Engineering and Chemical Thermodynamics

Table of Contents

1.1 Thermodynamic properties and other basic concepts

1.2 Measured thermodynamic properties

1.3 Equilibrium

1.4 States and phases

1.5 Thermodynamic property tables

1.6 Summary

1.7 Problems

2.1 First law of thermodynamics

2.2 Processes and paths

2.3 First law of thermodynamics for closed systems

2.4 First law of thermodynamics for open systems

2.5 Thermochemical data for \(U\) and \(H\)

2.6 Reversible processes in closed systems

2.7 Open system energy balances on process equipment

2.8 Summary

2.9 Problems

2.10 Problems (continued)

2.11 Problems (continued)

2.12 Problems (continued)

2.13 Problems (continued)

2.14 Problems (continued)

3.1 Directionality of processes/spontaneity

3.2 Reversible and irreversible processes and their relationship to directionality

3.3 Entropy, the thermodynamic property

3.4 The second law of thermodynamics

3.5 Molecular view of entropy

3.6 The second law of thermodynamics for closed and open systems

3.7 Calculation of \(s\) for an ideal gas

3.8 The mechanical energy balance and the Bernoulli equation

3.9 Vapor-compression power and refrigeration cycles

3.10 Exergy (availability) analysis

3.11 Summary

3.12 Problems

3.13 Problems (continued)

3.14 Problems (continued)

3.15 Problems (continued)

3.16 Problems (continued)

3.17 Problems (continued)

4.1 Equations of State

4.2 Intermolecular interactions

4.3 Potential functions and chemical effects

4.4 Cubic equations of state

4.5 Virial equation of state

4.6 Equations of state for liquids and solids

4.7 Generalized compressibility charts

4.8 Mixing rules

4.9 Summary

4.10 Problems

4.11 Problems (continued)

4.12 Problems (continued)

5.1 Types of thermodynamic properties

5.2 Thermodynamic property relations

5.3 Calculation of fundamental and derived properties using equations of state and other measured properties

5.4 Departure functions

5.5 Joule-Thompson Expansion and Liquefaction

5.6 Summary

5.7 Problems

5.8 Problems (continued)

5.9 Problems (continued)

5.10 Problems (continued)

5.11 Problems (continued)

6.1 The phase equilibria problem

6.2 Pure species phase equilibrium: Gibbs Energy

6.3 Pure species phase equilibrium: Relations between P and T

6.4 Thermodynamics of mixing

6.5 Partial molar properties

6.6 The chemical potential

6.7 Summary

6.8 Problems

6.9 Problems (continued)

6.10 Problems (continued)

6.11 Problems (continued)

7.1 Introducing fugacity

7.2 Fugacity in the vapor phase: Pure species

7.3 Fugacity in the vapor phase: Mixtures

7.4 Fugacity in the liquid phase: Reference states and activity coefficients

7.5 Introducing models for \(g^E\): the two-suffix Margules equation

7.6 Models for \(g^E\): Binary mixtures

7.7 Temperature and pressure dependence of \(g^E\)

7.8 Models for \(g^E\): Multicomponent mixtures

7.9 Summary

7.10 Problems

7.11 Problems (continued)

7.12 Problems (continued)

7.13 Problems (continued)

7.14 Problems (continued)

8.1 Vapor-liquid equilibrium (VLE): Concepts and phase diagrams

8.2 VLE: Bubble point, dew point and the lever rule

8.3 VLE: Solubility of gases in liquids

8.4 VLE: Fitting models for \(g^E\) with VLE data

8.5 VLE: Equation of state method

8.6 LLE: Liquid-liquid equilibrium

8.7 VLLE: Vapor-liquid-liquid equilibrium

8.8 SLE and SSE: Solid-liquid and solid-solid equilibrium

8.9 Colligative Properties

8.10 Summary

8.11 Problems

8.12 Problems (continued)

8.13 Problems (continued)

8.14 Problems (continued)

8.15 Problems (continued)

8.16 Problems (continued)

9.1 Chemical reactions: Kinetics and thermodynamics

9.2 Equilibrium constant formulation

9.3 Using thermochemical data to calculate \(K\)

9.4 Chemical equilibrium for a single reaction

9.5 Multiple chemical reactions

9.6 Equilibrium in electrochemical processes

9.7 Reaction equilibria of point defects in crystalline solids

9.8 Summary

9.9 Problems

9.10 Problems (continued)

9.11 Problems (continued)

9.12 Problems (continued)

9.13 Problems (continued)

10.1 Physical constants, conversion factors, and nomenclature

10.2 Periodic Table of the Elements

11.1 Critical constants, acentric factors, and antoine coefficients

11.2 Heat capacity data

11.3 Enthalpy and Gibbs Energy of Formation at 298 K and 1 bar

12.1 Symbols used in the steam tables

12.2 Saturated water: temperature table

12.3 Saturated water: pressure table

12.4 Saturated water: solid-vapor

12.5 Superheated water vapor

12.6 Subcooled liquid water

13.1 Values for \(z^{(0)}\)

13.2 Values for \(z^{(1)}\)

13.3 Values for \(\left[\frac{h_{T_{r}, P_{r}}-h_{T_{r}, P_{r}}^{\text {ideal gas }}}{R T_{c}}\right]^{(0)}\)

13.4 Values for \(\left[\frac{h_{T_{r}, P_{r}}-h_{T_{r}, P_{r}}^{\text {ideal gas }}}{R T_{c}}\right]^{(1)}\)

13.5 Values for \(\left[\frac{s_{T_{r}, P_{r}}-s_{T_{r}, P_{r}}^{\text {ideal gas }}}{R}\right]^{(0)}\)

13.6 Values for \(\left[\frac{s_{T_{r}, P_{r}}-s_{T_{r}, P_{r}}^{\text {ideal gas }}}{R}\right]^{(1)}\)

13.7 Values for log \(\left [ \Phi ^{(0)} \right ]\)

13.8 Values for log \(\left [ \Phi ^{(1)} \right ]\)

14.1 Common variables used in thermodynamics and their associated units

14.2 Conversion between CGS (gaussian) units and SI units

15.1 Software Description

15.2 Corresponding States Using The Lee–Kesler Equation of State

Same Text, More Action

Based on the original textbook, Engineering and Chemical Thermodynamics helps students understand and visualize thermodynamics through a qualitative discussion of the role of molecular interactions and a highly visual presentation of the material. In this zyVersion you’ll find:

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Milo D. Koretsky
Professor of Chemical and Biological Engineering, Professor of Education, McDonnell Family Bridge Professorship, Tufts University

Matthew Liberatore
Professor of Chemical Engineering, University of Toledo


Nikitha Sambamurthy
Editorial Director / zyBooks