A Detailed
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about the book  " Introductory Thermodynamics"
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A Detailed
index More
information
about the book "
Introductory Thermodynamics"
|
Activity coefficient and molality 166 coefficient in the concentration scale 168 coefficient of a species in a real solution 153 coefficient using convention I 157 coefficient using convention II 162 effect of pressure and temperature on the — coefficient 155 of a pure condensed phase 125 of a species in a real solution 153 Adiabatic chemical equilibrium of an — isobaric system 121 chemical equilibrium of an — isochoric system 122 closed — system 20, 53, 55 enclosure 2, 16 process 16 reversible process 17 reversible process of an ideal gas 29 Auxiliary functions 39 state variable 3 Azeotropy 158-162 Beau de Rochas cycle 34 Binary mixture 139, 144 system 158 Boiling point — 141, 144 elevation of the — of a solvent in the presence of a solute 150 Bubble point 141 Carnot cycle — 17, 30 reverse — 18 Change isothermal reversible — of a gas 11 of a state variable 5 of the Gibbs energy in a mixture of chemical species 117 of the Gibbs energy with the extent of reaction 117, 118 Characteristic variables 42-46 Châtelier Le —'s principle 135 Chemical conversion of — energy into work 113, 114 independent — reactions 128 reaction 103 Chemical equilibrium effect of an inert gas on a — 137 effect of pressure on a — 136 effect of temperature on a — 136 effect of volume on a — 137 of an adiabatic isobaric system 121 of an adiabatic isochoric system 122 of an isobaric isothermal system 119 of an isothermal isochoric system 120 Chemical potential definition 43 of a multiphase system at equilibrium 90 of a pure condensed phase 125 of a pure ideal gas 69 of a pure liquid 140 of a pure real gas 76 of a real gas in a mixture 83 of a species in a real solution 153 of an ideal gas in an ideal gas mixture 73 of an ideal species 139 of ions in solution 171 reference state — 140, 157, 162, 166, 168 standard — 69, 157, 162, 166, 168 Chemical reaction energetics of —s 103 isothermal and isobaric — 104 system with several —s 131 Clapeyron equations 92 Clausius inequality 22 Clausius-Clapeyron equations 94 Closed adiabatic system 20 system 1, 40-41 system with one chemical reaction, 103 Coefficient activity — and molality 166 activity — and the concentration scale 168 fugacity — of a pure real gas 77 fugacity — of a real gas in a mixture 83 isobaric — of thermal expansion 4 isothermal compressibility — 4 Joule-Thomson — 82 of performance 32 partition — 165 stoichiometric —s 103 thermal expansion — 4 van der Waals —s 79 Combustion internal — engine 34 Components number of — in a system 133 Composition concentration scale, 167 molality scale, 165 mole fraction scale, 61, 72, 140, 153 of the vapor phase of a binary solution 142, 144, 159, 161 Compressibility factor 77, 81 isothermal — coefficient 4 Compression isothermal — of an ideal gas 26 ratio 35 Concentration and composition 167 scale 167 Condensation — 78 curve 142, 144, 158, 161 Condensed phase chemical potential of a pure— 125 Constant Avogadro's — 13 critical —s 79 Henry's — 163 Raoult's — 141 standard equilibrium — 123 thermodynamic equilibrium — 123, 127 volume thermal expansion coefficient 4 Constant pressure process at — 119, 121 Constant volume process at — 40, 120, 122 Continuity of the fluid state 99 Convention for aqueous systems 173 I for the standard state and activity coefficient 157 II for the standard state and activity coefficient 162 relation between — I and II activity coefficients 164 relation between — II and the molality scale 166 sign — for energy exchanges 9 —s for activity coefficients in solutions 153 Conversion of chemical energy into work 113 Corresponding states of real gases 80 Critical constants 79 point 79 temperature 78 Curve condensation — 142, 144, 158, 161 dew point — 142, 144 fusion — 98 inversion — 82 sublimation — 98 vaporization — 98, 141, 144, 161 Cycle Beau de Rochas — 34 Carnot — 17, 30 dithermal — 17 Otto — 34 reverse Carnot — 18 Stirling — 36 Cyclic process 5, 16 Dalton's law 72 Debye-HŸckel theory 171 Degrees of freedom number of — 91, 133 Delay phase change —s 99 Dew point curve 142, 144 Diagram isobaric — for a perfect binary solution 143 isothermal — for a perfect binary solution 141 phase — 98 Diathermal enclosure 2 Differential exact — 6 Differential expression for the enthalpy 43 for the free energy 44 for the free enthalpy 44 for the Gibbs energy 44 for the Gibbs function 44 for the Helmholtz energy 44 for the Helmholtz function 44 for the internal energy 42 of state functions (multiple phases) 89 —s for open systems, 45, 132 Dilute solutions 157, 166, 167 Dissociation equilibrium 172 Dithermal cycle 17 Effect Joule–Thomson — 81 of an inert gas on chemical equilibria 137 of pressure and temperature on the activity coefficient 155 of pressure and volume on entropy at 0 K 101 of pressure on chemical equilibria 136 of pressure on phase equilibrium 92 of temperature on chemical equilibria 136 of temperature on the entropy of reaction 112 of temperature on the Gibbs energy of reaction 112 of temperature on the latent heat 97 of temperature on vapor pressure 97 of volume on chemical equilibria 137 Efficiency of an engine 31, 32 Electrical work 12 Electrode potential and standard entropy of reaction 175 definition 175 Electrolyte chemical potential of ions in solution 171 dissociation 170 Electroneutrality of a solution 170 Elevation of the boiling temperature of a solvent in the presence of a solute 150 Enclosure adiabatic — 2, 16 diathermal — 2 Endothermic reaction 109 Energetics of chemical reactions 103 Energy free — 44 Gibbs — 39 Helmholtz — 39, 44 internal — 15, 42 sign convention for — exchanges 9 various forms of — 13 Enthalpy — 3, 39 explicit expression for the — 62 of an ideal gas mixture 71 of mixing 74, 84, 146 of phase change 94 of reaction 105 standard — of formation 107 Entropy at 0 K 101 definition 19 effect of temperature on the — of reaction 112 evaluating — 100 global — 27, 54 of an ideal gas 70 of mixing 74, 146, 155 of reaction 105 standard — 107 Equation Clapeyron —s 92 Clausius-Clapeyron —s 94 Gibbs-Duhem — 62 Kirchhoff's — 110 van der Waals — of state 78 virial — 77 Equation of state of an ideal gas 50 thermodynamic — 49 van der Waals — 78 Equilibria simultaneous — 132 Equilibrium chemical — displacement laws 135 condition 24, 57 dissociation — 172 effect of an inert gas on a chemical — 137 effect of pressure and temperature on liquid vapor — 146 effect of pressure on a chemical — 136 effect of pressure on phase — 92 effect of temperature on a chemical — 136 effect of volume on a chemical — 137 gas and condensed phase — 94 liquid vapor — 141 of a chemical system 1, 117 of two phases 92 system in a state of — 1 thermal — 1, 2, 24 Equilibrium constant — 123 effect of temperature on the — 134 in heterogeneous systems 126 in solutions 169 in the gas phase 124 in the liquid phase 169 standard — 123 thermodynamic — 123, 127 Euler's identity 59 Eutectic 149 Evaluation of entropies 100 Exact differential 6 Excess entropy of mixing 155 entropy of mixing (gases) 86 Gibbs energy of mixing 154 Gibbs energy of mixing (gases) 85 variable of mixing (gases) 85 variables of mixing 154 Exothermic reaction 109 Expansion isobaric coefficient of thermal — 4 isothermal — of an ideal gas 26 monothermal — of an ideal gas 27 Expression explicit — for enthalpy 62 explicit — for the Gibbs energy 62 explicit — for the Helmholtz energy 62 explicit — for the internal energy 62 of the molar entropy of an ideal gas 70 |
Extensive properties of — variables, 60 variable 2, 39 Extent of reaction — 103 and expression of enthalpy 110 and work 113, 114 change of the Gibbs energy with the — 117, 118 Extraction liquid-liquid — 165 Field magnetic — 13 First law of thermodynamics 15 Fluid continuity of the — state 99 Force external — 9 van der Waals —s 75 work of an external — 9 Formation standard enthalpy of — 107 standard Gibbs energy of — 107 standard variables of — 107 Free energy 3, 39, 44 enthalpy 3, 39 Freezing point lowering by a solute 147 Fuel cell 114 Fugacity and the law of mass action 123 coefficient of a pure real gas 77 definition 76 of a real gas in a mixture 83 Function auxiliary state — 39 homogeneous —s 59 properties of homogeneous —s 59 state — 2, 89 Fusion 98 Gas constant 8 effect of an inert — on vapor pressure 95 equation of state of an ideal — 50 ideal — mixture 70 real —es 75 thermodynamics of —es 69 General process 5, 16 Generalization of Hess' law 108 Gibbs energy — 3, 39, 55 and extent of reaction 117 at 0 K 102 effect of temperature on the — energy 112 excess — of mixing 154 excess — of mixing (gases) 85 explicit expression for the — 62 of a mixture of reactants 117 of formation of hydrogen ions 173 of mixing 74, 146, 154 of mixing in solutions 146 of mixing of real gases 85 of reaction 104, 105 Gibbs function 3, 39 Gibbs-Duhem equation 62 Gibbs-Helmholtz equations 46 Global entropy — 27, 54 and spontaneity 27 Half-cell standard potential 175 Heat — 15 engine 17, 31 pump 31, 34 source 1, 17, 53 system in contact with one — source 17, 53, 55, 119, 120 system in contact with several — sources 22 system in contact with two — sources 17 transfer 24 Heat capacity at constant pressure 41 at constant volume 40 molar — 29 of reaction 105 Helmholtz energy — 3, 39, 44, 53 at 0 K 102 explicit expression for the — 62 of reaction 105 Helmholtz function 3, 39, 44 Henry's constant 163 law 163 Hess' law 108 Heterogeneous system — 1 —s and the law of mass action 126 Homogeneous functions 59 system 1 Hydrogen ion convention for aqueous solutions 173 Ideal gas mixture 70 mixture of gases 86 perfect and — solutions 139-152 species 140 Ideal gas Chemical potential of a pure — 69 definition 50 law of mass action for —es 124 mixture of —es 70 partial pressure of an — 71 Identity Euler's — 59 Implications of the first law 16 of the second law 20 of the third law 101 Independent reactions — 128 and the law of mass action 132 number of — 128 Inert effect of an — gas on chemical equilibria 137 Infinitesimal process 16 Intensive properties of — variables 60 variable 2, 39, 45, 61 Internal energy — 15, 42 differential expression for the — 23 explicit expression for the — 62 expression for the — 23 of an ideal gas mixture 70 of mixing 85 of reaction 105 Inversion curve and temperature 82 Ionic strength 171 Ions chemical potential of — in solutions 171 law of mass action for — 172 Irreversible (real) process 7 process 19 Isenthalpic process 82 Isentropic process 20, 29 Isobaric chemical equilibrium of an adiabatic — system 121 coefficient of thermal expansion 4 diagram 161 diagram for a perfect binary solution 143 equilibrium of an — isothermal system 119 expansivity 4 process 40 Isochoric chemical equilibrium of an adiabatic — system 122 equilibrium of an isothermal — system 120 Isochoric process 40, 120, 122 Isolated system 1 Isothermal compressibility coefficient 4 compression of an ideal gas 26 diagram 141, 158 equilibrium of an isobaric — system 119 equilibrium of an isochoric — system 120 expansion of an ideal gas 26 representation of perfect solution liquid vapor equilibrium 141 reversible process 17 Joule energy unit 15 the — experiment 15 Joule-Thomson coefficient 82 effect 81 Kirchhoff's equation 110 Latent heat effect of temperature on the — 97 of phase change 94 Law Dalton's — 72 displacement —s of equilibria 135 Henry's — 163 Hess' — 108 Raoult's — 141 Law of mass action — 123 for a heterogeneous system 126 for ideal gases 124 for ions 172 in a liquid phase 168 in solutions 168 Law of thermodynamics first — 15 second — 17 third — 101 zeroth — 2 Le Châtelier's principle 135 Lennard-Jones interaction 75 Lever rule 143, 144, 159 Lewis-Randall rule 87 Lowering of the freezing point in the presence of a solute 147 Magnetic field 13 Mass action law of — 123 law of — for a heterogeneous system 126 Maximum amount of work 55, 56, 113 azeotrope 158 entropy 24 extent of reaction 117 Maxwell's relations 46-48 Measurement of partial molar volumes 67 Mechanical equilibrium 1, 89 Mixing enthalpy of — 74, 84, 146 entropy of — 74, 146 excess entropy of — 155 excess variable of — (gases) 85 Gibbs energy of — 74, 146 Internal energy of — 85 irreversible — of two ideal gases 75 properties of ideal solutions 145 variables of — 154 variables of — for ideal gases 74 variables of — for real gases 84 volume of — 145 volume of — of real gases 84 Mixture binary 139, 144 chemical potential of an ideal gas in an ideal gas — 73 fugacity of a real gas in a — 83 ideal gas — 70 ideal — of gases 86 law of mass action for an ideal gas — 123 —s of ideal gases 70 —s of real gases 83 Molality definition 165 scale 165 Molar heat capacity 29 partial — enthalpy of an ideal gas 73 partial — entropy in a solution 155 partial — entropy of an ideal gas 73 partial — quantities 63, 67 partial — volume of an ideal gas 72 properties 65 quantities 65 Molarity 168 Mole fraction 61, 72, 140 Molecular interactions in real gases 75 Monobaric and monothermal process 56 process 41 Monothermal and monobaric process 56 process 17 Natural variables 42 Number of chemical species in a system 91, 133 of components of a system 133 of independent reactions 128 of independent species in a system 133 of phases in a system 91 Open system 42, 90 Osmotic pressure 151 Otto cycle 34 Partial molar enthalpy of an ideal gas 73 entropy in a solution 155 entropy of an ideal gas 73 quantities 63, 67 quantities of pure substances 65 volume of an ideal gas 72 Partial pressure of an ideal gas 71 Partition coefficient 165 Perfect and ideal solutions 139-152 solution 141 Phase change delays 99 chemical potential of a condensed — 125 definition 89 diagram 98 law of mass action in the liquid — 168 number of —s in a system 91 rule 3, 91, 133 rule and electrolytes 170 Physical meaning of the Gibbs function 55 the Helmholtz function 53 Point critical — 79 triple — 19, 99 Potential half-cell standard — 175 reduction — 175 |
Pressure effect of — on chemical equilibria 136 effect of — on the activity coefficient 155 intensive variable 61 osmotic — 151 standard state — 69, 105 Principle Le Châtelier's — 135 Process adiabatic — 16 at constant external pressure 11, 41, 56 at constant pressure 119, 121 at constant volume 40, 120, 122 chemical — 103 cyclic — 5, 16 irreversible — 7, 19 isenthalpic — 82 isentropic — 20, 29 isobaric — 40 isochoric — 40, 120, 122 monobaric — 41 monothermal and monobaric — 56 monothermal — 17 reverse — and work 12 reversible adiabatic — of an ideal gas 29 reversible — 7, 19 spontaneous — 75 Properties of extensive variables 60 of homogeneous functions 59 of intensive variables 60 Pure chemical potential of a — ideal gas 69 chemical potential of a — real gas 76 real gas 75 Rank of a matrix 129 Raoult's constant 141 law 141 Reaction endothermic — 109 exothermic — 109 extent of — 103 independent —s 128 Real mixtures of — gases 83 solution 153 volume of mixing of — gases 84 Real gas fugacity of a — in a mixture 83 partial molar volume of a — 84 pure — 75 Reduced variables 79 Reduction potential 175 Reference state for entropy 101 Refrigerator 31, 33 Relation between activity coefficients in binary systems 160 between Cp and CV 51-52 Maxwell's —s 46-48 —s between partial molar quantities 64 Reverse process and the sign of work 12 Reversible adiabatic process of an ideal gas 29 isothermal expansion or compression of an ideal gas 26 process 7, 19 Rule lever — 143, 144, 159 Lewis-Randall — 87 phase — 3, 91, 133 phase — and electrolytes 170 Schwarz theorem 7, 46, 52 Second law of thermodynamics Spontaneous processes and the — 57 — 17-37 Application to chemical equilibrium 119 Kelvin formulation of the — 17 Selection of the standard state pressure 69 Sign convention for energy exchanges 9 Simultaneous independent — reactions 128 reactions 131 Solute — 147, 162 effect of a — on the boiling temperature 150 freezing point lowering by a — 147 Solution ideal — 140 isothermal diagram 141 non ideal — 153 perfect and ideal — 139-152 perfect — 141 real — 153 Solvent — 147, 162 elevation of the boiling temperature of a — by a solute 150 lowering of the freezing point of a — by a solute 147 Spontaneous evolution of a system 57 process 20, 75 transfer of species between phases 90 Standard chemical potential 69 chemical potential in liquids 157 chemical potential using convention I 157 chemical potential using convention II 163 entropy 107 equilibrium constant 123 Gibbs energy of formation 107 heat capacity at constant pressure 107 molar heat capacity at constant pressure 107 variables of reaction 105 Standard state — 106 of a real gas 76 on the molality scale 166 pressure 69, 105 temperature 105 State corresponding —s of real gases 80 equation of — 8 function 2, 3, 15, 89 standard — 106 standard — and convention I for the activity coefficient 157 standard — and convention II for the activity coefficient 162 variable of — 3 Stirling cycle 36 Stoichiometric coefficients 103 Sublimation 98 System at equilibrium 1 binary — 158 closed adiabatic — 20 closed — 1, 40-41 heterogeneous — 1, 126 heterogeneous — and the law of mass action 126 homogeneous — 1 in contact with one thermal reservoir 17, 21, 53-56 in contact with several thermal reservoirs 22 in contact with two heat sources 17 irreversible process in a — 20 isolated — 1 open — 1, 42-46, 90 without chemical reaction 89 Temperature critical — 78 effect of — on chemical equilibria 136 effect of — on the activity coefficient 155 effect of — on the equilibrium constant 134 inversion — 82 standard state — 105 thermodynamic — 18 Thermal coefficients 4 equilibrium 1, 2 equilibrium and entropy 24 expansion coefficient 4 machines 31 Thermal reservoir definition of a — 1 entropy change of a — 21, 26, 54, 75 system in contact with one — 17, 21, 53 system in contact with several —s 22 Thermodynamic equilibrium constant 123, 127 Thermodynamic temperature 18 Third Law of thermodynamics 101 Transfer heat — 24 spontaneous — of species 90 Triple point 19, 99 Van der Waals coefficients 79 equation of state 78 Vapor pressure — 95, 140 effect of an inert gas on — 95 effect of temperature on — 97 of an ideal solution 141 Vaporization curve 98, 141, 144, 161 Variable auxiliary state — 3, 39 auxiliary — 39 excess — of mixing 154 extensive — 2, 39 intensive — 2, 39 natural —s 42 of mixing 154 of mixing for real gases 84 of reaction 104, 105 of state 3 reduced —s 79 standard —s of formation 107 standard —s of reaction 105 Variance of a system 91, 133 Variation of heat capacities with volume and pressure 52 Virial coefficients and equation 77 Volume effect of — on chemical equilibria 137 of mixing 145 of reaction 105 partial molar — of a real gas 84 partial molar — of an ideal gas 72 work due to — change 10 Work any form of — 113 due to volume change 10 electrical — 12 mechanical — 9 other than volume — 114 sign convention for — 9 various expressions for — 13
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