## Specifications

book-author | Stanley I. Sandler |
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publisher | Wiley; 5th edition |
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file-type | PDF |
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pages | 1032 pages |
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language | English |
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asin | B06XX2FN1R |
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isbn10 | 047050479X |
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isbn13 | 9780470504796/ 9781119343783 |
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## Book Description

In this newly revised** 5th Edition** of *Chemical and Engineering Thermodynamics (PDF); *Sandler presents a modern; applied approach to chemical thermodynamics and provides sufficient detail to develop a solid understanding of the key principles in the field. The ebook confronts current information on safety and environmental issues and how chemical engineering principles apply in biochemical engineering; biotechnology; polymers; and solid-state-processing. This ebook is appropriate for the graduate and undergraduate level courses.

**NOTE: Only includes ***Chemical; Biochemical; and Engineering Thermodynamics; 5e* in PDF. No access codes included.

## Table of contents

Table of contents :

Machine generated contents note: Instructional Objectives for Chapter 1 —

Important Notation Introduced in This Chapter —

1.1. The Central Problems of Thermodynamics —

1.2.A System of Units —

1.3. The Equilibrium State —

1.4. Pressure, Temperature, and Equilibrium —

1.5. Heat, Work, and the Conservation of Energy —

1.6. Specification of the Equilibrium State

Intensive and Extensive Variables

Equations of State —

1.7.A Summary of Important Experimental Observations —

1.8.A Comment on the Development of Thermodynamics —

Problems —

Instructional Objectives for Chapter 2 —

Important Notation Introduced in This Chapter —

2.1.A General Balance Equation and Conserved Quantities —

2.2. Conservation of Mass for a Pure Fluid —

2.3. The Mass Balance Equations for a Multicomponent System with a Chemical Reaction —

2.4. The Microscopic Mass Balance Equations in Thermodynamics and Fluid Mechanics (Optional —

only on the website for this book) —

Problems. Note continued: Instructional Objectives for Chapter 3 —

Notation Introduced in This Chapter —

3.1. Conservation of Energy —

3.2. Several Examples of Using the Energy Balance —

3.3. The Thermodynamic Properties of Matter —

3.4. Applications of the Mass and Energy Balances —

3.5. Conservation of Momentum —

3.6. The Microscopic Energy Balance (Optional —

only on website for this book) —

Problems —

Instructional Objectives for Chapter 4 —

Notation Introduced in This Chapter —

4.1. Entropy: A New Concept —

4.2. The Entropy Balance and Reversibility —

4.3. Heat, Work, Engines, and Entropy —

4.4. Entropy Changes of Matter —

4.5. Applications of the Entropy Balance —

4.6. Availability and the Maximum Useful Shaft Work that can be obtained In a Change of State —

4.7. The Microscopic Entropy Balance (Optional —

only on website for this book) —

Problems —

Instructional Objectives for Chapter 5 —

Notation Introduced in this Chapter —

5.1. Liquefaction. Note continued: 5.2. Power Generation and Refrigeration Cycles —

5.3. Thermodynamic Efficiencies —

5.4. The Thermodynamics of Mechanical Explosions —

Problems —

Instructional Objectives for Chapter 6 —

Notation Introduced in this Chapter —

6.1. Some Mathematical Preliminaries —

6.2. The Evaluation of Thermodynamic Partial Derivatives —

6.3. The Ideal Gas and Absolute Temperature Scales —

6.4. The Evaluation of Changes in the Thermodynamic Properties of Real Substances Accompanying a Change of State —

6.5. An Example Involving the Change of State of a Real Gas —

6.6. The Principle of Corresponding States —

6.7. Generalized Equations of State —

6.8. The Third Law of Thermodynamics —

6.9. Estimation Methods for Critical and Other Properties —

6.10. Sonic Velocity —

6.11. More About Thermodynamic Partial Derivatives (Optional —

only on website for this book) —

Problems —

Instructional Objectives for Chapter 7 —

Notation Introduced in This Chapter. Note continued: 7.1. The Criteria for Equilibrium —

7.2. Stability of Thermodynamic Systems —

7.3. Phase Equilibria: Application of the Equilibrium and Stability Criteria to the Equation of State —

7.4. The Molar Gibbs Energy and Fugacity of a Pure Component —

7.5. The Calculation of Pure Fluid-Phase Equilibrium: The Computation of Vapor Pressure from an Equation of State —

7.6. Specification of the Equilibrium Thermodynamic State of a System of Several Phases: The Gibbs Phase Rule for a One-Component System —

7.7. Thermodynamic Properties of Phase Transitions —

7.8. Thermodynamic Properties of Small Systems, or Why Subcooling and Superheating Occur —

Problems —

Instructional Objectives for Chapter 8 —

Notation Introduced in This Chapter —

8.1. The Thermodynamic Description of Mixtures —

8.2. The Partial Molar Gibbs Energy and the Generalized Gibbs-Duhem Equation —

8.3.A Notation for Chemical Reactions —

8.4. The Equations of Change for a Multicomponent System. Note continued: 8.5. The Heat of Reaction and a Convention for the Thermodynamic Properties of Reacting Mixtures —

8.6. The Experimental Determination of the Partial Molar Volume and Enthalpy —

8.7. Criteria for Phase Equilibrium in Multicomponent Systems —

8.8. Criteria for Chemical Equilibrium, and Combined Chemical and Phase Equilibrium —

8.9. Specification of the Equilibrium Thermodynamic State of a Multicomponent, Multiphase System

the Gibbs Phase Rule —

8.10.A Concluding Remark —

Problems —

Instructional Objectives for Chapter 9 —

Notation Introduced in This Chapter —

9.1. The Ideal Gas Mixture —

9.2. The Partial Molar Gibbs Energy and Fugacity —

9.3. Ideal Mixture and Excess Mixture Properties —

9.4. Fugacity of Species in Gaseous, Liquid, and Solid Mixtures —

9.5. Several Correlative Liquid Mixture Activity Coefficient Models —

9.6. Two Predictive Activity Coefficient Models —

9.7. Fugacity of Species in Nonsimple Mixtures. Note continued: 9.8. Some Comments on Reference and Standard States —

9.9.Combined Equation-of-State and Excess Gibbs Energy Model —

9.10. Electrolyte Solutions —

9.11. Choosing the Appropriate Thermodynamic Model —

Appendix A9.1 A Statistical Mechanical Interpretation of the Entropy of Mixing in an Ideal Mixture (Optional —

only on the website for this book) —

Appendix A9.2 Multicomponent Excess Gibbs Energy (Activity Coefficient) Models —

Appendix A9.3 The Activity Coefficient of a Solvent in an Electrolyte Solution —

Problems —

Instructional Objectives for Chapter 10 —

Notation Introduced in This Chapter —

10.0. Introduction to Vapor-Liquid Equilibrium —

10.1. Vapor-Liquid Equilibrium in Ideal Mixtures —

Problems for Section 10.1 —

10.2. Low-Pressure Vapor-Liquid Equilibrium in Nonideal Mixtures —

Problems for Section 10.2 —

10.3. High-Pressure Vapor-Liquid Equilibria Using Equations of State (0-0 Method) —

Problems for Section 10.3. Note continued: Instructional Objectives for Chapter 11 —

Notation Introduced in This Chapter —

11.1. The Solubility of a Gas in a Liquid —

Problems for Section 11.1 —

11.2. Liquid-Liquid Equilibrium —

Problems for Section 11.2 —

11.3. Vapor-Liquid-Liquid Equilibrium —

Problems for Section 11.3 —

11.4. The Partitioning of a Solute Among Two Coexisting Liquid Phases

The Distribution Coefficient —

Problems for Section 11.4 —

11.5. Osmotic Equilibrium and Osmotic Pressure —

Problems for Section 11.5 —

Instructional Objectives for Chapter 12 —

Notation Introduced in This Chapter —

12.1. The Solubility of a Solid in a Liquid, Gas, or Supercritical Fluid —

Problems for Section 12.1 —

12.2. Partitioning of a Solid Solute Between Two Liquid Phases —

Problems for Section 12.2 —

12.3. Freezing-Point Depression of a Solvent Due to the Presence of a Solute

the Freezing Point of Liquid Mixtures —

Problems for Section 12.3 —

12.4. Phase Behavior of Solid Mixtures. Note continued: Problems for Section 12.4 —

12.5. The Phase Behavior Modeling of Chemicals in the Environment —

Problems for Section 12.5 —

12.6. Process Design and Product Design —

Problems for Section 12.6 —

12.7. Concluding Remarks on Phase Equilibria —

Instructional Objectives for Chapter 13 —

Important Notation Introduced in This Chapter —

13.1. Chemical Equilibrium in a Single-Phase System —

13.2. Heterogeneous Chemical Reactions —

13.3. Chemical Equilibrium When Several Reactions Occur in a Single Phase —

13.4.Combined Chemical and Phase Equilibrium —

13.5. Ionization and the Acidity of Solutions —

13.6. Ionization of Biochemicals —

13.7. Partitioning of Amino Acids and Proteins Between Two Liquids —

Problems —

Instructional Objectives for Chapter 14 —

Notation Introduced in This Chapter —

14.1. The Balance Equations for a Tank-Type Chemical Reactor —

14.2. The Balance Equations for a Tubular Reactor. Note continued: 14.3. Overall Reactor Balance Equations and the Adiabatic Reaction Temperature —

14.4. Thermodynamics of Chemical Explosions —

14.5. Maximum Useful Work and Availability in Chemically Reacting Systems —

14.6. Introduction to Electrochemical Processes —

14.7. Fuel Cells and Batteries —

Problems —

Instructional Objectives for Chapter 15 —

Notation Introduced in This Chapter —

15.1. Solubilities of Weak Acids, Weak Bases, and Amino Acids as a Function of pH —

15.2. The Solubility of Amino Acids and Proteins as a function of Ionic Strength and Temperature —

15.3. Binding of a Ligand to a Substrate —

15.4. Some Other Examples of Biochemical Reactions —

15.5. The Denaturation of Proteins —

15.6. Coupled Biochemical Reactions: The ATP-ADP Energy Storage and Delivery Mechanism —

15.7. Thermodynamic Analysis of Fermenters and Other Bioreactors —

15.8. Gibbs-Donnan Equilibrium and Membrane Potentials —

15.9. Protein Concentration in an Ultracentrifuge. Note continued: Problems —

Appendix A.I Conversion Factors For Si Units —

Appendix A. II The Molar Heat Capacities Of Gases In The Ideal Gas (Zero Pressure) State —

Appendix A. III The Thermodynamic Properties Of Water And Steam —

Appendix A. IV Enthalpies And Free Energies Of Formation —

Appendix A.V Heats Of Combustion —

Appendix B.I Windows-Based Visual Basic Programs —

Appendix B. II Dos-Based Basic Programs —

Appendix B. III Mathcad Worksheets —

Appendix B. IV Matlab Programs.