The Solubility of Gases in
Metals 13.9 Solutions Containing Several Dilute Solutes 13.10
Summary 13.11 Numerical Examples Problems 14. PHASE DIAGRAMS FOR
BINARY SYSTEMS IN PRESSURE-TEMPERATURE-COMPOSITION SPACE 14.1
Introduction 14.2 A Binary System Exhibiting Complete Mutual
Solubility of the Components in the Solid and Liquid States. 14.3 A
Binary System Exhibiting Complete Mutual Solubility in the Solid
and Liquid States and Showing Minima on the Melting, Boiling, and
Sublimation Curves 14.4 A Binary System Containing a Eutectic
Equilibrium and Having Complete Mutual Solubility in the Liquid
14.5 A Binary System Containing a Peritectic Equilibrium and Having
Complete Mutual Solubility in the Liquid State 14.6 Phase
Equilibrium in a Binary System Containing an Intermediate y Phase
That Melts, Sublimes, and Boils Congruently 14.7 Phase Equilibrium
in a Binary System Containing and Intermediate y Phase That Melts
and Sublimes Congruently and Boils Incongruently 14.8 Phase
Equilibrium in a Binary System with a Eutectic and One Component
That Exhibits Allotropy 14.9 A Binary Eutectic System in Which Both
Components Exhibit Allotropy 14.10 Phase Equilibrium at Low
Pressure: The Cadmium-Zinc System 14.11 Phase Equilibrium at High
Pressure: The Na2O * Al2O3 * 2SiO2 - SiO2 System 14.12 Summary 15.
ELECTROCHEMISTRY 15.1 Introduction 15.2 The Relationship between
Chemical and Electrical Driving Forces 15.3 The Effect of
Concentration on EMF 15.4 Formation Cells 15.5 Concentration Cells
15.6 The Temperature Coefficient of EMF 15.7 Heat Effects 15.8 The
Thermodynamics of Aqueous Solutions 15.9 The Gibbs Free Energy of
Formation of Ions and Standard Reduction Potentials 15.10 Pourbaix
Diagrams 15.11 Summary 15.12 Numerical Examples Problems Appendix
A: Selected Thermodynamic and Thermochemical Data Appendix B Exact
Differential Equations Appendix C The Generation of Auxiliary
Functions as Legendre Transformations
Nomenclatures
Answers
Index
"'This is an excellent book...it's really what a 'standard'
textbook should be: it is detailed, and complete, but builds up
from the basics rather than jumping straight in to advanced
concepts...I like the iclusion of questions, most importantly, with
solutions, and the worked examples are also a valuable resource.
Plenty of diagrams for explanations, all clearly referenced and
sensibly placed; and there are useful appendices and references.'.
Dr. Zoe Barber, Department of Materials Science & Metallurgy,
University of Cambridge, UK.."
""T...he long life of this textbook is as good an evaluation of its
quality as any book reviewer's praise. ...It will remain as a
classic for times to come..."
."
LIBRARY
-MRS Bulletin, December 2004
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