Phase Equilibria, Phase Diagrams and Phase Transformations – Mats Hillert – 2nd Edition

Prefacios
•Preface to second edition
•Preface to first edition
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 + 1
•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 ? 1
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
Apéndices
•References
•Index