Phase transformations / Michel Soustelle.

Format:

Book

Author/Creator:

Soustelle, Michel, author.

Series:

Chemical engineering series (ISTE Ltd.)

Chemical thermodynamics set ; v. 5.

Chemical engineering series

Chemical thermodynamics set ; volume 5

Language:

English

Subjects (All):

Thermodynamics.

Chemical reactions.

Phase transformations (Statistical physics).

Physical Description:

1 online resource (252 pages) : illustrations (some color)

Edition:

1st ed.

Place of Publication:

Hoboken, New Jersey : ISTE Ltd/John Wiley and Sons Inc, 2015.

Summary:

This book is part of a set of books which offers advanced students successive characterization tool phases, the study of all types of phase (liquid, gas and solid, pure or multi-component), process engineering, chemical and electrochemical equilibria, and the properties of surfaces and phases of small sizes. Macroscopic and microscopic models are in turn covered with a constant correlation between the two scales. Particular attention has been given to the rigor of mathematical developments. This fifth volume is devoted to the study of transformations and equilibria between phases. First- and second-order pure phase transformations are presented in detail, just as with the macroscopic and microscopic approaches of phase equilibria. In the presentation of binary systems, the thermodynamics of azeotropy and demixing are discussed in detail and applied to strictly-regular solutions. Eutectic and peritectic points are examined, as well as the reactions that go with them. The study of ternary systems then introduces the concepts of ternary azeotropes and eutectics. For each type of solid-liquid system, the interventions of definite compounds with or without congruent melting are taken into account. The particular properties of the different notable points of a diagram are also demonstrated.

Contents:

Cover

Title Page

Copyright

Contents

Preface

Notations and Symbols

1: Phase Transformations of Pure Substances

1.1. Standard state: standard conditions of a transformation

1.2. Classification and general properties of phase transformations

1.2.1. First-order transformations and the Clapeyron relation

1.2.2. Second-order transformations

1.2.2.1. Ehrenfest equations

1.2.2.2. Landau theory

1.2.2.2.1. Symmetry and order parameters

1.2.2.2.2. Second-order transitions according to Landau

1.2.2.2.3. Critical exponents

1.2.2.2.4. Limitation of Landau's model

1.3. Liquid-vapor transformations and equilibrium states

1.3.1. Method of two equations of state, using the Clapeyron equation

1.3.2. Gibbs energy and fugacity method

1.3.3. Unique equation of state method

1.3.4. The region of the critical point and spinodal decomposition

1.3.5. Microscopic modeling

1.3.6. Liquid-vapor equilibrium in the presence of an inert gas

1.4. Solid-vapor transformations and equilibriums

1.4.1. Macroscopic treatment

1.4.2. Microscopic treatment

1.5. Transformations and solid-liquid equilibria

1.5.1. Macroscopic treatment

1.5.2. Microscopic treatment

1.6. Diagram for the pure substance and properties of the triple point

1.7. Allotropic and polymorphic varieties of a solid

1.7.1. Enantiotropy

1.7.2. Monotropy

1.7.3. Transition from enantiotropy to monotropy and vice versa

1.8. Mesomorphic states

2: Properties of Equilibria Between Binary Phases

2.1. Classification of equilibria between the phases of binary systems

2.2. General properties of two-phase binary systems

2.2.1. Equilibrium conditions for two-phase binary systems

2.2.2. Conditions of evolution of a two-phase binary system

2.3. Graphical representation of two-phase binary systems.

2.3.1. Gibbs energy graphs

2.3.2. Phase diagram in the mono- and bi-phase zones

2.3.2.1. Construction of the isobaric phase diagram in the mono- or biphasic regions

2.3.2.2. Properties of phase diagrams in regions with one or two phases

2.3.2.2.1. The lever rule or law of chemical moments

2.3.2.2.2. Crossing a line in the diagram

2.3.2.2.3. Gibbs-Konovalov theorem

2.3.2.2.4. The different types of azeotropic points

2.3.2.2.5. Property of the vertical axes at X1(α)=0 and X1(α)=1 in the phase diagram

2.3.2.3. Particular configurations of a diagram in the regions with one or two phases

2.3.2.3.1. One component is completely immiscible with the other

2.3.2.3.2. The two components may be entirely miscible with one another

2.3.3. Isobaric cooling curves

2.4. Isobaric representation of three-phase binary systems

2.4.1. Gibbs energy curve

2.4.2. Isobaric phase diagram in tri-phase regions

2.4.3. Isobaric cooling curves with tri-phase zones

2.5. Isothermal phase diagrams

2.6. Composition/composition curves

2.7. Activity of the components and consequences of Raoult's and Henry's laws

3: Equilibria Between Binary Condensed Phases

3.1. Equilibria between phases of the same nature: liquid-liquid or solid-solid

3.1.1. Thermodynamics of demixing

3.1.2. Demixing in the case of low reciprocal solubilities

3.1.3. Demixing of strictly-regular solutions

3.2. Liquid-solid systems

3.2.1. Thermodynamics of the equilibria between a liquid phase and a solid phase

3.2.2. Isobaric phase diagrams of equilibria between a solid and a liquid

3.2.2.1. Miscible components in all proportions in the two phases

3.2.2.2. Equilibria between a solid and a liquid with demixing of the solid phase

3.2.2.3. Equilibria between a solid and a liquid with demixing of the liquid phase.

3.2.2.4. Three-phase reactions in liquid-solid systems

3.2.2.5. Systems with formations of definite compounds

3.2.3. Solidus and liquidus in the vicinity of the pure substance

3.3. Equilibria between two solids with two polymorphic varieties of the solid

3.4. Applications of solid-liquid equilibria

3.4.1. Solubility of a solid in a liquid: Schröder-Le Châtelier law

3.4.1.1. Thermodynamics of solubility

3.4.1.2. Curves of solubility of salts in water

3.4.2. Determination of molar mass by cryometry

3.5. Membrane equilibria - osmotic pressure

3.5.1. Thermodynamics of osmotic pressure

3.5.2. Osmotic pressure of infinitely-dilute solutions: the Van 't Hoff law

3.5.3. Application of osmotic pressure to the determination of the molar mass of polymers

3.5.4. Osmotic pressure of strictly-regular solutions

3.5.5. Osmotic pressure and the osmotic coefficient

4: Equilibria Between Binary Fluid Phases

4.1. Thermodynamics of liquid-vapor equilibrium in a binary system

4.2. Liquid-vapor equilibrium in perfect solutions far from the critical conditions

4.2.1. Partial pressures and total pressure of a perfect solution

4.2.2. Isothermal diagram of a perfect solution

4.2.3. Isobaric diagram of a perfect solution

4.2.4. Phase composition curve

4.3. Liquid-gas equilibria in ideal dilute solutions

4.4. Diagrams of the liquid-vapor equilibria in real solutions

4.4.1. Total miscibility in the liquid phase

4.4.1.1. Isobaric diagrams

4.4.1.2. Isothermal diagrams

4.4.1.3. Partial pressures and total pressure

4.4.2. Partial miscibility in the liquid phase, heteroazeotropes

4.5. Thermodynamics of liquid-vapor azeotropy

4.5.1. Relation between the pressure of the azeotrope and the activity coefficients of the liquid phase at the azeotropic composition.

4.5.2. Relation between the activity coefficient and the temperature of the azeotrope

4.6. Liquid-vapor equilibria and models of solutions

4.6.1. Liquid-vapor equilibria in strictly-regular solutions

4.6.1.1. Azeotropy of strictly-regular solutions

4.6.1.1.1. Relation between temperature and composition of the azeotrope

4.6.1.1.2. Relation between composition and pressure in the azeotrope

4.6.1.1.3. Relation between the pressure and temperature of the azeotrope

4.6.1.1.4. Condition for the existence of the azeotrope

4.6.1.2. Liquid-vapor equilibrium and demixing of the liquid

4.6.2. Liquid-vapor equilibrium in associated solutions

4.7. Liquid-vapor equilibria in the critical region

4.8. Applications of liquid-vapor equilibria

4.8.1. Solubility of a gas in a liquid

4.8.2. Determination of molar masses by tonometry

4.8.3. Determination of molar masses by ebulliometry

4.8.4. Continuous rectification or fractional distillation

4.8.4.1. Insufficiency of simple distillation

4.8.4.2. Rectification in the case of a single-spindle binary system

4.8.4.2.1. Feasibility of separation by fractional distillation

4.8.4.2.2. Total reflux operation

theoretical trays

4.8.4.2.3. The Fenske equation

4.8.4.2.4. McCabe and Thiele diagram

4.8.4.2.5. Partial reflux operation. Sorel's equation

4.8.4.3. Fractional distillation in the presence of an azeotrope

5: Equilibria Between Ternary Fluid Phases

5.1. Representation of the composition of ternary systems

5.1.1. Symmetrical representation of the Gibbs triangle

5.1.2. Dissymmetrical representation of the right triangle

5.2. Representation of phase equilibria

5.2.1. Isothermal projections

5.2.2. Conjugate points and conodes

5.2.3. Isopleth sections

5.3. Equilibria in liquid phases with miscibility gaps.

5.3.1. Representation of the miscibility gap

5.3.2. Sharing in liquid-liquid systems

5.3.2.1. The shared substance has the same constitution in the two solvents

5.3.2.2. The shared substance does not have the same constitution in the two solvents

5.3.3. Application of sharing between two liquids to solvent extraction

5.3.3.1. Discontinuous extractions

5.3.3.2. Multi-stage counterflow extraction

5.4. Liquid-vapor systems

5.4.1. Isothermal and isopleth sections (boiling and dew)

5.4.2. Distillation trajectories

5.4.3. Systems with two distillation fields

5.4.4. Systems with three distillation fields

5.5. Examples of applications of ternary diagrams between fluid phases

5.5.1. Treatment of argentiferous lead

5.5.2. Purity of oil products: aniline point

5.5.3. Obtaining concentrated ethyl alcohol

6: Equilibria Between Condensed Ternary Fluid Phases

6.1. Solidification of a ternary system with total miscibility in the liquid state and in the solid state

6.2. Solidification of a ternary system with no miscibility and with a ternary eutectic

6.2.1. Invariant transformations of a liquid-solid ternary system

6.2.2. Representations of the ternary system with no miscibility in the solid state

6.2.2.1. The isobaric three-dimensional representation

6.2.2.2. Projection of an isothermal section

6.2.2.3. Cooling and solidification of a given liquid

6.2.2.4. Solidification trajectory

6.2.3. Lowering of the melting point of a binary system by the addition of a component

6.2.4. Slope at the ternary eutectic

6.3. Ternary systems with partial miscibilities in the solid state and ternary eutectic

6.4. Solidification of ternary systems with definite compounds

6.4.1. Ternary system with a binary definite compound binary with congruent melting.

6.4.2. Generalization to the case of a ternary compound and of multiple definite compounds.

Notes:

Includes bibliographical references and index.

Description based on print version record.

ISBN:

9781119178590

1119178592

9781119178583

1119178584

OCLC:

930041302