Chemical Thermodynamics: Basic Concepts and Methods

A new edition of the classic treatment of chemical thermodynamics
For more than fifty years, this critically acclaimed and highly influential publication has been the textbook of choice in the field of chemical thermodynamics. This Seventh Edition not only brings the text thoroughly up to date with the latest developments and applications, it also offers new features that better enable students to master key concepts and apply them in practice.
While thoroughly revised and updated, the text′s fundamental objectives remain unchanged: to present the foundations and interrelationships of thermodynamics and to enable students to apply basic concepts in solving problems typically encountered by chemists, biologists, geologists, and materials scientists. Moreover, the text continues to maintain a logical unity throughout by focusing on the laws of classical thermodynamics and applications to gases, solutions, phase equilibria, and chemical equilibria.
Designed to meet the needs of today′s students and instructors, the text offers:
Rigorous explanations of abstract concepts that are clear and simple
Logical organization of materials that enables students to progressively build and apply knowledge
Worked examples demonstrating how concepts are applied to solve actual problems
Detailed coverage of essential mathematical tools, with mathematical review chapters provided for additional support
A thorough presentation of graphical, numerical, and analytical computational techniques
Exercises that accurately reflect the types of problems encountered by practicing scientists
An explanation of the treatment of mixtures of gases, followed by an explanation of thetreatment of chemical equilibrium
A new discussion of the relation of Henry′s law to regular solutions and the relation of regular solutions to limited miscibility
Updated to reflect the latest applications in science and engineering, Chemical Thermo–dynamics continues to set the standard in its field.

Spis treści:
PREFACE.
1 INTRODUCTION.
1.1 Origins of Chemical Thermodynamics.
1.2 Objectives of Chemical Thermodynamics.
1.3 Limitations of Classic Thermodynamics.
References.
2 MATHEMATICAL PREPARATION FOR THERMODYNAMICS.
2.1 Variables of Thermodynamics.
Extensive and Intensive Quantities.
Units and Conversion Factors.
2.2 Analytic Methods.
Partial Differentiation.
Exact Differentials.
Homogeneous Functions.
Exercises.
References 
3 THE FIRST LAW OF THERMODYNAMICS.
3.1 Definitions.
Temperature.
Work.
3.2 The First Law of Thermodynamics.
Energy.
Heat.
General Form of the First Law.
Exercises.
References.
4 ENTHALPY, ENTHALPY OF REACTION, AND HEAT CAPACITY.
4.1 Enthalpy.
Definition.
Relationship between Qv and Qp.
4.2 Enthalpy of Reactions.
Definitions and Conventions.
4.3 Enthalpy as a State Function.
Enthalpy of Formation from Enthalpy of Reaction.
Enthalpy of Formation from Enthalpy of Combustion.
Enthalpy of Transition from Enthalpy of Combustion.
Enthalpy of Conformational Transition of a Protein from Indirect Calorimetric Measurements.
Enthalpy of Solid–State Reaction from Measurements of Enthalpy of Solution.
4.4 Bond Enthalpies.
Definition of Bond Enthalpies.
Calculation of Bond Enthalpies.
Enthalpy of Reaction from Bond Enthalpies.
4.5 Heat Capacity.
Definition.
Some Relationships between Cp and Cv.
Heat Capacities of Gases.
Heat Capacities of Solids.
Heat Capacities of Liquids.
Other Sources of Heat Capacity Data.
4.6 Enthalpy of Reaction as a Function of Temperature.
Analytic Method.
Arithmetic Method.
Graphical or Numerical Methods.
Exercises.
References.
5 A PPLICATIONS OF THE FIRST LAW TO GASES.
5.1 Ideal Gases.
Definition.
Enthalpy as a Function of Temperature Only.
Relationship Between Cp and Cv.
Calculation of the Thermodynamic Changes in Expansion Processes.
5.2 Real Gases.
Equations of State.
Joule–Thomson Effect.
Calculations of Thermodynamic Quantities in Reversible Expansions.
Exercises.
References.
6 THE SECOND LAW OF THERMODYNAMICS.
6.1 The Need for a Second Law.
6.2 The Nature of the Second Law.
Natural Tendencies Toward Equilibrium.
Statement of the Second Law.
Mathematical Counterpart of the Verbal Statement.
6.3 The Carnot Cycle.
The Forward Cycle.
The Reverse Cycle.
Alternative Statement of the Second Law.
Carnot’s Theorem.
6.4 The Thermodynamic Temperature Scale.
6.5 The Definition of S, the Entropy of a System.
6.6 The Proof that S is a Thermodynamic Property.
Any Substance in a Carnot Cycle.
Any Substance in Any Reversible Cycle.
Entropy S Depends Only on the State of the System.
6.7 Entropy Changes in Reversible Processes.
General Statement.
Isothermal Reversible Changes.
Adiabatic Reversible Changes.
Reversible Phase Transitions.
Isobaric Reversible Temperature Changes.
Isochoric Reversible Temperature Changes.
6.8 Entropy Changes in Irreversible Processes.
Irreversible Isothermal Expansion of an Ideal Gas.
Irreversible Adiabatic Expansion of an Ideal Gas.
Irreversible Flow of Heat from a Higher Temperature to a Lower Temperature.
Irreversible Phase Transitions.
Irreversible Chemical Reactions.
General Statement.
6.9 General Equations for the Entropy of Gases.
Entropy of the Ideal Gas.
Entropy of a Real Gas.
6.10 Temperature–Entropy Diagram.
6.11 Entropy as an Index of Exhaustion.
Exercises.
References.
7 EQUILIBRIUM AND SPONTANEITY FOR SYSTEMS AT CONSTANT TEMPERATURE.
7.1 Re versibility, Spontaneity, and Equilibrium.
Systems at Constant Temperature and Volume.
Systems at Constant Temperature and Pressure.
Heat of Reaction as an Approximate Criterion of Spontaneity.
7.2 Properties of the Gibbs, Helmholtz, and Planck Functions.
The Functions as Thermodynamic Properties.
Relationships among G, Y, and A.
Changes in the Functions for Isothermal Conditions.
Equations for Total Differentials.
Pressure and Temperature Derivatives of the Functions.
Equations Derived from the Reciprocity Relationship.
7.3 The Gibbs Function and Chemical Reactions.
Standard States.
7.4 Pressure and Temperature Dependence of ΔG.
7.5 Useful Work and the Gibbs and Helmholtz Functions.
Isothermal Changes.
Changes at Constant Temperature and Pressure.
Relationship between ΔHp and Qp When Useful Work is Performed.
Application to Electrical Work.
Gibbs–Helmholtz Equation.
The Gibbs Function and Useful Work in Biologic Systems.
Exercises.
References.
8 APPLICATION OF THE GIBBS FUNCTION AND THE PLANCK FUNCTION TO SOME PHASE CHANGES.
8.1 Two Phases at Equilibrium as a Function of Pressure and Temperature.
Clapeyron Equation.
Clausius–Clapeyron Equation.
8.2 The Effect of an Inert Gas on Vapor Pressure.
Variable Total Pressure at Constant Temperature.
Variable Temperature at Constant Total Pressure.
8.3 Temperature Dependence of Enthalpy of Phase Transition.
8.4 Calculation of Change in the Gibbs Function for Spontaneous Phase Change.
Arithmetic Method.
Analytic Method.
Exercises.
References.
9 THERMODYNAMICS OF SYSTEMS OF VARIABLE COMPOSITION.
9.1 State Functions for Systems of Variable Composition.
9.2 Criteria of Equilibrium and Spontaneity in Systems of Variable Composition.
9.3 Relationships Among Partial Molar Properties of a Single Component.
9.4 Relationships B