[醉染正版]物理化学 Physical Chemistry 英文版 景苏 高等院校化工化学类材料类制药类环境类等专业 基

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ISBN编号: 9787122385390

书名: 物理化学=Physical Chemistry：英文

作者: 无

定价: 49.80元

是否是套装: 否

出版社名称: 化学工业出版社

《物理化学（英文版）Physical Chemistry》为“十三五”江苏省高等学校本科重点教材（新编）。本书是在继承既有物理化学中文、英文教材体系成果的基础上编写而成的，在“新工科”理念指导下，注重借助数学、物理等基础科学的理论原理及新实验技术手段研究化学变化中的基本规律。本书共包括九章内容，分别是气体的性质、热力学、热力学二定律、多组分系统热力学、化学平衡、相平衡、电化学平衡、化学动力学和界面化学，每章均配有与章节基本概念、公式和知识内容相对应的不同难度的例题、练习题和思考题，有助于巩固掌握基础知识，增强解题及逻辑思维能力。
本书注重提高学生的学习兴趣和效果，培养多学科基础厚实、工程能力强、综合素质高且能实现跨界整合的复合型人才。本书既可作为高等院校化工类、化学类、材料类、生工制药类、环境类等专业基础物理化学课程的全英文教学用书，也可供其他相关专业使用，并可作为相关科研和工程技术人员的参考用书。

Chapter 1 The Properties of Gases 1
1.1 State Equation of the Ideal Gas 1
1.1.1 Empirical Laws of Gases 1
1.1.2 State Equation of Ideal Gas 2
1.1.3 Model and Definition of Ideal Gas 4
1.2 The Properties of Mitures of the Ideal Gases 5
1.2.1 Composition of Mitures 5
1.2.2 Dalton’s Law of Partial Pressures 6
1.2.3 Amagat’s Law of Partial Volumes 7
1.3 State Equations of Real Gas 8
1.3.1 The van der Waals Equation 8
1.3.2 Generalized Equation of State for Real Gases 9
1.4 Isothermal Curves and Liquefaction of Real Gas 10
1.4.1 Saturated Vapor Pressure of the Liquid 10
1.4.2 Isothermal Curves and Liquefaction 12
1.4.3 Critical Parameters and Critical Compression Factor Zc 14
1.5 Eercises 15

Chapter 2 The First Law of Thermodynamics 17
2.1 Basic Concepts 17
2.1.1 System and Surroundings 17
2.1.2 Property, State, and State Function 18
2.1.3 Process and Route 19
2.1.4 Work, Heat, and Energy 20
2.2 The First Law of Thermodynamics 22
2.2.1 The First Law of Thermodynamics 22
2.2.2 Internal Energy 23
2.3 Heat, Enthalpy, and Heat Capacities 23
2.3.1 Heat in Isochoric Conditions, and Internal Energy 23
2.3.2 Heat in Isobaric Conditions, and Enthalpy 25
2.3.3 Hess’s Law 26
2.3.4 Heat Capacities 27
2.4 Pressure-Volume Work and Reversible Processes 29
2.4.1 Pressure-Volume Work 29
2.4.2 Reversible Processes 30
2.5 Isoenthalpic Processes 36
2.5.1 The Joule-Thomson Effect 36
2.5.2 Adiabatic Joule-Thomson Coefficient 37
2.6 Thermochemistry 37
2.6.1 Standard Enthalpy of Formation 38
2.6.2 Enthalpy of Reaction 39
2.6.3 Temperature-Dependence of Standard Enthalpy of Reaction 40
2.7 Eercises 41

Chapter 3 The Second Law of Thermodynamics 42
3.1 Statements of the Second Law of Thermodynamics 42
3.1.1 Spontaneous Process 42
3.1.2 Conversion of Heat and Work 43
3.1.3 Statements of the Second Law of Thermodynamics 43
3.2 Cart Cycle and Cart Theorem 44
3.2.1 Cart Cycle 44
3.2.2 Cart Theorem 45
3.3 Entropy and Clausius Inequality 46
3.3.1 Derivation and Definition of Entropy 46
3.3.2 The Clausius Inequality 47
3.3.3 The Principle of the Increase of Entropy 47
3.3.4 Physical Significance of Entropy 48
3.4 The Calculation of Entropy Changes 49
3.4.1 The Calculation of Entropy Changes in Simple pVT Process 49
3.4.2 The Calculation of Entropy Changes for Phase Changes 51
3.5 The Standard Molar Reaction Entropy Change of Chemical Reaction 52
3.5.1 The Third Law of Thermodynamics 52
3.5.2 Absolute Entropy and Standard Molar Entropy of Matter 52
3.5.3 Calculation of Entropy Changes for Chemical Reactions 53
3.6 The Gibbs and Helmholtz Functions 55
3.6.1 Helmholtz Function 55
3.6.2 Gibbs Function 56
3.7 The Calculation of ΔA and ΔG 57
3.7.1 Simple pVT Change Process 57
3.7.2 Phase Change Processes 57
3.7.3 Chemical Change Processes 58
3.8 The Fundamental Equation of Thermodynamics 59
3.8.1 The Fundamental Equations of Thermodynamics 59
3.8.2 The Relations of Characteristic Function 60
3.8.3 The Mawell Relations 61
3.9 The Application of the Second Law of Thermodynamics in the Phase Equilibria of Single Component Systems 62
3.9.1 The Clapeyron Equation 62
3.9.2 The Clausius-Clapeyron Equation 63
3.9.3 The Effect of Total Pressure on the Vapor Pressure 64
3.10 Eercises 65

Chapter 4 The Thermodynamics of Multi-Component Systems 68
4.1 Composition scale of multi-component systems 68
4.1.1 Mass Concentration 68
4.1.2 Amount of Substance concentration 68
4.1.3 Molality 69
4.2 Partial Molar Quantities 69
4.2.1 Definition of Partial Molar Quantity 70
4.2.2 Collected Formula of Partial Molar Quantity 71
4.2.3 The Gibbs-Duhem Equation 71
4.3 Chemical Potential 72
4.3.1 Definition of Chemical Potential 72
4.3.2 Equilibrium Criterion of Material 73
4.3.3 Application of Chemical Potential in Phase Equilibrium 74
4.4 Chemical Potential of Gas 75
4.4.1 Chemical Potential of a Pure Ideal Gas 75
4.4.2 Chemical Potentials in an Ideal Gas Miture 76
4.5 Raoult’s law and Henry’s law 77
4.5.1 Raoult’s Law 77
4.5.2 Henry’s Law 78
4.5.3 Comparison of Raoult’s Law and Henry’s Law 79
4.6 Miture of Ideal Liquid 79
4.6.1 Definition and Features of Miture of Ideal Liquid 79
4.6.2 Chemical Potential of Arbitrary Component in Miture of Ideal Liquid 80
4.6.3 Miing Properties of Miture of Ideal Liquid 81
4.7 Ideal Dilute Solution 82
4.7.1 Definition of Ideal Dilute Solution 82
4.7.2 Chemical Potential of the Solvent and Solute in Ideal Dilute Solution 82
4.8 Real Liquid Solution 83
4.8.1 The Solvent Activity 83
4.8.2 The Solute Activity 84
4.9 Colligative Properties 84
4.9.1 Depression of Vapor Pressure (Vapor Pressure of Solvent A) 85
4.9.2 Depression of Freezing Point 85
4.9.3 Elevation of Boiling Point 87
4.9.4 Osmotic Pressure 89
4.10 Eercises 90

Chapter 5 Chemical Equilibrium 92
5.1 Direction of Chemical Reaction and Condition of Equilibrium 92
5.1.1 Relationship between Condition of Equilibrium and Etent of Chemical Reaction 92
5.1.2 Chemical Affinity and Direction of Chemical Reaction 93
5.2 Equilibrium Constant Epressions for Gas Reaction 95
5.2.1 Isothermal Equation for Ideal Gas Reaction 95
5.2.2 Standard Equilibrium Constant Epression for Ideal Gas Reaction 96
5.2.3 Standard Equilibrium Constant Epression for Ideal Gas Reaction involving Pure Condensed Matter 97
5.2.4 Other Equilibrium Constant Epressions for Ideal Gas Reaction 99
5.2.5 Relationship between Dissociation Pressure and Standard Equilibrium Constant for Dissociation Reaction of Solid 100
5.2.6 Inherent Relation between Standard Equilibrium Constants of Relative Reactions 101
5.3 Calculation of Chemical Equilibrium 102
5.3.1 Calculation of Standard Molar Gibbs Function Change of Reaction and Standard Equilibrium Constant 102
5.3.2 Calculation of Equilibrium Composition of System and Equilibrium Conversion of Reactant 104
5.4 Response of Equilibrium to Conditions 106
5.4.1 Response of Equilibrium to Temperature 106
5.4.2 Response of Equilibrium to Pressure 107
5.4.3 Response of Equilibrium to Inert Component 108
5.4.4 Response of Equilibrium to Starting Materials Ratio 108
5.5 Eercises 109

Chapter 6 Phase Equilibrium 112
6.1 Phase Rule 113
6.1.1 Basic Concept 113
6.1.2 Phase Rule 114
6.2 Phase Diagram of One-Component System 116
6.2.1 Phase Diagram of Water 117
6.2.2 Phase Diagram of Sulfur 119
6.3 Gas-Liquid Phase Diagram of Two-Component Ideal Liquid Miture System 120
6.3.1 Pressure-composition Phase Diagram 121
6.3.2 Lever Rule 123
6.3.3 Temperature-composition Phase Diagram 123
6.4 Gas-Liquid Phase Diagram of Two-Component Real Liquid Miture System 124
6.4.1 Pressure-composition Phase Diagram 124
6.4.2 Temperature-composition Phase Diagram 126
6.5 Distillation Principle 128
6.6 Gas-Liquid Phase Diagrams of Partially Miscible and nmiscible Two-Component Liquid Systems 130
6.6.1 Solubility Relation of Partially Miscible Liquids 130
6.6.2 Temperature-composition Phase Diagrams of Partially Miscible Systems 131
6.6.3 Temperature-composition Phase Diagram of nmiscible System 131
6.7 Liquid-Solid Phase Diagram of Two-Component Condensed System with Solid-Phase Immiscibility 132
6.7.1 Phase Diagram Analysis 133
6.7.2 Thermal Analysis Method 134
6.7.3 Solubility Method 137
6.8 Liquid-Solid Phase Diagram of Condensed System for the Formation of Compounds 138
6.8.1 Liquid-solid Phase Diagram for the Formation of a Stable Compound System 138
6.8.2 Liquid-solid Phase Diagram for the Formation of an Unstable Compound System 139
6.9 Liquid-Solid Phase Diagram of Two-Component Condensed Systems with Solid-Phase Miscibility and Partial Miscibility 140
6.9.1 Liquid-solid Phase Diagram of Solid-phase Complete Miscibility System 140
6.9.2 Liquid-solid Phase Diagram of Solid-phase Partially Miscible System 141
6.10 Liquid-Solid Phase Diagram of Two-Component Systems with Solid-Phase Immiscible and Liquid-Phase Miscible 143
6.11 Liquid-Liquid Equilibrium Phase Diagram for Three-Component System 145
6.11.1 Graphical Representation of a Three-component System 145
6.11.2 Liquid-liquid Phase Diagram of Three-liquid System with One Pair of Partially Soluble Liquids at Constant Temperature 147
6.12 Eercises 147

Chapter 7 Electrochemistry 153
7.1 Basic Concepts and Faraday's Law 155
7.1.1 Electrolyte and Types of Electrolyte 155
7.1.2 Galvanic Cell, Electrolytic Cell and Conductance Mechanism of Electrolyte Solution 155
7.1.3 Faraday’s Law 158
7.2 Mobility and Transference Number of Ions 160
7.2.1 Mobility and Transference Number of Ions 160
7.2.2 Determination of Transference Numbers of Ions 164
7.3 Conductance, Conductivity and Molar Conductivity 165
7.3.1 Conductance and Conductivity 166
7.3.2 Measurement of Conductance 168
7.3.3 Molar Conductivity and Its Relation to the Concentration of Electrolyte Solution 169
7.3.4 Law of the Independent Migration of Ions and Limiting Molar Conductivity of Ions 171
7.4 Application of Conductance Measurement 174
7.4.1 Calculate the Degree of Dissociation and the Dissociation Constant of Weak Electrolyte 174
7.4.2 Calculate the Solubility of Insoluble Salts 176
7.4.3 Conductance Titration 177
7.5 Activities and Activity Coefficients of Electrolyte Solution 178
7.5.1 Mean Ionic Activity and Mean Ionic Activity Coefficient 178
7.5.2 Ionic Intensity I 180
7.5.3 Debye-Hückel Theory to Calculating γ± 181
7.6 Reversible Galvanic Cell 184
7.6.1 Galvanic Cell and Its Representation 185
7.6.2 Preconditions for Being a Reversible Cell 188
7.6.3 Weston Standard Cell 189
7.7 Thermodynamics of Reversible Galvanic Cells 190
7.7.1 Calculating the Change of Molar Gibbs Function of Cell Reaction ΔrGm from the Reversible E of Cell 190
7.7.2 Calculating the Molar Reaction Entropy of Cell Reaction ΔrSm from Temperature Coefficient of E 191
7.7.3 Calculating the Molar Reaction Enthalpy of Cell Reaction ΔrHm 191
7.7.4 Calculating the Thermal Effect of the Reversible Discharge Process of a Galvanic Cell Qr,m 192
7.7.5 The Nernst Equation of Cell Reaction 193
7.8 Electrode Potential and the Electromotive Force of Cell 196
7.8.1 Electrode Potential 196
7.8.2 Nernst Equation for Electrode Potential 197
7.8.3 Calculation of Electromotive Force for Galvanic Cell 200
7.8.4 Liquid-junction Potential and Its Elimination 202
7.9 Types of Reversible electrodes 204
7.9.1 First-class Electrodes 204
7.9.2 Second-class Electrodes 205
7.9.3 Third-class Electrodes 206
7.9.4 Ion-selective Electrode 207
7.10 Design of Galvanic Cell 208
7.10.1 Redo Reactions 208
7.10.2 Neutralization Reaction 209
7.10.3 Precipitation Reaction 209
7.10.4 Diffusion Process 209
7.11 Determination and Application of Electromotive Force of Reversible Cell 210
7.11.1 The Principle of EMF Measurement 210
7.11.2 Determination of the Mean ionic Activity Coefficients γ± 211
7.11.3 Determination of the Standard Equilibrium Constant K and the Solubility Product Kap of Insoluble Salt 211
7.11.4 Measurement of pH 213
7.12 Electrolytic Cell and Decomposition Voltage 214
7.12.1 Electrolytic Cell and Decomposition Voltage 214
7.12.2 Polarization 216
7.12.3 Electrode Reaction in Electrolysis 220
7.13 Eercises 221

Chapter 8 Chemical Kinetics 226
8.1 The Rates of Reactions 226
8.1.1 The definition of rate 226
8.1.2 The Determination of Rate 228
8.2 The Rate Laws of Reactions 228
8.2.1 The Reaction Mechanism and Elementary Reactions 228
8.2.2 Rate Laws of Reactions 229
8.2.3 Rate Laws of Gas-Phase Reactions 230
8.3 Integrated Rate Laws of Reactions with Simple Orders 230
8.3.1 Zeroth-Order Reactions 230
8.3.2 First-Order Reactions 231
8.3.3 Second-Order Reactions 232
8.3.4 nth-Order Reactions 233
8.4 Determination of Reaction Orders 234
8.4.1 The Method of Integrated Rate Laws 234
8.4.2 The Method of Differential Rate Laws 234
8.4.3 The Method of Half-Lifes 235
8.4.4 The Method of Initial Rates 235
8.5 The Effect of Temperature on Reaction Rates 236
8.5.1 The Arrhenius Equation 236
8.5.2 The Activation Energy 237
8.5.3 Apparent Activation Energy 237
8.5.4 Relationship between the Activation Energy and the Reaction Heat 238
8.6 Typical Comple Reactions 239
8.6.1 Opposing Reactions 239
8.6.2 Parallel Reactions 240
8.6.3 Consecutive Reactions 240
8.7 Approimations for Comple Reactions 241
8.7.1 The Rate-Determining Step Approimation 241
8.7.2 The Equilibrium-State Approimation 242
8.7.3 The Steady-State Approimation 242
8.8 Eercises 242

Chapter 9 Interface Chemistry 246
9.1 Interfacial Tension 247
9.1.1 Surface Tension, Surface Work, and the Surface Gibbs Function of the Liquid 247
9.1.2 Surface Thermodynamic Fundamental Equation 249
9.1.3 Factors Affecting Interfacial Tensions 250
9.2 Ecess Pressure at Curved Liquid Surface and Capillarity 251
9.2.1 Ecess Pressure at Curved Liquid Surface 251
9.2.2 Capillarity Action 253
9.3 Kelvin Equation and Metastable State 254
9.3.1 The Vapour Pressure over A Small Droplet ——the Kelvin Equation 254
9.3.2 Metastable State and the Generation of New Phases 255
9.4 Adsorption on Solids Surface 257
9.4.1 Physical Adsorption and Chemisorption 258
9.4.2 Amount of Adsorption and Isotherm Equations 259
9.4.3 Adsorption Isotherm Equations 260
9.4.4 Thermodynamics of Adsorption 264
9.5 The Solid-Liquid Interface and Wetting Phemen 264
9.5.1 Wetting Phemen 264
9.5.2 Contact Angle and Young Equation 266
9.6 Adsorption of Solution Surface 268
9.6.1 Adsorption Phemena at Solution Surface 268
9.6.2 Surface Adsorption and Gibbs Adsorption Isotherm 269
9.6.3 Directional Arrangement of Surfactants in Adsorption Layer 270
9.7 Eercises 272

Appendi 275
Appendi Ⅰ Critical Parameters of Certain Substances 275
Appendi Ⅱ Van der Waals Constants of Certain Gases 275
Appendi Ⅲ The Relationship between the Molar Heat Capacity of Certain Gases and the Temperature 276
Appendi Ⅳ Standard Molar Formation Enthalpy, Standard Molar Formation Gibbs Function, Standard Molar Entropy and Molar Constant Pressure Heat Capacity of Certain Substances 277
Appendi Ⅴ Standard Molar Combustion Enthalpy of Certain Organic Compounds 278

Reference 280