: Applications of Thermodynamics (SI Units), 4e, Volume 3

Title
Contents
1. Equilibrium Between Phases
	1.1 Thermodynamic Criterion of Phase Equilibria
	1.2 Chemical Potential Versus Temperature Graphs of a Pure Substance
	1.3 E ffect of Pressure on the Chemical Potential Versus Temperature Graphs
	1.4 Clapeyron Equation
	1.5 Application of Clapeyron Equation
	1.6 First- and Second-order Phase Transitions
	1.7 E ffect of Pressure on the Vapour Pressure of a Liquid
2. Colligative Properties
	2.1 Solution
	2.2 Methods of Expressing Concentration of a Solution
	2.3 L owering of Vapour Pressure – Experimental Observations
	2.4 Relative Lowering of Vapour Pressure
	2.5 Chemical Potentials of Solute and Solvent in an Ideal Liquid Solution
	2.6 Origin of Colligative Properties
	2.7 E levation of Boiling Point
	2.8 Depression of Freezing Point
	2.9 Osmosis and Osmotic Pressure
	2.10 Relations Between Different Colligative Properties
	2.11 Colligative Properties of Strong and Weak Electrolytes
	2.12 Solubility of a Solute in an Ideal Solution
3. Phase rule
	3.1 Introduction and Definitions
	3.2 Derivation of Phase Rule
	3.3 Some Typical Examples to Compute the Number of Components
4. Solutions
	4.1 I deal Solubility of Gases in Liquids
	4.2 E ffect of Pressure and Temperature on the Solubility of Gases
	4.3 H enry’s Law and Raoult’s Law
	4.4 Raoult’s Law for Solvent and Henry’s Law for Solute
	4.5 Derivations of Raoult’s and Henry’s Laws from Kinetic-Molecular Theory
	4.6 I deal and Ideally Dilute Solutions
	4.7 Variation of Henry’s Law Constant with Temperature
	4.8 Thermodynamics of Ideal Solutions of Liquid in Liquid
	4.9 Vapour Pressure of an Ideal Binary Liquid Solution
	4.10 Vapour Pressure-Composition Diagram of a Binary Liquid Solution
	4.11 I sothermal Fractional Distillation of an Ideal Binary Solution
	4.12 Temperature-Composition Diagram of a Binary Liquid Solution
	4.13 I sobaric Fractional Distillation of an Ideal Binary Solution
	4.14 Nonideal Solutions of Liquid in Liquid
	4.15 The Duhem-Margules Equation
	4.16 Temperature-Composition Diagrams of Nonideal Solutions
	4.17 Konowaloff’s Rule – Revisited
	4.18 Partially Miscible Liquids
	4.19 Completely Immiscible Liquids (Steam Distillation)
	4.20 Distribution of a Solute Between Two Immiscible Liquids – The Nernst Distribution Law
5. Phase Diagrams of One-Component Systems
	5.1 Application of the Phase Rule
	5.2 Qualitative Discussion of a Phase Diagram
	5.3 Phase Diagram of Water
	5.4 Polymorphism
6. Phase Diagrams of Two-Component Systems
	6.1 Application of the Phase Rule
	6.2 Classification of Diagrams
	6.3 Thermal Analysis
	6.4 Crystallization of Pure Components – Simple Eutectic Phase Diagram
	6.5 Crystallization of Pure Components and One of the Solids Exists in More than One Crystalline Form
	6.6 Formation of a Compound Stable up to Its Melting Point
	6.7 Formation of a Compound which Decomposes Before Attaining its Melting Point
	6.8 Formation of a Complete Series of Solid Solutions
	6.9 Formation of Partial Misciblity in the Solid State Leading to Stable Solid Solutions
	6.10 Formation of Partial Misciblity in the Solid Phase Leading to Solid Solutions Stable up to a Transition Temperature
	6.11 Formation of Partial Miscibility in the Liquid Phase and Crystallization of Pure Components
	6.12 Phase Diagrams of Aqueous Solutions of Salts
7. Phase Diagrams of Three-Component Systems
	7.1 Application of the Phase Rule
	7.2 Scheme of Triangular Plot
	7.3 Systems of Three Liquid Components Exhibiting Partial Miscibility
	7.4 Triangular Plots of a Ternary System Depicting Crystallization of its Components at Various Temperatures
	7.5 Ternary Systems of Two Solid Components and a Liquid
	7.6 Crystallization of Pure Components Only
	7.7 Formation of Binary Compounds such as Hydrates
	7.8 Formation of a Double Salt
	7.9 Formation of a Ternary Compound
	7.10 Formation of Solid Solutions
	7.11 Formation of Solid Solutions with Partial Miscibility
	7.12 Salting out Phenomenon
	7.13 E xperimental Methods Employed for Obtaining Triangular Plots
8. Electrochemical Cells
	8.1 Introduction
	8.2 Reversible and Irreversible Cells
	8.3 E lectromotive Force and its Measurement
	8.4 Formulation of a Galvanic Cell
	8.5 E lectrical and Electrochemical Potentials
	8.6 Different Types of Half-Cells and Their Reduction Potentials
	8.7 The Emf of a Cell and its Cell Reaction
	8.8 Determination of Standard Potentials
	8.9 Significance of Standard Half-Cell Potentials
	8.10 Influence of Ionic Activity on Reduction Potential
	8.11 E ffect of Complex Formation on Reduction Potential
	8.12 Relation Between Metal-metal Ion Half-Cell and the Corresponding Metal-Insoluble Salt-Anion Half-Cell
	8.13 Cell Reaction and its Relation with Cell Potential
	8.14 Calculation of Standard Potential for an Unknown Half-Cell Reaction
	8.15 Reference Half-Cells
	8.16 E xpression of Ecell in the Unit of Molality
	8.17 Determination of Accurate Value of Half-Cell Potential
	8.18 Applications of Electrochemical Cells
	8.19 Construction of Potentiometric Titration Curves
	8.20 Concentration Cells without Liquid Junction Potential
	8.21 Concentration Cells with Liquid Junction Potential
	8.22 Commercial Cells
	8.23 Solved Problems
	Annexure I: Concept of Activity
	Annexure II: Derivation of Debye-Hückel Law
	Annexure III: Operational Definition of pH
Appendix I: Units and Conversion Factors
Index