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This brand-new text makes thermodynamics far easier to teach and learn. Drawing on his award-winning courses at Penn State, Dr. Themis Matsoukas organizes the test for more effective learning, focuses on "why" as well as "how," offers imagery that helps students conceptualize the equations, and illuminates thermodynamics with relevant examples from within and beyond the chemical engineering discipline. Matsoukas presents solved problems in every chapter, ranging from basic calculations to realistic safety and environmental applications. Part I introduces the First and Second laws of thermodynamics. Part II presents the equation of state and the phase diagram of pure component, and establishes methodologies for calculating thermodynamic properties from equations of state, charts, and correlations. These methodologies are applied to closed and open systems of varying complexity, from isolated units (heat exchangers, throttling valves, and compressors) to power plants and refrigeration cycles. Part III focuses on mixtures, surveying phase diagrams, introducing the calculus of multicomponent thermodynamics, and applying the theory to vapor/liquid equilibrium. Matsoukas concludes by discussing reacting mixtures, including energy balances and equilibrium calculations. Throughout, many problems require mathematical software; however, instructors have the flexibility to use any software package they prefer.

Themis Matsoukas has taught graduate and undergraduate thermodynamics, materials and energy balances, and various electives at Penn State–home to one of the world’s largest undergraduate programs in engineering–since 1991. He has taught thermodynamics more than twenty times, to more than a thousand undergraduate students. His honors at Penn State include the George W. Atherton Award for Excellence in Teaching (2009); the Outstanding Teaching Award, Penn State Engineering Society (2006); and the AXE: Outstanding Teacher Award (2005).

Preface         xiii
Acknowledgments         xvii

About the Author         xix

Nomenclature         xxi

Part I: Pure Fluids 1

Chapter 1: Scope and Language of Thermodynamics 3

1.1 Molecular Basis of Thermodynamics 5

1.2 Statistical versus Classical Thermodynamics 11

1.3 Definitions 13

1.4 Units 22

1.5 Summary 26

1.6 Problems 26

Chapter 2: Phase Diagrams of Pure Fluids 29

2.1 The PVT Behavior of Pure Fluid 29

2.2 Tabulation of Properties 40

2.3 Compressibility Factor and the ZP Graph 43

2.4 Corresponding States 45

2.5 Virial Equation 53

2.6 Cubic Equations of State 57

2.7 PVT Behavior of Cubic Equations of State 61

2.8 Working with Cubic Equations 64

2.9 Other Equations of State 67

2.10 Thermal Expansion and Isothermal Compression 71

2.11 Empirical Equations for Density 72

2.12 Summary 77

2.13 Problems 78

Chapter 3: Energy and the First Law 87

3.1 Energy and Mechanical Work 88

3.2 Shaft Work and PV Work 90

3.3 Internal Energy and Heat 96

3.4 First Law for a Closed System 98

3.5 Elementary Paths 101

3.6 Sensible Heat–Heat Capacities 109

3.7 Heat of Vaporization 119

3.8 Ideal-Gas State 124

3.9 Energy Balances and Irreversible Processes 133

3.10 Summary 139

3.11 Problems 140

Chapter 4: Entropy and the Second Law 149

4.1 The Second Law in a Closed System 150

4.2 Calculation of Entropy 153

4.3 Energy Balances Using Entropy 163

4.4 Entropy Generation 167

4.5 Carnot Cycle 168

4.6 Alternative Statements of the Second Law 177

4.7 Ideal and Lost Work 183

4.8 Ambient Surroundings as a Default Bath–Exergy 189

4.9 Equilibrium and Stability 191

4.10 Molecular View of Entropy 195

4.11 Summary 199

4.12 Problems 201

Chapter 5: Calculation of Properties 205

5.1 Calculus of Thermodynamics 205

5.2 Integration of Differentials 213

5.3 Fundamental Relationships 214

5.4 Equations for Enthalpy and Entropy 217

5.5 Ideal-Gas State 219

5.6 Incompressible Phases 220

5.7 Residual Properties 222

5.8 Pressure-Explicit Relations 228

5.9 Application to Cubic Equations 230

5.10 Generalized Correlations 235

5.11 Reference States 236

5.12 Thermodynamic Charts 242

5.13 Summary 245

5.14 Problems 246

Chapter 6: Balances in Open Systems 251

6.1 Flow Streams 252

6.2 Mass Balance 253

6.3 Energy Balance in Open System 255

6.4 Entropy Balance 258

6.5 Ideal and Lost Work 266

6.6 Thermodynamics of Steady-State Processes 272

6.7 Power Generation 295

6.8 Refrigeration 301

6.9 Liquefaction 309

6.10 Unsteady-State Balances 315

6.11 Summary 323

6.12 Problems 324

Chapter 7: VLE of Pure Fluid 337

7.1 Two-Phase Systems 337

7.2 Vapor-Liquid Equilibrium 340

7.3 Fugacity 343

7.4 Calculation of Fugacity 345

7.5 Saturation Pressure from Equations of State 353

7.6 Phase Diagrams from Equations of State 356

7.7 Summary 358

7.8 Problems 360

Part II: Mixtures 367

Chapter 8: Phase Behavior of Mixtures 369

8.1 The Txy Graph 370

8.2 The Pxy Graph 373

8.3 Azeotropes 380

8.4 The xy Graph 381

8.5 VLE at Elevated Pressures and Temperatures 383

8.6 Partially Miscible Liquids 384

8.7 Ternary Systems 390

8.8 Summary 393

8.9 Problems 394

Chapter 9: Properties of Mixtures 401

9.1 Composition 402

9.2 Mathematical Treatment of Mixtures 404

9.3 Properties of Mixing 409

9.4 Mixing and Separation 411

9.5 Mixtures in the Ideal-Gas State 413

9.6 Equations of State for Mixtures 419

9.7 Mixture Properties from Equations of State 421

9.8 Summary 428

9.9 Problems 428

Chapter 10: Theory of Vapor-Liquid Equilibrium 435

10.1 Gibbs Free Energy of Mixture 435

10.2 Chemical Potential 439

10.3 Fugacity in a Mixture 443

10.4 Fugacity from Equations of State 446

10.5 VLE of Mixture Using Equations of State 448

10.6 Summary 453

10.7 Problems 454

Chapter 11: Ideal Solution 461

11.1 Ideality in Solution 461

11.2 Fugacity in Ideal Solution 464

11.3 VLE in Ideal Solution—Raoult’s Law 466

11.4 Energy Balances 475

11.5 Noncondensable Gases 480

11.6 Summary 484

11.7 Problems 484

Chapter 12: Nonideal Solutions 489

12.1 Excess Properties 489

12.2 Heat Effects of Mixing 496

12.3 Activity Coefficient 504

12.4 Activity Coefficient and Phase Equilibrium 507

12.5 Data Reduction: Fitting Experimental Activity Coefficients 512

12.6 Models for the Activity Coefficient 515

12.7 Summary 531

12.8 Problems 533

Chapter 13: Miscibility, Solubility, and Other Phase Equilibria 545

13.1 Equilibrium between Partially Miscible Liquids 545

13.2 Gibbs Free Energy and Phase Splitting 548

13.3 Liquid Miscibility and Temperature 556

13.4 Completely Immiscible Liquids 558

13.5 Solubility of Gases in Liquids 563

13.6 Solubility of Solids in Liquids 575

13.7 Osmotic Equilibrium 580

13.8 Summary 586

13.9 Problems 586

Chapter 14: Reactions 593

14.1 Stoichiometry 593

14.2 Standard Enthalpy of Reaction 596

14.3 Energy Balances in Reacting Systems 601

14.4 Activity 606

14.5 Equilibrium Constant 614

14.6 Composition at Equilibrium 622

14.7 Reaction and Phase Equilibrium 624

14.8 Reaction Equilibrium Involving Solids 629

14.9 Multiple Reactions 632

14.10 Summary 636

14.11 Problems 637

Bibliography 647

Appendix A: Critical Properties of Selected Compounds 649

Appendix B: Ideal-Gas Heat Capacities 653

Appendix C: Standard Enthalpy and Gibbs Free Energy of Reaction 655

Appendix D: UNIFAC Tables 659

Appendix E: Steam Tables 663

Index 677

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