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　　《相平衡、相图和相变——其热力学基础（第二版）》是影印版英文专著，原书由剑桥大学出版社于2008年出版。相平衡、相变等热力学原理是理解、设计材料属性的基础。计算工具的出现使材料学家能够处理越来越复杂的情况，但对于热力学基础理论的理解也越来越重要。本书图文并茂，深入浅出地讲解了热力学原理以及在计算机计算中的应用，对于材料科学、材料工程方面的研究者会有很大帮助。

内容简介

　　《相平衡、相图和相变——其热力学基础（第二版）（英文影印版）》主要内容为现代计算机应用观点下的热力学基本原理。化学平衡和化学变化的理论基础也是本书的内容之一，其重点在于相图的性质。本书从基本原理出发，讨论延及多相的系统。第二版新增加的内容包括不可逆热力学、极值原理和表面、界面热力学等等。平衡条件的理论刻画、系统的平衡状态和达到平衡时的变化都以图解的形式给出。
　　《相平衡、相图和相变——其热力学基础（第二版）（英文影印版）》适合材料科学与工程领域的研究人员、研究生和高年级本科生阅读。

作者简介

　　(瑞典)希勒特（M. Hillert），瑞典皇家工学院教授。

目　　录

Preface to second edition page xii
Preface to first edition xiii
1 Basic concepts of thermodynamics
　1.1 External state variables
　1.2 Internal state variables
　1.3 The first law of thermodynamics
　1.4 Freezing-in conditions
　1.5 Reversible and irreversible processes
　1.6 Second law of thermodynamics
　1.7 Condition of internal equilibrium
　1.8 Driving force
　1.9 Combined first and second law
　1.10 General conditions of equilibrium
　1.11 Characteristic state functions

Preface to second edition page xii 
Preface to first edition xiii 
1 Basic concepts of thermodynamics  
　1.1 External state variables  
　1.2 Internal state variables  
　1.3 The first law of thermodynamics  
　1.4 Freezing-in conditions  
　1.5 Reversible and irreversible processes  
　1.6 Second law of thermodynamics  
　1.7 Condition of internal equilibrium  
　1.8 Driving force  
　1.9 Combined first and second law  
　1.10 General conditions of equilibrium  
　1.11 Characteristic state functions  
　1.12 Entropy  
2 Manipulation of thermodynamic quantities  
　2.1 Evaluation of one characteristic state function from another  
　2.2 Internal variables at equilibrium  
　2.3 Equations of state  
　2.4 Experimental conditions  
　2.5 Notation for partial derivatives  
　2.6 Use of various derivatives  
　2.7 Comparison between CV and CP  
　2.8 Change of independent variables  
　2.9 Maxwell relations  
3 Systems with variable composition  
　3.1 Chemical potential  
　3.2 Molar and integral quantities  
　3.3 More about characteristic state functions  
　3.4 Additivity of extensive quantities. Free energy and exergy  
　3.5 Various forms of the combined law  
　3.6 Calculation of equilibrium  
　3.7 Evaluation of the driving force  
　3.8 Driving force for molecular reactions  
　3.9 Evaluation of integrated driving force as function of 
　T or P  
　3.10 Effective driving force  
4 Practical handling of multicomponent systems  
　4.1 Partial quantities  
　4.2 Relations for partial quantities  
　4.3 Alternative variables for composition  
　4.4 The lever rule  
　4.5 The tie-line rule  
　4.6 Different sets of components  
　4.7 Constitution and constituents  
　4.8 Chemical potentials in a phase with sublattices  
5 Thermodynamics of processes  
　5.1 Thermodynamic treatment of kinetics of 
　internal processes  
　5.2 Transformation of the set of processes  
　5.3 Alternative methods of transformation  
　5.4 Basic thermodynamic considerations for processes  
　5.5 Homogeneous chemical reactions  
　5.6 Transport processes in discontinuous systems  
　5.7 Transport processes in continuous systems  
　5.8 Substitutional diffusion  
　5.9 Onsager’s extremum principle  
6 Stability  
　6.1 Introduction  
　6.2 Some necessary conditions of stability  
　6.3 Sufficient conditions of stability  
　6.4 Summary of stability conditions  
　6.5 Limit of stability  
　6.6 Limit of stability against fluctuations in composition  
　6.7 Chemical capacitance  
　6.8 Limit of stability against fluctuations of 
　internal variables  
　6.9 Le Chatelier’s principle  
7 Applications of molar Gibbs energy diagrams  
　7.1 Molar Gibbs energy diagrams for binary systems  
　7.2 Instability of binary solutions  
　7.3 Illustration of the Gibbs–Duhem relation  
　7.4 Two-phase equilibria in binary systems  
　7.5 Allotropic phase boundaries  
　7.6 Effect of a pressure difference on a two-phase 
　equilibrium  
　7.7 Driving force for the formation of a new phase  
　7.8 Partitionless transformation under local equilibrium  
　7.9 Activation energy for a fluctuation  
　7.10 Ternary systems  
　7.11 Solubility product  
8 Phase equilibria and potential phase diagrams  
　8.1 Gibbs’ phase rule  
　8.2 Fundamental property diagram  
　8.3 Topology of potential phase diagrams  
　8.4 Potential phase diagrams in binary and multinary systems  
　8.5 Sections of potential phase diagrams  
　8.6 Binary systems  
　8.7 Ternary systems  
　8.8 Direction of phase fields in potential phase diagrams  
　8.9 Extremum in temperature and pressure  
9 Molar phase diagrams  
　9.1 Molar axes  
　9.2 Sets of conjugate pairs containing molar variables  
　9.3 Phase boundaries  
　9.4 Sections of molar phase diagrams  
　9.5 Schreinemakers’ rule  
　9.6 Topology of sectioned molar diagrams  
10 Projected and mixed phase diagrams  
　10.1 Schreinemakers’ projection of potential phase diagrams  
　10.2 The phase field rule and projected diagrams  
　10.3 Relation between molar diagrams and Schreinemakers’ 
　projected diagrams  
　10.4 Coincidence of projected surfaces  
　10.5 Projection of higher-order invariant equilibria  
　10.6 The phase field rule and mixed diagrams  
　10.7 Selection of axes in mixed diagrams  
　10.8 Konovalov’s rule  
　10.9 General rule for singular equilibria  
11 Direction of phase boundaries  
　11.1 Use of distribution coefficient  
　11.2 Calculation of allotropic phase boundaries  
　11.3 Variation of a chemical potential in a two-phase field  
　11.4 Direction of phase boundaries  
　11.5 Congruent melting points  
　11.6 Vertical phase boundaries  
　11.7 Slope of phase boundaries in isothermal sections  
　11.8 The effect of a pressure difference between two phases  
12 Sharp and gradual phase transformations  
　12.1 Experimental conditions  
　12.2 Characterization of phase transformations  
　12.3 Microstructural character  
　12.4 Phase transformations in alloys  
　12.5 Classification of sharp phase transformations  
　12.6 Applications of Schreinemakers’ projection  
　12.7 Scheil’s reaction diagram  
　12.8 Gradual phase transformations at fixed composition  
　12.9 Phase transformations controlled by a chemical potential  
13 Transformations in closed systems  
　13.1 The phase field rule at constant composition  
　13.2 Reaction coefficients in sharp transformations 
　for p = c +　 
　13.3 Graphical evaluation of reaction coefficients  
　13.4 Reaction coefficients in gradual transformations 
　for p = c  
　13.5 Driving force for sharp phase transformations  
　13.6 Driving force under constant chemical potential  
　13.7 Reaction coefficients at constant chemical potential  
　13.8 Compositional degeneracies for p = c  
　13.9 Effect of two compositional degeneracies for p = c .　 
14 Partitionless transformations  
　14.1 Deviation from local equilibrium  
　14.2 Adiabatic phase transformation  
　14.3 Quasi-adiabatic phase transformation  
　14.4 Partitionless transformations in binary system  
　14.5 Partial chemical equilibrium  
　14.6 Transformations in steel under quasi-paraequilibrium  
　14.7 Transformations in steel under partitioning of alloying elements  
15 Limit of stability and critical phenomena  
　15.1 Transformations and transitions  
　15.2 Order–disorder transitions  
　15.3 Miscibility gaps  
　15.4 Spinodal decomposition  
　15.5 Tri-critical points  
16 Interfaces  
　16.1 Surface energy and surface stress  
　16.2 Phase equilibrium at curved interfaces  
　16.3 Phase equilibrium at fluid/fluid interfaces  
　16.4 Size stability for spherical inclusions  
　16.5 Nucleation  
　16.6 Phase equilibrium at crystal/fluid interface  
　16.7 Equilibrium at curved interfaces with regard to composition  
　16.8 Equilibrium for crystalline inclusions with regard to composition  
　16.9 Surface segregation  
　16.10 Coherency within a phase  
　16.11 Coherency between two phases  
　16.12 Solute drag  
17 Kinetics of transport processes  
　17.1 Thermal activation  
　17.2 Diffusion coefficients  
　17.3 Stationary states for transport processes  
　17.4 Local volume change  
　17.5 Composition of material crossing an interface  
　17.6 Mechanisms of interface migration  
　17.7 Balance of forces and dissipation  
18 Methods of modelling  
　18.1 General principles  
　18.2 Choice of characteristic state function  
　18.3 Reference states  
　18.4 Representation of Gibbs energy of formation  
　18.5 Use of power series in T  
　18.6 Representation of pressure dependence  
　18.7 Application of physical models  
　18.8 Ideal gas  
　18.9 Real gases  
　18.10 Mixtures of gas species  
　18.11 Black-body radiation  
　18.12 Electron gas  
19 Modelling of disorder  
　19.1 Introduction  
　19.2 Thermal vacancies in a crystal  
　19.3 Topological disorder  
　19.4 Heat capacity due to thermal vibrations  
　19.5 Magnetic contribution to thermodynamic properties  
　19.6 A simple physical model for the magnetic contribution  
　19.7 Random mixture of atoms  
　19.8 Restricted random mixture  
　19.9 Crystals with stoichiometric vacancies  
　19.10 Interstitial solutions  
20 Mathematical modelling of solution phases  
　20.1 Ideal solution  
　20.2 Mixing quantities  
　20.3 Excess quantities  
　20.4 Empirical approach to substitutional solutions  
　20.5 Real solutions  
　20.6 Applications of the Gibbs–Duhem relation  
　20.7 Dilute solution approximations  
　20.8 Predictions for solutions in higher-order systems  
　20.9 Numerical methods of predictions for higher-order systems  
21 Solution phases with sublattices  
　21.1 Sublattice solution phases  
　21.2 Interstitial solutions  
　21.3 Reciprocal solution phases  
　21.4 Combination of interstitial and substitutional solution  
　21.5 Phases with variable order  
　21.6 Ionic solid solutions  
22 Physical solution models  
　22.1 Concept of nearest-neighbour bond energies  
　22.2 Random mixing model for a substitutional solution  
　22.3 Deviation from random distribution  
　22.4 Short-range order  
　22.5 Long-range order  
　22.6 Long- and short-range order  
　22.7 The compound energy formalism with short-range order  
　22.8 Interstitial ordering  
　22.9 Composition dependence of physical effects  
References  
Index

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相平衡、相图和相变——其热力学基础（第二版）（英文影印版）下载

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