采用二维码，课外拓展资料、部分例题以文件、图片的方式，对物理化学典型题和重点知识点的讲解以视频方式加入教材

本书是为了适应物理化学双语教学这一全新的教学模式，解决物理化学双语教材短缺的问题，尽量做到内容精练、简明易懂，并坚持对每一部分内容均采用英、汉双语进行编写。内容包括：气体的pVT性质；化学热力学；多组分系统热力学；化学平衡；相平衡；电化学；界面现象；化学动力学。采用二维码将课外拓展资料、例题、典型题和重点知识点的讲解以文件、图片音频、视频等形式加入教材，使教材更加生动、形象、易于理解，提高使用者的学习兴趣。本书既可作为高等院校双语物理化学教学的教材使用，也可以作为非双语物理化学教学的参考教材。

CONTENTSIntroduction（1）0.1Physical chemistry（1）0.1.1Contents of physical chemistry（1）0.1.2Issues to be solved by physical chemistry（1）0.1.3Advice for studying physical chemistry（2）0.2Indication and operation of physical quantity（3）0.2.1Indication of physical quantity（3）0.2.2Operation of physical quantity（3）Chapter 1The pVT properties of gases（4）1.1State equation of the perfect gas（4）1.1.1Empirical law of gas（4）1.1.2State equation of the perfect gas（5）1.1.3Model of the perfect gas（6）1.2Mixture of the perfect gas（6）1.2.1Composition of perfect gas mixture（6）1.2.2Daltons law of partial pressures（7）1.2.3Amagats law of partial volumes（8）1.2.4Mean molar mass of mixed gas（8）1.3Liquefaction of real gas and critical properties（9）1.3.1Saturated vapor pressure of liquid（9）1.3.2Liquefaction of real gas and critical properties（9）1.4State equations of real gas（10）1.4.1The van der Waals equation（10）1.4.2The virial equation of state（11）1.5The law of corresponding states（11）1.5.1Compression factors（11）1.5.2The law of corresponding states（12）EXERCISES（12）Chapter 2The first law of thermodynamics（14）2.1The basic concept of thermodynamics（14）2.1.1System and surroundings（14）2.1.2Extensive property and intensive property of system（15）2.1.3State and state function of system（15）2.1.4Equilibrium state of thermodynamics（16）2.1.5Process and path（16）2.2The first law of thermodynamics（17）2.2.1Heat（18）2.2.2Work（18）2.2.3Calculation of volume work（19）2.2.4Thermodynamic energy（20）2.2.5The first law of thermodynamics（21）2.3The heat at constant volume, the heat at constant pressure and enthalpy（22）2.3.1The heat at constant volume（22）2.3.2The heat at constant pressure（22）2.3.3Enthalpy（22）2.3.4Hesss Law（23）2.4Heat capacity（24）2.4.1Heat capacity（24）2.4.2Relation between Cp, m and p（25）2.4.3Empirical formula between Cp, m and T（25）2.4.4Relation between Cp, m and CV, m（25）2.4.5Joule experiment（26）2.5Reversible process and equation of adiabatic reversible process of the perfect gas（29）2.5.1Reversible process（29）2.5.2Isothermal reversible process of the perfect gas（29）2.5.3Adiabatic reversible process of the perfect gas（30）2.6Phase transformation process（33）2.6.1Phase and enthalpy of phase transition（33）2.6.2Calculation of ΔH of phase transformation process（33）2.7Standard molar enthalpy of reaction（35）2.7.1Chemical stoichiometric number（35）2.7.2Extent of a reaction（35）2.7.3Molar enthalpy of reaction（36）2.7.4Standard molar enthalpy of reaction（36）2.8Standard molar enthalpy of formation and standard molar enthalpy of combustion（37）2.8.1Standard molar enthalpy of formation（37）2.8.2Standard molar enthalpy of combustion（38）2.8.3The temperature—dependence of ΔrHm(T)—Kirchhoffs formula（39）2.8.4The relation between Qp and QV（40）2.8.5Maximum temperature of explosion and flame reaction（40）2.9Throttling process and JouleThomson effect（41）2.9.1JouleThomson experiment（41）2.9.2Experiment result（41）2.9.3Result analysis（41）2.9.4Characteristics of throttling process（42）2.9.5JouleThomson coefficient（42）EXERCISES（42）Chapter 3The second law of thermodynamics（45）3.1Carnot cycle（45）3.1.1Efficiency of heat engine（45）3.1.2Carnot cycle（46）3.1.3Carnot theorem（47）3.2The second law of thermodynamics（48）3.2.1Spontaneous process（48）3.2.2Statements of the second law of thermodynamics（48）3.2.3Essence of the second law of thermodynamics（49）3.3Entropy and the principle of the increase of entropy（49）3.3.1Entropy（49）3.3.2Clausius inequality（50）3.3.3The principle of the increase of entropy and entropy criterion of equilibrium（50）3.4Calculation of entropy change of system（52）3.4.1Calculation of ΔS of system in simple pVT process（52）3.4.2Calculation of ΔS in phase transformation process（57）3.5The Third law of thermodynamics and calculation of the entropy change of reaction（59）3.5.1The Third law of thermodynamics（59）3.5.2Conventional molar entropy and standard molar entropy（60）3.5.3Calculation of ΔrSm(T)（60）3.6Helmholtz function and Gibbs function（61）3.6.1Helmholtz function（61）3.6.2Helmholtz function criterion（61）3.6.3Gibbs function（62）3.6.4Gibbs function criterion（62）3.7Calculation of ΔA and ΔG（63）3.7.1Simple pVT change process（63）3.7.2Phase transformation process（64）3.7.3Chemical change process（65）3.8The fundamental equation of thermodynamics（67）3.8.1The fundamental equation of thermodynamics（67）3.8.2The relation of characteristic function（67）3.8.3Gibbs-Helmholtz equation（68）3.8.4Maxwells relations（68）3.8.5Thermodynamic equation of state（69）3.9Clapeyron equation（71）3.9.1Condition for phase equilibrium of onecomponent system（71）3.9.2Clapeyron equation（72）3.9.3ClausiusClapeyron equation（72）EXERCISES（75）Chapter 4The thermodynamics of multicomponent systems（78）4.1Mixture and solution（78）4.1.1Composition scale of mixture（78）4.1.2Composition scale of solute B in solution（79）4.2Partial molar quantities（80）4.2.1Definition of partial molar quantity（81）4.2.2Collected formula of partial molar quantity（81）4.2.3GibbsDuhem equation（82）4.2.4Relations among different partial molar quantities（82）4.3Chemical potential（83）4.3.1Definition of chemical potential（83）4.3.2Thermodynamic fundamental equation of multicomponent homogeneous system changing of composition（83）4.3.3Equilibrium criterion of material（84）4.4Chemical potential of gas and fugacity（85）4.4.1Expression of chemical potential of perfect gas（85）4.4.2Expression of chemical potential of real gas and fugacity（86）4.5Raoults Law and Henrys Law（87）4.5.1Gasliquid equilibrium of liquid mixture or solution（87）4.5.2Raoults law（87）4.5.3Henrys law（88）4.6Mixture of ideal liquid（89）4.6.1Definition and features of mixture of ideal liquid（89）4.6.2Chemical potential of arbitrary component in mixture of ideal liquid（89）4.6.3Mixing properties of mixture of ideal liquid（90）4.6.4Gasliquid equilibrium of mixture of ideal liquid（91）4.7Ideal dilute solution（93）4.7.1Definition and gasliquid equilibrium of ideal dilute solution（93）4.7.2Chemical potential of solvent and solute in ideal dilute solution（93）4.7.3Distribution law of ideal dilute solution（95）4.8Colligative properties of ideal dilute solution（96）4.8.1Depression of vapor pressure (vapor pressure of solvent A)（96）4.8.2Depression of freezing point (precipitation of solid pure solvent)（96）4.8.3Elevation of boiling point (solute B: involatile)（97）4.8.4Osmotic pressure（97）4.9Real liquid mixture, real liquid solution and activity（99）4.9.1Positive deviation and negative deviation（99）4.9.2Activity and activity factor（99）EXERCISES（101）Chapter 5Chemical equilibrium（103）5.1Standard equilibrium constant of chemical reaction（103）5.1.1Molar Gibbs function change of chemical reaction（103）5.1.2Definition of standard equilibrium constant of chemical reaction（104）5.2Thermodynamic calculation of standard equilibrium constant（104）5.2.1Calculate ΔrGmT from ΔfGmB,β,T（105）5.2.2Calculate ΔrGmT from ΔfHmB,β,T, ΔcHmB,β,T, SmB,β,T and Cp,mB,β,T（105）5.2.3Calculate ΔrGm(T) from relative reactions（105）5.3Relations between K(T) and T（106）5.3.1Relations between K(T) and T（106）5.3.2Integral formula of Vant Hoff equation（107）5.4Chemical equilibrium of perfect gas mixture reaction（108）5.4.1Expression of standard equilibrium constant（108）5.4.2Other expression of equilibrium constant（109）5.5Chemical equilibrium of real gas mixture reaction（109）5.6Vant Hoff isothermal equation and determination of direction of chemical reaction（110）5.7Calculation of equilibrium conversion of reactant and equilibrium composition of system（113）5.7.1Definition of equilibrium conversion of reactant and equilibrium composition of system（113）5.7.2Calculation of equilibrium conversion of reactant and equilibrium composition of system（113）5.8The response of equilibrium to the conditions（114）5.8.1Temperature（114）5.8.2Pressure（115）5.8.3Inert gas（116）5.8.4Input material ratio（117）5.9Chemical equilibrium of reaction of perfect gas and pure condensed phase（117）5.9.1Expression of standard equilibrium constant（117）5.9.2Dissociation pressure of pure solid compound（118）EXERCISES（119）Chapter 6Phase equilibrium（121）6.1Phase rule（121）6.1.1Basic concepts（121）6.1.2Phase rule（122）6.1.3Application of phase rule（122）6.2p-T graph of onecomponent systems（124）6.2.1pT graph for water（125）6.2.2pT graph for carbon dioxide and supercritical CO2 fluid（126）6.2.3pT graph for sulfur（127）6.3Twocomponent liquidgas phase diagram of liquid full miscible system（127）6.3.1Twocomponent liquidgas phase diagram of ideal liquid mixture（128）6.3.2Twocomponent liquidgas phase diagram of real liquid mixture（131）6.4Twocomponent liquidgas phase diagram of liquid full immiscible and partially miscible system（134）6.4.1Twocomponent boiling pointcomposition diagram of liquid full immiscible system（134）6.4.2Twocomponent boiling pointcomposition diagram of liquid partially miscible system（135）6.5Solidliquid phase diagram of twocomponent system（139）6.5.1Twocomponent solidliquid phase diagram of solid full immiscible system（139）6.5.2Thermal analysis method（140）6.5.3Twocomponent solidliquid phase diagram of condensed system forming compound（141）EXERCISES（148）Chapter 7Electrolyte solution（151）7.1Electrolyte and types of electrolyte（151）7.1.1Definition of electrolyte（151）7.1.2Conducting mechanism of electrolyte solution（152）7.1.3Types of electrolyte（152）7.1.4Faradays Law（152）7.2Transference numbers of ions（153）7.2.1Electromigration（153）7.2.2Transference Numbers of ions（153）7.3Conductance, conductivity and molar conductivity（154）7.3.1Conductance（154）7.3.2Conductivity（154）7.3.3Molar conductivity（155）7.3.4Calculation of conductivity and molar conductivity（155）7.3.5Relationship between κ and c or Λm and c（156）7.3.6Law of the independent migration of ions—Kohlrauschs law（157）7.3.7Application of conductance measurement（158）7.4Mean ionic activity of electrolyte（159）7.4.1Mean ionic activity and mean ionic activity factor（159）7.4.2Ionic strength of electrolyte solution（161）7.5Ionic mutual attraction theory of strong electrolyte and DebyeHückel limiting law（162）7.5.1Ionic atmosphere model（162）7.5.2DebyeHückel limiting law（162）EXERCISES（163）Chapter 8Electrochemical system（165）8.1Cell（165）8.1.1Cell（166）8.1.2Electrode（166）8.1.3Cell diagram, electrode reaction and cell reaction of galvanic cell（166）8.1.4Types of electrodes（167）8.1.5Types of galvanic cells（168）8.2Definition of electromotive force of cell and reversible cell（169）8.2.1Definition of electromotive force of cell（169）8.2.2Reversible cell（169）8.3Electromotive force（170）8.3.1Electromotive force（170）8.3.2Standard electrode potential（171）8.3.3Calculation of EMF（173）8.4Design of galvanic cell（174）8.5Applications of EMF measurements（175）8.5.1Determination of ΔrGm， ΔrHm， ΔrSm， Qr， m for the cell reaction（175）8.5.2Determination of K of reaction（176）8.5.3Determination of solubility product Ksp of insoluble salt（177）8.5.4Determination of mean ionic activity factor γ±（177）8.5.5Determination of pH（178）8.5.6Judgement on the direction of reaction（179）8.6Decomposition voltage（179）8.7Polarization（180）8.7.1Polarization（180）8.7.2Types of polarization（180）8.7.3Polarization curve（181）8.7.4Overpotential（181）8.8Competition of electrode reaction（182）EXERCISES（183）Chapter 9Interface phenomena（185）9.1Surface tension（185）9.1.1Surface tension, Surface work and Surface Gibbs function（185）9.1.2The fundamental equation of thermodynamics of high disperse system（188）9.2Excess pressure of curved liquid surface（189）9.2.1Excess pressure of curved liquid surface—Laplace equation（189）9.2.2Capillary phenomenon（190）9.2.3Saturated vapor pressure of curved liquid surface—Kelvin Equation（190）9.2.4Metastable state and new phase formation（191）9.3Soild Surface（192）9.3.1Adsorption（192）9.3.2Difference between physical adsorption and chemisorption（192）9.3.3Adsorption quantity（193）9.3.4Adsorption curve（193）9.3.5Types of adsorption isotherm（193）9.3.6Theory of Langmuir adsorption of unimolecular layer（193）9.3.7Empirical formula of adsorption—Freundlich formula（195）9.3.8BET adsorption isotherm of polymolecular layer（195）9.4Liquidsolid interface（196）9.4.1Types of wetting（196）9.4.2Contact angle（198）9.5Adsorption phenomenon of solution surface（199）9.5.1Adsorption phenomenon of solution surface（199）9.5.2Gibbs adsorption isotherm（200）9.5.3Surface active agent（201）EXERCISES（202）Chapter 10Chemical kinetics（204）10.1Reaction rates and rate equations of chemical reactions（204）10.1.1Definition of reaction rate（205）10.1.2Elementary reaction and overall reaction（206）10.1.3Rate equation of elementary reaction—law of mass action（207）10.1.4 General form of rate equation, order of reaction（207）10.1.5 Gas phase reaction（208）10.2Integral form of rate equation（209）10.2.1Zerothorder reaction（209）10.2.2 Firstorder reaction（209）10.2.3Secondorder reaction（210）10.2.4nthorder reaction（213）10.3Determination of rate equation（214）10.3.1c~t curve determination（214）10.3.2Determination of the order of reaction（214）10.4Temperature dependence of rate equation， activation energy（215）10.4.1Vant Hoff rule（216）10.4.2Arrhenius equation（216）10.4.3Definition of activation energy and preexponential parameter（217）10.4.4Physical significance of activation energy（218）10.4.5Relationship between the activation energy and the reaction heat（218）10.5Typical complex reactions（219）10.5.1Parallel firstorder reaction（219）10.5.2Reversible firstorder reaction（221）10.5.3Consecutive firstorder reaction（222）10.6Approximation methods of rate equation of complex reaction（223）10.6.1Ratedetermining step method（223）10.6.2Equilibriumstate approximation method（224）10.6.3Steadystate approximation method（224）10.6.4Relation between the activation energy of the overall reaction and the elementary reaction（225）10.7Chain reaction（226）10.7.1Common procedure of chain reaction（226）10.7.2Types of chain reaction（227）10.7.3Rate equation of straight chain reaction（227）10.7.4Chain explosion and explosion limit of chain explosion reaction（228）10.8Simple collision theory of gas reaction（SCT) （229）10.9Transition state theory（231）10.10Photochemistry（233）10.10.1Photon and photochemistry（233）10.10.2The basic laws of photochemistry and quantum yield（234）10.11Catalysts and catalysis（235）10.11.1Definition of catalyst（235）10.11.2Types of catalysis（235）10.11.3General characteristics of catalyst（236）10.11.4Mechanism of the catalyst reaction and the rate constant（236）10.11.5Activation energy of catalytic reaction（236）10.11.6Composition of solid catalysts（237）10.11.7Basic knowledge about catalysts（237）EXERCISES（237）APPENDIXⅠSI units（240）APPENDIX ⅡGreek characters（241）APPENDIX ⅢBasic constants（242）APPENDIX ⅣConversion factor（243）APPENDIX ⅤAtomic weights of the elements（1997) （244）APPENDIX ⅥCritical parameters of substance（246）APPENDIX Ⅶvan der Waals constants of gas（247）APPENDIX ⅧRelation between Cp， m and T（248）APPENDIX ⅨStandard thermodynamic properties at 25℃（standard pressure p=100kPa)（249）APPENDIX ⅩΔcHm of organic compounds at 25℃ （standard pressure p=100kPa)（253）REFERENCE BOOKS（254）