相平衡、相图和相变 : 其热力学基础 : 第2版

Preface to second edition page xiiPreface to first edition xiii1 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

Preface to second edition page xiiPreface to first edition xiii1 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 Entropy2 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 relations3 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 force4 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 sublattices5 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 principle6 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 principle7 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 product8 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 pressure9 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 diagrams10 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 equilibria11 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 phases12 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 potential13 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 elements15 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 points16 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 drag17 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 dissipation18 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 gas19 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 solutions20 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 systems21 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 solutions22 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 effectsReferencesIndex

《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。

《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。