Introductory chemical engineering thermodynamics

Başlık:

Yazar:

Elliott, J. Richard.

ISBN:

9780130113863

Ek Yazar:

Elliott, J. Richard.

Yayım Bilgisi:

Upper Saddle River, NJ : Prentice Hall PTR, 1999.

Fiziksel Tanım:

xxi, 660 s : res. ; 27 cm.

Series:

Prentice-Hall international series in the physical and chemical engineering sciences

Prentice-Hall international series in the physical and chemical engineering sciences.

Contents:

First and Second Laws -- The Molecular Nature of Energy -- Intermolecular potentials for mixtures -- The Molecular Nature of Entropy -- Brief Summary of Several Thermodynamic Quantities -- Basic Concepts -- Introduction to steam tables -- Interpolation -- Double interpolation -- Double interpolation using different tables -- Double interpolation using Excel -- Quality calculations -- Constant volume cooling -- The Energy Balance -- Expansion/Contraction Work -- Shaft Work -- Work Associated With Flow -- Lost Work vs. Reversibility -- Isothermal compression of an ideal gas -- Path Properties and State Properties -- Work as a path function -- Heat Flow -- The Closed-System Energy Balance -- Internal energy and heat -- The Open-System, Steady-State Balance -- The Complete Energy Balance -- Internal Energy, Enthalpy, and Heat Capacities -- Enthalpy of H[subscript 2]O above its saturation pressure -- Adiabatic compression of an ideal gas in a piston/cylinder -- Transformation of kinetic energy into enthalpy -- Kinetic and Potential Energy -- On the relative magnitude of kinetic, potential, internal energy and enthalpy changes -- Energy Balances for Process Equipment -- The integral representing shaft work -- Strategies for Solving Process Thermodynamics Problems -- Closed and Steady-State Open Systems -- Adiabatic, reversible expansion of an ideal gas -- Continuous adiabatic, reversible compression of an ideal gas -- Continuous, isothermal, reversible compression of an ideal gas -- Heat loss from a turbine.

Abstract:

"Introductory Chemical Engineering Thermodynamics will help students master the fundamentals of applied thermodynamics as practiced today, with a molecular perspective and step-by-step guidelines for process simulation." "Introductory Chemical Engineering Thermodynamics presents extensive practical examples, especially in its coverage of non-ideal mixtures which addresses water contamination via hydrocarbons, polymer blending/recycling, oxygenated fuels, and other contemporary issues."--Jacket.

Konu Terimleri:

Thermodynamics.

Termodinamik

Chemical engineering.

Kimya Mühendisliği

Added Author:

Lira, Carl T.

Mevcut:*

Library	Materyal Türü	Barkod	Yer Numarası	Durum
Searching... Pamukkale Merkez Kütüphanesi	Kitap	0086019	TP 149 .E45 1999	Searching... Unknown

Bound With These Titles

On Order

Özet

The four units of this textbook address first and second laws, generalized analysis of fluid properties, fluid phase equilibria in mixtures, and reacting systems. Appendices summarize models for process simulators, and computer programs for calculators, spreadsheets and Fortran. DEGREES DEGREES DEGR

Author Notes

J. Richard Elliott is Associate Professor of Chemical Engineering at the University of Akron in Akron, OH
Carl T. Lira is Associate Professor in the Department of Chemical Engineering at Michigan State University

Alıntılar

Preface "No happy phrase of ours is ever quite original with us; there is nothing of our own in it except some slight change born of our temperament, character, environment, teachings and associations." -- Mark Twain Thank you for your interest in our book. We have developed this book to address ongoing evolutions in applied thermodynamics and computer technology. Molecular perspective is becoming more important in the refinement of thermodynamic models for fluid properties and phase behavior. Molecular simulation is increasingly used for exploring and improving fluid models. While many of these techniques are still outside the scope of this text, these new technologies will be important to practicing engineers in the near future, and an introduction to the molecular perspective is important for this reason. We expect our text to continue to evolve with the chemical engineering field. Computer technology has made process simulators commonplace in most undergraduate curriculums and professional work environments. This increase in computational flexibility has moved many of the process calculations from mainframe computers and thermodynamic property experts to the desktop and practicing engineers and students. This increase in computational ability also increases the responsibility of the individuals developing process simulations to choose meaningful models for the components in the system because most simulators provide even more options for thermodynamic models than we can cover in this text. We have included background and comparison on many of the popular thermodynamic models to address this issue. Computational advances are also affecting education. Thus we have significant usage of equations of state throughout the text. We find these computational tools remove much of the drudgery of repetitive calculations, which permits more class time to be spent on the development of theories, molecular perspective, and comparisons of alternative models. We have included FORTRAN, Excel spreadsheets, TI85, and HP48 calculator programs to complement the text. The programs are summarized in the appendices. Solutions to cubic equations of state are no longer tedious with the handheld calculators available today for about $100. We provide programs for calculation of thermodynamic properties via the Peng-Robinson equation, vapor pressure programs, Peng-Robinson K-ratios and bubble pressures of mixtures, and van Laar and UNIFAC activity coefficients as well as several other utility programs. Our choice of the HP48 calculator is due to its being one of the first to provide a computer interface for downloading programs from a PC and provide calculator-to-calculator communication, which facilitates distribution of the programs. If all students in the class have access to these engineering calculators, as practiced at the University of Akron, questions on exams can be designed to apply to these programs directly. This obviates the need for traditional methods of reading charts for departure functions and K-ratios and enables treatment of modern methods like equations of state and UNIFAC. Spreadsheets have also improved to the point that they are powerful tools for solving engineering problems. We have chosen to develop spreadsheets for Microsoft® Excel because of the widespread availability. Certainly Mathcad®, Mathematica®, and other software could be used, but none has the widespread availability of spreadsheets. We have found the solver within Excel to provide a good tool for solving a wide variety of problems. We provide spreadsheets for thermodynamic properties, phase and reaction equilibria. High-level programming is still necessary for more advanced topics. For these applications, we provide compiled programs for thermodynamic properties and phase behavior. For an associating system, such as an alcohol, we provide the ESD equation of state. These programs are menu-driven and do not require knowledge of a computer language. In a limited number of instances, we provide FORTRAN source code. We provide FORTRAN code because of our own abilities to program faster in FORTRAN, although other languages are finding increasing popularity in the engineering community. We have tried to avoid customization of the code for a specific FORTRAN compiler, which improves portability to other operating platforms but also limits the "bells and whistles" that a specific interface could provide. These programs provide a framework for students and practicing engineers to customize for their own applications. Energy and entropy balances are at the heart of process engineering calculations. We develop these approaches first using the ideal gas law or thermodynamic tables, then revisit the topics after developing equation-of-state techniques for thermodynamic properties. We are well aware of the concern that students often apply the ideal gas law inappropriately. Therefore we clearly mark equations using the ideal gas law or assuming a temperature-independent heat capacity. From a pedagogical standpoint, we are faced with the issues of developing first and second law balances, equations of state (and their departure functions) for fluid properties, and then combining the principles. We have found it best that students quickly develop ability and confidence in application of the balances with simple calculational procedures before introducing the equation of state. The balance concepts are typically more easily grasped and are essential for extension to later courses in the curriculum. Another benefit of this approach is that the later development of the equation of state can be directly followed by departure functions, and the reasons for needing properties such as enthalpy and entropy are well understood from the earlier emphasis on the balances. This enables students to focus on the development of the departure functions without being distracted by not completely understanding how these properties will be used. Fugacity is another property which is difficult to understand. We have tried to focus on the need for a property which is a natural function of T and P, and also stress how it is related to departure functions. There are many ways to calculate fugacities (which provides many trees to block the view of the forest), and we have tried to provide tables and diagrams to show the inter-relations between fugacity coefficients, activity coefficients, ideal gases, ideal solutions, and real solutions. A distinct feature of this text is its emphasis on molecular physics at the introductory level. Our perspective is that this background must be made available to students in an integrated manner, but it is up to instructors to decide the level of emphasis for the entire spectrum of their students. We have organized this material such that it may be covered as a supplementary reading assignment or as a homework and test assignment. With the latter emphasis, it is possible to formulate a graduate course based on this text. Throughout the text, we have used text boxes to highlight important statements and equations. Boxed equations are not always final results of derivations. In some cases, the boxes highlight mathematical definitions of important intermediate results that might be useful for homework problems. We consider the examples to be an integral part of the text, and we use them to illustrate important points. In some cases, derivations and important equations are within an example because the equations are model-specific (e.g., ideal gas). Examples are often cross-referenced and are therefore listed in the table of contents. There are many marginal notes throughout the text. Where you find an EXCLAMATION POINT icon, it means that an important point is made, or a useful equation has been introduced. Where you find an HP or TI icon, it means that a calculator program is available to assist in calculations. The calculator programs are sometimes not necessary, but extremely helpful. Where you find a DISK icon, it means that an Excel spreadsheet or a compiled program is available. In some cases, the program is simply convenient, but typically you will find that these calculations are tedious without the program. For calculator or PC icons, the program names are given by the icons. See the computer appendix or the readme files for specific program instructions. We periodically update computer software and the computer appendix. The latest software is available from our website http://www.egr.msu.edu/~lira/thermtxt.htm. We hope you find our approaches helpful in your learning and educational endeavors. We welcome your suggestions for further improvements and enhancements. You may contact us easily at the email addresses below. Unfortunately, we will be unable to personally respond to all comments, although we will try. Notes to Students Computer programs facilitate the solution to homework problems, but should not be used to replace an understanding of the material. Always understand exactly which formulas are required before turning to the computer. Before using the computer, we recommend that you know how to solve the problem by hand calculations. If you do not understand the formulas in the spreadsheets it is a good indication that you need to do more studying before using the program so that the structure of the spreadsheet will make sense. When you understand the procedures, it should be obvious which spreadsheet cells will help you to the answer, and which cells are intermediate calculations. It is also helpful to rework example problems from the text using the software. Acknowledgments We would like to thank the many people who helped this work find its way to the classroom. We express appreciation to Professors Joan Brennecke, Mike Matthews, Bruce Poling, Ross Taylor, and Mark Thies, who worked with early versions of the text and provided suggestions for improve-ment. We are also greatly indebted to Dave Hart for proofreading an early version. There are many students who suffered through error-prone preliminary versions, and we thank them all for their patience and vision of the common goal of an error-free book. CTL would like to thank Ryoko Yamasaki for her work in typing many parts of the manuscript and problem solutions. CTL also thanks family members Gail, Nicolas, and Adrienne for their patience while the text was prepared, as many family sacrifices helped make this book possible. JRE thanks family members Guliz, Serra, and Eileen for their similar forbearance. We acknowledge Dan Friend and NIST, Boulder for contributions to the steam tables and thermodynamic charts. Lastly, we acknowledge the influences of the many authors of previous thermodynamics texts. We hope we have done justice to this distinguished tradition, while simultaneously bringing deeper insight to a broader audience. Carl T. Lira , Michigan State University, lira@egr.msu.edu J. Richard Elliott , University of Akron, Excerpted from Introductory Chemical Engineering Thermodynamics by J. Richard Elliott, Carl T. Lira All rights reserved by the original copyright owners. Excerpts are provided for display purposes only and may not be reproduced, reprinted or distributed without the written permission of the publisher.

Preface	p. xv
Notation	p. xix
Unit I First and Second Laws	p. 1
Chapter 1 Introduction	p. 3
1.1 The Molecular Nature of Energy	p. 5
Example 1.1 Intermolecular potentials for mixtures	p. 10
1.2 The Molecular Nature of Entropy	p. 10
1.3 Brief Summary of Several Thermodynamic Quantities	p. 11
1.4 Basic Concepts	p. 15
Example 1.2 Introduction to steam tables	p. 22
Example 1.3 Interpolation	p. 23
Example 1.4 Double interpolation	p. 24
Example 1.5 Double interpolation using different tables	p. 25
Example 1.6 Double interpolation using Excel	p. 26
Example 1.7 Quality calculations	p. 28
Example 1.8 Constant volume cooling	p. 29
1.5 Summary	p. 30
1.6 Homework Problems	p. 31
Chapter 2 The Energy Balance	p. 35
2.1 Expansion/Contraction Work	p. 35
2.2 Shaft Work	p. 36
2.3 Work Associated With Flow	p. 37
2.4 Lost Work vs. Reversibility	p. 38
Example 2.1 Isothermal compression of an ideal gas	p. 41
2.5 Path Properties and State Properties	p. 41
Example 2.2 Work as a path function	p. 42
2.6 Heat Flow	p. 43
2.7 The Closed-System Energy Balance	p. 43
Example 2.3 Internal energy and heat	p. 45
2.8 The Open-System, Steady-State Balance	p. 47
2.9 The Complete Energy Balance	p. 49
2.10 Internal Energy, Enthalpy, and Heat Capacities	p. 51
Example 2.4 Enthalpy of H[subscript 2]O above its saturation pressure	p. 53
Example 2.5 Adiabatic compression of an ideal gas in a piston/cylinder	p. 56
Example 2.6 Transformation of kinetic energy into enthalpy	p. 57
2.11 Kinetic and Potential Energy	p. 58
Example 2.7 On the relative magnitude of kinetic, potential, internal energy and enthalpy changes	p. 58
2.12 Energy Balances for Process Equipment	p. 59
Example 2.8 The integral representing shaft work	p. 64
2.13 Strategies for Solving Process Thermodynamics Problems	p. 65
2.14 Closed and Steady-State Open Systems	p. 66
Example 2.9 Adiabatic, reversible expansion of an ideal gas	p. 66
Example 2.10 Continuous adiabatic, reversible compression of an ideal gas	p. 68
Example 2.11 Continuous, isothermal, reversible compression of an ideal gas	p. 69
Example 2.12 Heat loss from a turbine	p. 70
2.15 Unsteady-State Open Systems (Optional)	p. 72
Example 2.13 Adiabatic expansion of an ideal gas from a leaky tank	p. 72
Example 2.14 Adiabatically filling a tank with an ideal gas	p. 73
Example 2.15 Adiabatic expansion of steam from a leaky tank	p. 74
2.16 Details of Terms in the Energy Balance (Optional)	p. 75
2.17 Summary	p. 77
2.18 Practice Problems	p. 77
2.19 Homework Problems	p. 80
Chapter 3 Entropy	p. 87
3.1 The Concept of Entropy	p. 87
3.2 Microscopic View of Entropy	p. 89
Example 3.1 Entropy change vs. volume change	p. 93
Example 3.2 Entropy change of mixing ideal gases	p. 94
3.3 The Macroscopic Definition of Entropy	p. 96
Example 3.3 Ideal gas entropy changes in a piston/cylinder	p. 100
Example 3.4 Steam entropy changes in a piston/cylinder	p. 102
Example 3.5 Entropy generation in a temperature gradient	p. 102
Example 3.6 Entropy generation and lost work in a gas expansion	p. 103
3.4 The Entropy Balance	p. 104
Example 3.7 Steady-state entropy generation	p. 105
Example 3.8 Reversible work between heat reservoirs, lost work	p. 107
Example 3.9 Entropy change of quenching	p. 109
3.5 The Carnot Engine	p. 110
3.6 Carnot Heat Pump	p. 112
3.7 Internal Reversibility	p. 113
3.8 Maximum/Minimum Work in Real Process Equipment	p. 114
3.9 Entropy Balance For Process Equipment	p. 116
3.10 Charts Including Entropy	p. 117
3.11 Turbine Calculations	p. 119
Example 3.10 Turbine efficiency	p. 120
3.12 Multistage Turbines	p. 121
3.13 Pumps and Compressors	p. 122
3.14 Strategies for Applying the Entropy Balance	p. 123
3.15 Additional Steady-State Examples	p. 124
Example 3.11 Heat pump analysis	p. 124
Example 3.12 Entropy in a heat exchanger	p. 125
3.16 Unsteady-State Open Systems (Optional)	p. 127
Example 3.13 Entropy change in a leaky tank	p. 127
Example 3.14 An ideal gas leaking through a turbine (unsteady-state)	p. 128
3.17 The Entropy Balance in Brief	p. 129
3.18 Summary	p. 129
3.19 Practice Problems	p. 130
3.20 Homework Problems	p. 131
Chapter 4 Thermodynamics of Processes	p. 141
4.1 The Carnot Cycle	p. 141
4.2 The Rankine Cycle	p. 143
Example 4.1 Rankine cycle	p. 144
Example 4.2 Two-phase turbine output	p. 145
4.3 Rankine Modifications	p. 146
Example 4.3 Rankine with reheat	p. 146
Example 4.4 Regenerative Rankine cycle	p. 148
4.4 Refrigeration	p. 149
Example 4.5 Refrigeration by vapor-compression cycle	p. 151
4.5 Liquefaction	p. 154
Example 4.6 Liquefaction of methane by the Linde process	p. 155
4.6 Internal Combustion Engines	p. 156
Example 4.7 Air-standard Brayton cycle thermal efficiency	p. 157
Example 4.8 Thermal efficiency of the Otto engine	p. 158
Example 4.9 Thermal efficiency of a Diesel engine	p. 160
4.7 Fluid Flow	p. 161
4.8 Problem-Solving Strategies	p. 164
4.9 Practice Problems	p. 165
4.10 Homework Problems	p. 165
Unit II Generalized Analysis of Fluid Properties	p. 171
Chapter 5 Classical Thermodynamics--Generalization to Any Fluid	p. 173
5.1 The Fundamental Property Relation	p. 174
5.2 Derivative Relations	p. 180
Example 5.1 Pressure dependence of H	p. 176
Example 5.2 Entropy change with respect to T at constant P	p. 181
Example 5.3 Entropy as a function of T and P	p. 182
Example 5.4 Entropy change for an ideal gas	p. 183
Example 5.5 Entropy change for a simple non-ideal gas	p. 183
Example 5.6 Application of the triple product relation	p. 184
Example 5.7 TCH for an ideal gas	p. 184
Example 5.8 Volumetric dependence of C[subscript V] for ideal gas	p. 185
Example 5.9 Master equation for an ideal gas	p. 185
Example 5.10 Relating C[subscript P] to C[subscript V]	p. 186
5.3 Advanced Topics (Optional)	p. 186
5.4 Summary	p. 189
5.5 Homework Problems	p. 190
Chapter 6 Engineering Equations of State for PVT Properties	p. 193
6.1 Experimental Measurements	p. 194
6.2 Three-Parameter Corresponding States	p. 195
6.3 Generalized Compressibility Factor Charts	p. 198
Example 6.1 Application of the generalized charts	p. 198
6.4 The Virial Equation of State	p. 200
Example 6.2 Application of the virial equation	p. 201
6.5 Cubic Equations of State	p. 202
6.6 Solving the Equation of State for Z	p. 205
Example 6.3 Solution of the Peng-Robinson equation for molar volume	p. 207
Example 6.4 Application of the Peng-Robinson equation	p. 208
6.7 Implications of Real Fluid Behavior	p. 210
Example 6.5 Derivatives of the Peng-Robinson equation	p. 210
6.8 The Molecular Theory Behind Equations of State	p. 210
Example 6.6 Deriving your own equation of state	p. 217
6.9 Matching the Critical Point	p. 220
Example 6.7 Critical parameters for the van der Waals equation	p. 220
6.10 Summary and Concluding Remarks	p. 220
6.11 Practice Problems	p. 221
6.12 Homework Problems	p. 222
Chapter 7 Departure Functions	p. 229
7.1 The Departure Function Pathway	p. 230
7.2 Internal Energy Departure Function	p. 231
7.3 Entropy Departure Function	p. 234
7.4 Other Departure Functions	p. 234
7.5 Summary of Density-Dependent Formulas	p. 235
Example 7.1 Enthalpy and entropy departures from the Peng-Robinson equation	p. 236
Example 7.2 Real entropy in an engine	p. 238
Example 7.3 Enthalpy departure for the Peng-Robinson equation	p. 240
Example 7.4 Gibbs departure for the Peng-Robinson equation	p. 241
7.6 Pressure-Dependent Formulas	p. 241
Example 7.5 Application of pressure-dependent formulas in compression of methane	p. 242
7.7 Reference States	p. 243
Example 7.6 Enthalpy and entropy from the Peng-Robinson equation	p. 245
Example 7.7 Liquefaction revisited	p. 245
Example 7.8 Adiabatically filling a tank with propane (optional)	p. 247
7.8 Generalized Charts for the Enthalpy Departure	p. 247
7.9 Summary	p. 247
7.10 Practice Problems	p. 249
7.11 Homework Problems	p. 250
Chapter 8 Phase Equilibrium in a Pure Fluid	p. 257
8.1 Criteria for Equilibrium	p. 258
8.2 The Clausius-Clapeyron Equation	p. 258
Example 8.1 Clausius-Clapeyron equation near or below the boiling point	p. 260
8.3 Shortcut Estimation of Saturation Properties	p. 260
Example 8.2 Vapor pressure interpolation	p. 261
Example 8.3 Application of the shortcut vapor pressure equation	p. 262
Example 8.4 General application of the Clapeyron equation	p. 263
8.4 Changes in Gibbs Energy With Pressure	p. 264
8.5 Fugacity and Fugacity Coefficient	p. 266
8.6 Fugacity Criteria for Phase Equilibria	p. 368
8.7 Calculation of Fugacity (Gases)	p. 268
8.8 Calculation of Fugacity (Liquids)	p. 271
8.9 Calculation of Fugacity (Solids)	p. 273
8.10 Saturation Conditions from an Equation of State	p. 274
Example 8.5 Vapor pressure from the Peng-Robinson equation	p. 274
Example 8.6 Acentric factor for the van der Waals equation	p. 275
8.11 Summary	p. 277
8.12 Temperature Effects on G and f (Optional)	p. 278
8.13 Practice Problems	p. 278
8.14 Homework Problems	p. 279
Unit III Fluid Phase Equilibria in Mixtures	p. 283
Chapter 9 Introduction to Multicomponent Systems	p. 285
9.1 Phase Diagrams	p. 285
9.2 Concepts	p. 288
9.3 Ideal Solutions	p. 296
9.4 Vapor-Liquid Equilibrium (VLE) Calculations	p. 301
Example 9.1 Bubble and dew temperatures and isothermal flash of ideal solutions	p. 305
9.5 Emission Modeling	p. 307
9.6 Non-Ideal Systems	p. 310
9.7 Advanced Topics (Optional)	p. 313
9.8 Summary And Concluding Remarks	p. 314
9.9 Practice Problems	p. 315
9.10 Homework Problems	p. 315
Chapter 10 Phase Equilibria in Mixtures by an Equation of State	p. 319
Example 10.1 The virial equation for vapor mixtures	p. 321
10.1 A Simple Model for Mixing Rules	p. 321
10.2 Fugacity and Chemical Potential From An Eos	p. 324
Example 10.2 K-values from the Peng-Robinson equation	p. 328
10.3 Differentiation of Mixing Rules	p. 329
Example 10.3 Fugacity coefficient from the virial equation	p. 331
Example 10.4 Fugacity coefficient for van der Waals equation	p. 332
Example 10.5 Fugacity coefficient from the Peng-Robinson equation	p. 334
10.4 Vle Calculations by an Equation of State	p. 335
Example 10.6 Bubble point pressure from the Peng-Robinson equation	p. 336
Example 10.7 Isothermal flash using the Peng-Robinson equation	p. 337
Example 10.8 Phase diagram for azeotropic methanol + benzene	p. 339
Example 10.9 Phase diagram for nitrogen + methane	p. 340
Example 10.10 Ethane + heptane phase envelopes	p. 342
10.5 Strategies for Applying Vle Routines	p. 344
10.6 Summary and Concluding Remarks	p. 345
10.7 Practice Problems	p. 345
10.8 Homework Problems	p. 346
Chapter 11 Activity Models	p. 355
11.1 Excess Properties	p. 356
11.2 Modified Raoult's Law and Excess Gibbs Energy	p. 357
Example 11.1 Activity coefficients and the Gibbs-Duhem relation (optional)	p. 359
Example 11.2 VLE prediction using UNIFAC activity coefficients	p. 360
11.3 Determination of G[superscript E] From Experimental Data	p. 363
Example 11.3 Gibbs excess energy for system 2-propanol + water	p. 363
Example 11.4 Activity coefficients by the one-parameter Margules equation	p. 365
Example 11.5 VLE predictions from the Margules one-parameter equation	p. 365
11.4 The Van Der Waals' Perspective	p. 367
Example 11.6 Application of the van Laar equation	p. 370
Example 11.7 Infinite dilution activity coefficients from van Laar theory	p. 371
Example 11.8 VLE predictions using regular-solution theory	p. 373
Example 11.9 Scatchard-Hildebrand versus van Laar theory for methanol + benzene	p. 375
Example 11.10 Combinatorial contribution to the activity coefficient	p. 378
Example 11.11 Polymer mixing	p. 378
11.5 Flory-Huggins and Van Der Waals' Theories (Optional)	p. 379
11.6 Local Composition Theory	p. 381
Example 11.12 Local compositions in a 2-dimensional lattice	p. 383
Example 11.13 Application of Wilson's equation to VLE	p. 388
Example 11.14 Calculation of group mole fractions	p. 397
Example 11.15 Detailed calculations of activity coefficients via UNIFAC	p. 397
11.7 Fitting Activity Models to Data (Optional)	p. 400
Example 11.16 Using Excel for fitting model parameters	p. 401
11.8 T and P Dependence of Gibbs Energy (Optional)	p. 403
11.9 The Molecular Basis of Solution Models (Optional)	p. 404
11.10 Summary	p. 410
11.11 Practice Problems	p. 411
11.12 Homework Problems	p. 412
Chapter 12 Liquid-Liquid Phase Equilibria	p. 423
12.1 The Onset of Liquid-Liquid Instability	p. 423
Example 12.1 Simple liquid-liquid-vapor equilibrium (LLVE) calculations	p. 424
12.2 Stability and Excess Gibbs Energy	p. 424
Example 12.2 LLE predictions using Flory-Huggins theory: polymer mixing	p. 426
Example 12.3 LLE predictions using UNIFAC	p. 427
12.3 Plotting Ternary Lle Data	p. 430
12.4 Vlle With Immiscible Components	p. 432
Example 12.4 Steam distillation	p. 432
12.5 Critical Points in Binary Liquid Mixtures (Optional)	p. 433
Example 12.5 Liquid-liquid critical point of the Margules one-parameter model	p. 434
Example 12.6 Liquid-liquid critical point of the Flory-Huggins model	p. 435
12.6 Excel Procedure for Binary, Ternary Lle (Optional)	p. 436
12.7 Summary	p. 438
12.8 Practice Problems	p. 439
12.9 Homework Problems	p. 439
Chapter 13 Special Topics	p. 445
13.1 Phase Behavior	p. 445
13.2 Solid-Liquid Equilibria	p. 459
Example 13.1 Eutectic behavior of chloronitrobenzenes	p. 463
Example 13.2 Eutectic behavior of benzene + phenol	p. 464
Example 13.3 Wax precipitation	p. 465
13.3 Residue Curves	p. 470
13.4 Homework Problems	p. 475
Unit Iv Reacting Systems	p. 481
Chapter 14 Reacting Systems	p. 483
14.1 Reaction Coordinate	p. 483
Example 14.1 Stoichiometry and the reaction coordinate	p. 485
14.2 Equilibrium Constraint	p. 486
Example 14.2 Calculation of standard state Gibbs energy of reaction	p. 487
14.3 Reaction Equilibria for Ideal Solutions	p. 489
Example 14.3 Computing the reaction coordinate	p. 489
Example 14.4 Butadiene revisited	p. 490
14.4 Temperature Effects	p. 492
Example 14.5 Equilibrium constant as a function of temperature	p. 493
14.5 Shortcut Estimation of Temperature Effects	p. 494
Example 14.6 Application of the shortcut van't Hoff equation	p. 495
14.6 Energy Balances for Reactions	p. 496
Example 14.7 Adiabatic reaction in an ammonia reactor	p. 498
14.7 General Observations About Pressure Effects	p. 502
14.8 Multireaction Equilibria	p. 503
Example 14.8 Simultaneous reactions that can be solved by hand	p. 503
Example 14.9 Solving multireaction equilibrium equations by EXCEL	p. 505
Example 14.10 Direct minimization of the Gibbs energy with EXCEL	p. 507
Example 14.11 Pressure effects for Gibbs energy minimization	p. 509
14.9 Simultaneous Reaction and Phase Equilibrium	p. 510
Example 14.12 The solvent methanol process	p. 511
Example 14.13 NO[subscript 2] absorption	p. 514
14.10 Electrolyte Thermodynamics	p. 516
Example 14.14 Chlorine + water electrolyte solutions	p. 517
14.11 Solid Components in Reactions	p. 520
Example 14.15 Thermal decomposition of methane	p. 521
14.12 Summary and Concluding Remarks	p. 521
14.13 Practice Problems	p. 522
14.14 Homework Problems	p. 524
Chapter 15 Molecular Association and Solvation	p. 529
15.1 Association and Solvation	p. 529
15.2 Equilibrium Criteria	p. 534
15.3 Balance Equations	p. 536
15.4 Ideal Chemical Theory	p. 537
Example 15.1 Compressibility factors in associating/solvating systems	p. 538
Example 15.2 Dimerization of carboxylic acids	p. 539
Example 15.3 Activity coefficients in a solvated system	p. 540
15.5 Chemical-Physical Theory	p. 541
15.6 Pure Species With Linear Association	p. 542
15.7 A Van Der Waals H-Bonding Model	p. 547
Example 15.4 Molecules of H[subscript 2]O in a 100-ml beaker	p. 551
15.8 The Esd Equation for Associating Fluids	p. 555
15.9 Extension to Complex Mixtures	p. 565
15.10 Statistical Associating Fluid Theory (SAFT)	p. 569
15.11 Summary Analysis of Association Models	p. 571
15.12 Homework Problems	p. 573
Glossary	p. 579
Appendix A Summary of Computer Programs	p. 583
A.1 HP48 Calculator Programs	p. 583
A.2 TI-85 Programs	p. 587
A.3 PC Programs for Pure Component Properties	p. 587
A.4 PC Programs for Mixture Phase Equilibria	p. 587
A.5 Reaction Equilibria	p. 588
A.6 How to Load Programs	p. 589
A.7 Downloading HP Programs	p. 589
A.8 Using Fortran Programs	p. 589
A.9 Notes on Excel Spreadsheets	p. 590
A.10 Notes on HP Calculator	p. 595
A.11 Disclaimer	p. 597
Appendix B Mathematics	p. 599
B.1 Important Relations	p. 599
B.2 Solutions to Cubic Equations	p. 603
B.3 The Dirac Delta Function	p. 606
Example B.1 The Hard Sphere Equation of State	p. 608
Example B.2 The Square-Well Equation of State	p. 610
Appendix C Strategy for Solving Vle Problems	p. 613
C.1 Eos Methods	p. 613
C.2 Activity Coefficient (Gamma-Phi) Method	p. 618
Appendix D Models for Process Simulators	p. 623
D.1 Overview	p. 623
D.2 Equations of State	p. 623
D.3 Solutions Models	p. 624
D.4 Hybrid Models	p. 624
D.5 Recommended Decision Tree	p. 625
D.6 Thermal Properties of Mixtures	p. 626
Example D.1 Contamination from a reactor leak	p. 627
D.7 Literature Cited	p. 628
Appendix E Pure Component Properties	p. 631
E.1 Ideal Gas Heat Capacities	p. 631
E.2 Liquid Heat Capacities	p. 634
E.3 Solid Heat Capacities	p. 634
E.4 Antoine Constants	p. 635
E.5 Latent Heats	p. 636
E.6 Enthalpies and Gibbs Energies of Formation	p. 637
E.7 Properties of Water	p. 640
E.8 Pressure-Enthalpy Diagram for Methane	p. 651
E.9 Pressure-Enthalpy Diagram for Propane	p. 652
E.10 Thermodynamic Properties of Hfc-134a	p. 653
Index	p. 655

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