THERMODYNAMICS OF MATERIALS VOLUME 1PDF电子书下载

Chapter 1 First Law 1

1.1 System and Surroundings 1

1.2 Energy Transfer 2

1.3 Energy of a System 4

1.4 Energy as a State Function 5

1.5 Work 5

1.6 The Closed System 7

1.7 Notation 8

1.8 Intensive and Extensive Properties 9

1.9 The Open System 10

1.10 Enthalpy 11

1.11 Steady State 11

1.12 Heat Capacity at Constant Volume 12

1.13 Heat Capacity at Constant Pressure 13

1.14 Adiabatic Flow Through a Valve: Joule-Thomson Expansion 16

1.15 Equations of State 17

1.16 Nonideal Gases 22

1.17 Adiabatic Compression or Expansion 26

1.18 Enthalpies of Formation 29

1.19 Enthalpy Changes in Chemical Reactions 31

1.20 Adiabatic Temperature Change in Chemical Reactions 34

References 38

Problems 38

Chapter 2 Second Law 45

2.1 Entropy as a State Function 46

2.2 Entropy Not Conserved 49

2.3 Open System Entropy Balance 50

2.4 Adiabatic, Reversible, Steady State System 50

2.5 Heat Engines 51

2.6 Diagrammatic Representation 54

2.7 Refrigerators 55

2.8 Heat Pumps 57

2.9 Entropy Changes 57

2.10 Entropy Changes in Chemical Reactions and the Third Law 60

References 62

Problems 62

Chapter 3 Property Relationships 67

3.1 The Property Relation 69

3.2 The Functions F and G 70

3.3 Chemical Potentials 71

3.4 Partial Molar Quantities 73

3.5 Property Relations Derived from U, H, F, and G 75

3.6 Ideal Gas 78

3.7 Entropy of Mixing 78

3.8 Heat Capacity 80

3.9 Variation of Heat Capacity 81

3.10 Isentropic Pressure-Temperature Relationship 82

3.11 Isentropic Compression of Solids 83

3.12 Thermoelastic Effect 84

3.13 Compressibility 87

3.14 Magnetic Effects 89

References 93

Problems 93

Chapter 4 Equilibrium 97

4.1 Condition of Equilibrium 98

4.2 Barometric Equation 100

4.3 Phase Equilibria 101

4.4 Special Case: Closed System, Constant Volume 103

4.5 First-Order Transitions: Variation of Equilibrium Pressure with Temperature 104

4.6 Clapeyron Equation in Vapor Equilibria 107

4.7 Variation of Vapor Pressure of a Condensed Phase with Total Applied Pressure 109

4.8 Variation of Vapor Pressure with Particle Size 111

4.9 Second-Order Transitions 112

4.10 Superconductivity: An Example 114

References 116

Problems 116

Chapter 5 Chemical Equilibrium 119

5.1 Thermodynamic Activity 119

5.2 Chemical Equilibrium 122

5.3 Gaseous Equilibria 123

5.4 Solid-Vapor Equilibria 125

5.5 Sources of Information on ？G° 127

5.6 Ellingham Diagrams 130

5.7 Variation of Equilibrium Constant with Temperature 135

5.8 Gases Dissolved in Metals (Sievert's Law) 138

5.9 Chemical Equilibrium and Adiabatic Flame Temperatures 139

References 144

Problems 144

Chapter 6 Electrochemistry 149

6.1 Electrochemical Cell 150

6.2 Nomenclature 151

6.3 Calculation of Cell Voltage 152

6.4 Direction of Reaction 153

6.5 Half-Cell Reactions 154

6.6 Variation of Voltage with Concentration: Nernst Equation 156

6.7 Pourbaix Diagrams 156

6.8 Concentration Cells 159

6.9 Oxygen Pressure Determination 161

6.10 Temperature Dependence of Voltage 162

6.11 Electrochemical Potential 162

References 164

Problems 164

Chapter 7 Solutions 169

7.1 Thermodynamic Activity 169

7.2 Partial Molar Quantities 171

7.3 Relative Partial Molar Quantities 173

7.4 Entropy of Mixing: Ideal Solution 174

7.5 Enthalpy of Mixing: Ideal Solution 174

7.6 Graphical Representation 175

7.7 Nonideal Solutions 178

7.8 Gibbs-Duhem Relation 181

7.9 Dilute Solutions and Colligative Properties 183

7.10 Integrating the Gibbs-Duhem Equation 184

7.11 Regular Solutions 186

7.12 Regular Solutions: Atomistic Interpretation 188

7.13 Polymer Solutions 190

7.14 Osmotic Pressure 192

References 195

Problems 195

Chapter 8 Phase Rule 199

8.1 Phases 199

8.2 Components 200

8.3 Specifying a System 200

8.4 Equilibrium Conditions 201

8.5 Gibbs Phase Rule 201

8.6 One-Component System 201

8.7 Examples 202

8.8 Phase Rule for Condensed Systems 204

Problems 205

Chapter 9 Phase Diagrams 207

9.1 Freezing Point Depression 208

9.2 The Lever Rule 211

9.3 Simple Eutectic Diagram 213

9.4 Cooling Curves 214

9.5 Complete Miscibility 216

9.6 Immiscibility 220

9.7 Spinodal Points 222

9.8 Peritectic Phase Diagrams 224

9.9 Compounds 225

9.10 Ternary Diagrams 225

References 234

Problems 234

Chapter 10 Statistical Thermodynamics 245

10.1 Average Velocity of Gas Molecules 246

10.2 Macrostates and Microstates 249

10.3 Isolated Systems and the Boltzmann Hypothesis 252

10.4 The Third Law 254

10.5 Systems at Constant Temperature 255

10.6 Information and Entropy 256

10.7 Boltzmann Distribution 258

10.8 Degeneracy 262

10.9 Partition Function 263

10.10 Distinguishability of Particles 264

10.11 Ideal Gas 265

10.12 Maxwell-Boltzmann Distribution: Ideal Gas 267

10.13 Fermi-Dirac Distribution 270

10.14 Heat Capacity of Solids 274

10.15 Molecular Weight Distribution in Polymers 278

10.16 Entropy of Mixing of Polymer Solutions 284

References 287

Appendix 10.A: Proof that β = 1/kT 287

Problems 288

Appendix Background 293

A.1 Length 294

A.2 Mass and Amount of Material 294

A.3 Time 294

A.4 Electric Current 295

A.5 Temperature 295

A.6 Force 296

A.7 Pressure 296

A.8 Volume 296

A.9 Energy 296

A.10 Power 297

A.11 Composition 297

A.12 Checking Units 298

A.13 Logarithms 299

A.14 Differentials 300

A.15 Partial Derivatives 300

A.16 Total Differential 301

A.17 Factorials 301

A.18 Homogeneous Functions 302

A.19 Lagrange Method of Undetermined Multipliers 302

Exercises in Unit Conversions 306

Index 309