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Introduction to the Thermodynamics of Materials, Fifth Edition 4th New edition [Kietas viršelis]

3.80/5 (103 ratings by Goodreads)
(Carnegie Mellon University, Pittsburgh, Pennsylvania, USA), (Purdue University, West Lafayette, Indiana, USA)
  • Formatas: Hardback, 634 pages, aukštis x plotis: 229x152 mm, weight: 1134 g, 375 Illustrations, color
  • Išleidimo metai: 07-Feb-2003
  • Leidėjas: Taylor & Francis Inc
  • ISBN-10: 1560329920
  • ISBN-13: 9781560329923
Kitos knygos pagal šią temą:
Introduction to the Thermodynamics of Materials, Fifth Edition 4th New editionDidesnis paveikslėlis
  • Formatas: Hardback, 634 pages, aukštis x plotis: 229x152 mm, weight: 1134 g, 375 Illustrations, color
  • Išleidimo metai: 07-Feb-2003
  • Leidėjas: Taylor & Francis Inc
  • ISBN-10: 1560329920
  • ISBN-13: 9781560329923
Kitos knygos pagal šią temą:
Pastovi nuoroda: https://www.kriso.lt/db/9781560329923.html
Raktažodžiai:
Gaskell (materials engineering, Purdue U.) presents an introduction to the theory and application of the systems behavior of metallic and non-metallic materials. Chapters cover such topics as entropy, behavior of gases and solutions, various chemical reactions, and electrochemistry. The CD-ROM contains spreadsheet data and descriptive material for making thermodynamic calculations involving materials processing. This text is a revision of Introduction to metallurgical thermodynamics , 2nd ed. (1981). Annotation (c) Book News, Inc., Portland, OR (booknews.com)

This classic textbook is the definitive introduction to the thermodynamic behavior of materials systems. Written as a basic text for advanced undergraduates and first year graduate students in metallurgy, metallurgical engineering, ceramics, or materials science, it presents the underlying thermodynamic principles of materials and their plethora of applications. The book is also of proven interest to working professionals in need of a reference or refresher course.
Preface xiii
Introduction and Definition of Terms
1(14)
Introduction
1(1)
The Concept of State
1(3)
Simple Equilibrium
4(1)
The Equation of State of an Ideal Gas
5(3)
The Units of Energy and Work
8(1)
Extensive and Intensive Properties
8(1)
Phase Diagrams and Thermodynamic Components
9(6)
The First Law of Thermodynamics
15(22)
Introduction
15(1)
The Relationship between Heat and Work
16(1)
Internal Energy and the First Law of Thermodynamics
17(4)
Constant-Volume Processes
21(1)
Constant-Pressure Processes and the Enthalpy H
21(1)
Heat Capacity
21(4)
Reversible Adiabatic Processes
25(2)
Reversible Isothermal Pressure or Volume Changes of an Ideal Gas
27(1)
Summary
28(1)
Numerical Examples
29(8)
Problems
34(3)
The Second Law of Thermodynamics
37(32)
Introduction
37(1)
Spontaneous or Natural Processes
38(1)
Entropy and the Quantification of Irreversibility
39(1)
Reversible Processes
40(1)
An Illustration of Irreversible and Reversible Processes
41(2)
Entropy and Reversible Heat
43(3)
The Reversible Isothermal Compression of an Ideal Gas
46(1)
The Reversible Adiabatic Expansion of an Ideal Gas
47(1)
Summary Statements
48(1)
The Properties of Heat Engines
48(3)
The Thermodynamic Temperature Scale
51(2)
The Second Law of Thermodynamics
53(2)
Maximum Work
55(2)
Entropy and the Criterion for Equilibrium
57(1)
The Combined Statement of the First and Second Laws of Thermodynamics
58(1)
Summary
59(2)
Numerical Examples
61(8)
Problems
66(3)
The Statistical Interpretation of Entropy
69(18)
Introduction
69(1)
Entropy and Disorder on an Atomic Scale
70(1)
The Concept of Microstate
71(1)
Determination of the Most Probable Microstate
72(4)
The Influence of Temperature
76(2)
Thermal Equilibrium and the Boltzmann Equation
78(1)
Heat Flow and the Production of Entropy
79(1)
Configurational Entropy and Thermal Entropy
80(3)
Summary
83(1)
Numerical Examples
84(3)
Problems
86(1)
Auxiliary Functions
87(22)
Introduction
87(2)
The Enthalpy H
89(1)
The Helmholtz Free Energy A
89(5)
The Gibbs Free Energy G
94(1)
Summary of the Equations for a Closed System
95(1)
The Variation of the Composition and Size of the System
96(1)
The Chemical Potential
97(1)
Thermodynamic Relations
98(1)
Maxwell's Equations
99(2)
The Upstairs-Downstairs-Inside-Out Formula
101(1)
The Gibbs-Helmholtz Equation
102(1)
Summary
103(1)
Example of the Use of the Thermodynamic Relations
104(5)
Problems
106(3)
Heat Capacity, Enthalpy, Entropy, and the Third Law of Thermodynamics
109(40)
Introduction
109(1)
Theoretical Calculation of the Heat Capacity
110(5)
The Empirical Representation of Heat Capacities
115(1)
Enthalpy as a Function of Temperature and Composition
116(9)
The Dependence of Entropy on Temperature and the Third Law of Thermodynamics
125(3)
Experimental Verification of the Third Law
128(6)
The Influence of Pressure on Enthalpy and Entropy
134(2)
Summary
136(1)
Numerical Examples
137(12)
Problems
147(2)
Phase Equilibrium in a One-Component System
149(28)
Introduction
149(1)
The Variation of Gibbs Free Energy with Temperature at Constant Pressure
150(7)
The Variation of Gibbs Free Energy with Pressure at Constant Temperature
157(2)
Gibbs Free Energy as a Function of Temperature and Pressure
159(1)
Equilibrium between the Vapor Phase and a Condensed Phase
160(2)
Graphical Representation of Phase Equilibria in a One-Component System
162(6)
Solid-Solid Equilibria
168(3)
Summary
171(6)
Numerical Examples
172(3)
Problems
175(2)
The Behavior of Gases
177(34)
Introduction
177(1)
The P-V-T Relationships of Gases
177(3)
Deviations from Ideality and Equations of State for Real Gases
180(2)
The van der Waals Gas
182(9)
Other Equations of State for Nonideal Gases
191(1)
The Thermodynamic Properties of Ideal Gases and Mixtures of Ideal Gases
192(6)
The Thermodynamic Treatment of Nonideal Gases
198(6)
Summary
204(2)
Numerical Examples
206(5)
Problems
208(3)
The Behavior of Solutions
211(52)
Introduction
211(1)
Raoult's Law and Henry's Law
211(4)
The Thermodynamic Activity of a Component in Solution
215(1)
The Gibbs-Duhem Equation
216(2)
The Gibbs Free Enrgy of Formation of a Solution
218(3)
The Properties of Raoultian Ideal Solutions
221(5)
Nonideal Solutions
226(3)
Application of the Gibbs-Duhem Relation to the Determination of Activity
229(11)
Regular Solutions
240(5)
A Statistical Model of Solutions
245(7)
Subregular Solutions
252(2)
Summary
254(3)
Numerical Examples
257(6)
Problems
259(4)
Gibbs Free Energy Composition and Phase Diagrams of Binary Systems
263(42)
Introduction
263(1)
Gibbs Free Energy and Thermodynamic Activity
264(2)
The Gibbs Free Energy of Formation of Regular Solutions
266(2)
Criteria for Phase Stability in Regular Solutions
268(5)
Liquid and Solid Standard States
273(10)
Phase Diagrams, Gibbs Free Energy, and Thermodynamic Activity
283(9)
The Phase Diagrams of Binary Systems That Exhibit Regular Solution Behavior in the Liquid and Solid States
292(6)
Summary
298(1)
Numerical Examples
299(6)
Problems
301(4)
Reactions Involving Gases
305(32)
Introduction
305(1)
Reaction Equilibrium in a Gas Mixture and the Equilibrium Constant
306(5)
The Effect of Temperature on the Equilibrium Constant
311(1)
The Effect of Pressure on the Equilibrium Constant
312(2)
Reaction Equilibrium as a Compromise between Enthalpy and Entropy
314(2)
Reaction Equilibriu in the System SO2(g)-SO3(g)-O2(g)
316(5)
Equilibrium in H2O-H2 and CO2-CO Mixtures
321(2)
Summary
323(1)
Numerical Examples
324(13)
Problems
335(2)
Reactions Involving Pure Condensed Phases and a Gaseous Phase
337(46)
Introduction
337(1)
Reaction Equilibrium in a System Containing Pure Condensed Phases and a Gas Phase
338(5)
The Variation of the Standard Gibbs Free Energy Change with Temperature
343(3)
Ellingham Diagrams
346(7)
The Effect of Phase Transformations
353(5)
The Oxides of Carbon
358(7)
Graphical Representation of Equilibria in the System Metal-Carbon-Oxygen
365(3)
Summary
368(1)
Numerical Examples
369(14)
Problems
380(3)
Reaction Equilibria in Systems Containing Components in Condensed Solution
383(92)
Introduction
383(2)
The Criteria for Reaction Equilibrium in Systems Containing Components in Condensed Solution
385(8)
Alternative Standard States
393(6)
The Gibbs Phase Rule
399(18)
Binary Systems Containing Compounds
417(12)
Graphical Representation of Phase Equilibria
429(8)
The Formation of Oxide Phases of Variable Composition
437(9)
The Solubility of Gases in Metals
446(4)
Solutions Containing Several Dilute Solutes
450(10)
Summary
460(2)
Numerical Examples
462(13)
Problems
470(5)
Phase Diagrams for Binary Systems in Pressure-Temperature-Composition Space
475(58)
Introduction
475(1)
A Binary System Exhibiting Complete Mutual Solubility of the Components in the Solid and Liquid States
475(5)
A Binary System Exhibiting Complete Mutual Solubility in the Solid and Liquid States and Showing Minima on the Melting, Boiling, and Sublimation Curves
480(5)
A Binary System Containing a Eutectic Equilibrium and Having Complete Mutual Solubility in the Liquid
485(8)
A Binary System Containing a Peritectic Equilibrium and Having Complete Mutual Solubility in the Liquid State
493(8)
Phase Equilibrium in a Binary System Containing an Intermediate γ Phase That Melts, Sublimes, and Boils Congruently
501(7)
Phase Equilibrium in a Binary System Containing an Intermediate γ Phase That Melts and Sublimes Congruently and Boils Incongruently
508(5)
Phase Equilibrium in a Binary System with a Eutectic and One Component That Exhibits Allotropy
513(4)
A Binary Eutectic System in Which Both Components Exhibit Allotropy
517(7)
Phase Equilibrium at Low Pressure: The Cadmium-Zinc System
524(1)
Phase Equilibrium at High Pressure: The Na2O.Al2O3.2SiO2-SiO2 System
525(6)
Summary
531(2)
Electrochemistry
533(66)
Introduction
533(2)
The Relationship between Chemical and Electrical Driving Forces
535(5)
The Effect of Concentration on EMF
540(1)
Formation Cells
541(3)
Concentration Cells
544(5)
The Temperature Coefficient of the EMF
549(2)
Heat Effects
551(1)
The Thermodynamics of Aqueous Solutions
552(3)
The Gibbs Free Energy of Formation of Ions and Standard Reduction Potentials
555(9)
Pourbaix Diagrams
564(10)
Summary
574(2)
Numerical Examples
576(5)
Problems
579(2)
Appendices
A Selected Thermodynamic and Thermochemical Data
581(8)
B Exact Differential Equations
589(2)
C The Generation of Auxiliary Functions as Legendre Transformations
591(8)
Nomenclature 599(4)
Answers 603(12)
Index 615