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物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版)

物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版)

出版社:中國(guó)石化出版社出版時(shí)間:2024-07-01
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物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版) 版權(quán)信息

  • ISBN:9787511475220
  • 條形碼:9787511475220 ; 978-7-5114-7522-0
  • 裝幀:平裝-膠訂
  • 冊(cè)數(shù):暫無(wú)
  • 重量:暫無(wú)
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物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版) 本書(shū)特色

采用二維碼,課外拓展資料、部分例題以文件、圖片的方式,對(duì)物理化學(xué)典型題和重點(diǎn)知識(shí)點(diǎn)的講解以視頻方式加入教材

物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版) 內(nèi)容簡(jiǎn)介

本書(shū)是為了適應(yīng)物理化學(xué)雙語(yǔ)教學(xué)這一全新的教學(xué)模式,解決物理化學(xué)雙語(yǔ)教材短缺的問(wèn)題,盡量做到內(nèi)容精練、簡(jiǎn)明易懂,并堅(jiān)持對(duì)每一部分內(nèi)容均采用英、漢雙語(yǔ)進(jìn)行編寫(xiě)。內(nèi)容包括:氣體的pVT性質(zhì);化學(xué)熱力學(xué);多組分系統(tǒng)熱力學(xué);化學(xué)平衡;相平衡;電化學(xué);界面現(xiàn)象;化學(xué)動(dòng)力學(xué)。采用二維碼將課外拓展資料、例題、典型題和重點(diǎn)知識(shí)點(diǎn)的講解以文件、圖片音頻、視頻等形式加入教材,使教材更加生動(dòng)、形象、易于理解,提高使用者的學(xué)習(xí)興趣。本書(shū)既可作為高等院校雙語(yǔ)物理化學(xué)教學(xué)的教材使用,也可以作為非雙語(yǔ)物理化學(xué)教學(xué)的參考教材。

物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版) 目錄

CONTENTS Introduction(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 galva
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物理化學(xué)簡(jiǎn)明雙語(yǔ)教程:英漢對(duì)照(第二版) 作者簡(jiǎn)介

何美,工學(xué)博士。現(xiàn)為沈陽(yáng)化工大學(xué)理學(xué)院副教授。自1999年以來(lái)一直從事《物理化學(xué)》和《結(jié)構(gòu)化學(xué)》的教學(xué)與研究工作。主講本科生的《物理化學(xué)》(省精品課、省一流課)、《物理化學(xué)實(shí)驗(yàn)》(省一流課),教學(xué)過(guò)程采用雙語(yǔ)授課。主編、參編教材5部。
李文澤,博士,沈陽(yáng)化工大學(xué)教授,碩士生導(dǎo)師,東北大學(xué)兼職博士生導(dǎo)師。遼寧省稀土化學(xué)及應(yīng)用重點(diǎn)實(shí)驗(yàn)室科研團(tuán)隊(duì)負(fù)責(zé)人。沈陽(yáng)化工大學(xué)理學(xué)院副院長(zhǎng),沈陽(yáng)化工大學(xué)基礎(chǔ)化學(xué)實(shí)驗(yàn)教學(xué)中心主任,遼寧省化工學(xué)會(huì)理事,遼寧省優(yōu)秀教師。

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