{"product_id":"chemical-thermodynamics-basic-concepts-and-methods-9780471780151","title":"Chemical Thermodynamics Basic Concepts and","description":"\u003cb\u003eBook Synopsis\u003c\/b\u003e\u003cbr\u003eA completely updated, expanded edition of a longstanding and influential text on chemical thermodynamics, this text presents the logical foundations and interrelationships of thermodynamics and its applications to practical problems. It is restricted to classical thermodynamics, thus maintaining a logical unity throughout the book.\u003cbr\u003e\u003cbr\u003e\u003cb\u003eTrade Review\u003c\/b\u003e\u003cbr\u003e\"[This] book is necessary to people working in various field chemistry, biology, geology and materials science.\" (\u003ci\u003eEnvironmental Engineering and Management Journal\u003c\/i\u003e, September\/October 2008)\u003cbr\u003e\u003cbr\u003e\u003cb\u003eTable of Contents\u003c\/b\u003e\u003cbr\u003e\u003cp\u003ePreface xix\u003c\/p\u003e \u003cp\u003e\u003cb\u003e1 Introduction 1\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e1.1 Origins of Chemical Thermodynamics 1\u003c\/p\u003e \u003cp\u003e1.2 Objectives of Chemical Thermodynamics 4\u003c\/p\u003e \u003cp\u003e1.3 Limitations of Classic Thermodynamics 4\u003c\/p\u003e \u003cp\u003eReferences 6\u003c\/p\u003e \u003cp\u003e\u003cb\u003e2 Mathematical Preparation for Thermodynamics 9\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e2.1 Variables of Thermodynamics 10\u003c\/p\u003e \u003cp\u003eExtensive and Intensive Quantities 10\u003c\/p\u003e \u003cp\u003eUnits and Conversion Factors 10\u003c\/p\u003e \u003cp\u003e2.2 Analytic Methods 10\u003c\/p\u003e \u003cp\u003ePartial Differentiation 10\u003c\/p\u003e \u003cp\u003eExact Differentials 15\u003c\/p\u003e \u003cp\u003eHomogeneous Functions 18\u003c\/p\u003e \u003cp\u003eExercises 21\u003c\/p\u003e \u003cp\u003eReferences 27\u003c\/p\u003e \u003cp\u003e\u003cb\u003e3 The First Law of Thermodynamics 29\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e3.1 Definitions 29\u003c\/p\u003e \u003cp\u003eTemperature 31\u003c\/p\u003e \u003cp\u003eWork 33\u003c\/p\u003e \u003cp\u003e3.2 The First Law of Thermodynamics 37\u003c\/p\u003e \u003cp\u003eEnergy 37\u003c\/p\u003e \u003cp\u003eHeat 38\u003c\/p\u003e \u003cp\u003eGeneral Form of the First Law 38\u003c\/p\u003e \u003cp\u003eExercises 40\u003c\/p\u003e \u003cp\u003eReferences 41\u003c\/p\u003e \u003cp\u003e\u003cb\u003e4 Enthalpy, Enthalpy of Reaction, and Heat Capacity 43\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e4.1 Enthalpy 44\u003c\/p\u003e \u003cp\u003eDefinition 44\u003c\/p\u003e \u003cp\u003eRelationship between \u003ci\u003eQ\u003csub\u003eV\u003c\/sub\u003e\u003c\/i\u003e and \u003ci\u003eQ\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e  46\u003c\/p\u003e \u003cp\u003e4.2 Enthalpy of Reactions 47\u003c\/p\u003e \u003cp\u003eDefinitions and Conventions 47\u003c\/p\u003e \u003cp\u003e4.3 Enthalpy as a State Function 52\u003c\/p\u003e \u003cp\u003eEnthalpy of Formation from Enthalpy of Reaction 52\u003c\/p\u003e \u003cp\u003eEnthalpy of Formation from Enthalpy of Combustion 53\u003c\/p\u003e \u003cp\u003eEnthalpy of Transition from Enthalpy of Combustion 53\u003c\/p\u003e \u003cp\u003eEnthalpy of Conformational Transition of a Protein from Indirect Calorimetric Measurements 54\u003c\/p\u003e \u003cp\u003eEnthalpy of Solid-State Reaction from Measurements of Enthalpy of Solution 56\u003c\/p\u003e \u003cp\u003e4.4 Bond Enthalpies 57\u003c\/p\u003e \u003cp\u003eDefinition of Bond Enthalpies 57\u003c\/p\u003e \u003cp\u003eCalculation of Bond Enthalpies 58\u003c\/p\u003e \u003cp\u003eEnthalpy of Reaction from Bond Enthalpies 59\u003c\/p\u003e \u003cp\u003e4.5 Heat Capacity 60\u003c\/p\u003e \u003cp\u003eDefinition 61\u003c\/p\u003e \u003cp\u003eSome Relationships between \u003ci\u003eC\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e and \u003ci\u003eC\u003csub\u003eV\u003c\/sub\u003e\u003c\/i\u003e  62\u003c\/p\u003e \u003cp\u003eHeat Capacities of Gases 64\u003c\/p\u003e \u003cp\u003eHeat Capacities of Solids 67\u003c\/p\u003e \u003cp\u003eHeat Capacities of Liquids 68\u003c\/p\u003e \u003cp\u003eOther Sources of Heat Capacity Data 68\u003c\/p\u003e \u003cp\u003e4.6 Enthalpy of Reaction as a Function of Temperature 68\u003c\/p\u003e \u003cp\u003eAnalytic Method 69\u003c\/p\u003e \u003cp\u003eArithmetic Method 71\u003c\/p\u003e \u003cp\u003eGraphical or Numerical Methods 72\u003c\/p\u003e \u003cp\u003eExercises 72\u003c\/p\u003e \u003cp\u003eReferences 78\u003c\/p\u003e \u003cp\u003e\u003cb\u003e5 Applications of the First Law to Gases 81\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e5.1 Ideal Gases 81\u003c\/p\u003e \u003cp\u003eDefinition 81\u003c\/p\u003e \u003cp\u003eEnthalpy as a Function of Temperature Only 83\u003c\/p\u003e \u003cp\u003eRelationship Between \u003ci\u003eC\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e and \u003ci\u003eC\u003csub\u003eV\u003c\/sub\u003e\u003c\/i\u003e 84\u003c\/p\u003e \u003cp\u003eCalculation of the Thermodynamic Changes in Expansion Processes 84\u003c\/p\u003e \u003cp\u003e5.2 Real Gases 94\u003c\/p\u003e \u003cp\u003eEquations of State 94\u003c\/p\u003e \u003cp\u003eJoule–Thomson Effect 98\u003c\/p\u003e \u003cp\u003eCalculations of Thermodynamic Quantities in Reversible Expansions 102\u003c\/p\u003e \u003cp\u003eExercises 104\u003c\/p\u003e \u003cp\u003eReferences 108\u003c\/p\u003e \u003cp\u003e\u003cb\u003e6 The Second Law of Thermodynamics 111\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e6.1 The Need for a Second Law 111\u003c\/p\u003e \u003cp\u003e6.2 The Nature of the Second Law 112\u003c\/p\u003e \u003cp\u003eNatural Tendencies Toward Equilibrium 112\u003c\/p\u003e \u003cp\u003eStatement of the Second Law 112\u003c\/p\u003e \u003cp\u003eMathematical Counterpart of the Verbal Statement 113\u003c\/p\u003e \u003cp\u003e6.3 The Carnot Cycle 113\u003c\/p\u003e \u003cp\u003eThe Forward Cycle 114\u003c\/p\u003e \u003cp\u003eThe Reverse Cycle 116\u003c\/p\u003e \u003cp\u003eAlternative Statement of the Second Law 117\u003c\/p\u003e \u003cp\u003eCarnot’s Theorem 118\u003c\/p\u003e \u003cp\u003e6.4 The Thermodynamic Temperature Scale 120\u003c\/p\u003e \u003cp\u003e6.5 The Definition of \u003ci\u003eS\u003c\/i\u003e, the Entropy of a System 125\u003c\/p\u003e \u003cp\u003e6.6 The Proof that \u003ci\u003eS\u003c\/i\u003e is a Thermodynamic Property 126\u003c\/p\u003e \u003cp\u003eAny Substance in a Carnot Cycle 126\u003c\/p\u003e \u003cp\u003eAny Substance in Any Reversible Cycle 127\u003c\/p\u003e \u003cp\u003eEntropy S Depends Only on the State of the System 129\u003c\/p\u003e \u003cp\u003e6.7 Entropy Changes in Reversible Processes 130\u003c\/p\u003e \u003cp\u003eGeneral Statement 130\u003c\/p\u003e \u003cp\u003eIsothermal Reversible Changes 130\u003c\/p\u003e \u003cp\u003eAdiabatic Reversible Changes 131\u003c\/p\u003e \u003cp\u003eReversible Phase Transitions 131\u003c\/p\u003e \u003cp\u003eIsobaric Reversible Temperature Changes 132\u003c\/p\u003e \u003cp\u003eIsochoric Reversible Temperature Changes 133\u003c\/p\u003e \u003cp\u003e6.8 Entropy Changes in Irreversible Processes 133\u003c\/p\u003e \u003cp\u003eIrreversible Isothermal Expansion of an Ideal Gas 133\u003c\/p\u003e \u003cp\u003eIrreversible Adiabatic Expansion of an Ideal Gas 135\u003c\/p\u003e \u003cp\u003eIrreversible Flow of Heat from a Higher Temperature to a Lower Temperature 136\u003c\/p\u003e \u003cp\u003eIrreversible Phase Transitions 137\u003c\/p\u003e \u003cp\u003eIrreversible Chemical Reactions 138\u003c\/p\u003e \u003cp\u003eGeneral Statement 139\u003c\/p\u003e \u003cp\u003e6.9 General Equations for the Entropy of Gases 142\u003c\/p\u003e \u003cp\u003eEntropy of the Ideal Gas 142\u003c\/p\u003e \u003cp\u003eEntropy of a Real Gas 143\u003c\/p\u003e \u003cp\u003e6.10 Temperature–Entropy Diagram 144\u003c\/p\u003e \u003cp\u003e6.11 Entropy as an Index of Exhaustion 146\u003c\/p\u003e \u003cp\u003eExercises 150\u003c\/p\u003e \u003cp\u003eReferences 157\u003c\/p\u003e \u003cp\u003e\u003cb\u003e7 Equilibrium and Spontaneity for Systems at Constant Temperature 159\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e7.1 Reversibility, Spontaneity, and Equilibrium 159\u003c\/p\u003e \u003cp\u003eSystems at Constant Temperature and Volume 160\u003c\/p\u003e \u003cp\u003eSystems at Constant Temperature and Pressure 162\u003c\/p\u003e \u003cp\u003eHeat of Reaction as an Approximate Criterion of Spontaneity 164\u003c\/p\u003e \u003cp\u003e7.2 Properties of the Gibbs, Helmholtz, and Planck Functions 165\u003c\/p\u003e \u003cp\u003eThe Functions as Thermodynamic Properties 165\u003c\/p\u003e \u003cp\u003eRelationships among \u003ci\u003eG\u003c\/i\u003e, \u003ci\u003eY\u003c\/i\u003e, and \u003ci\u003eA\u003c\/i\u003e 165\u003c\/p\u003e \u003cp\u003eChanges in the Functions for Isothermal Conditions 165\u003c\/p\u003e \u003cp\u003eEquations for Total Differentials 166\u003c\/p\u003e \u003cp\u003ePressure and Temperature Derivatives of the Functions 167\u003c\/p\u003e \u003cp\u003eEquations Derived from the Reciprocity Relationship 169\u003c\/p\u003e \u003cp\u003e7.3 The Gibbs Function and Chemical Reactions 170\u003c\/p\u003e \u003cp\u003eStandard States 170\u003c\/p\u003e \u003cp\u003e7.4 Pressure and Temperature Dependence of Δ\u003ci\u003eG\u003c\/i\u003e 172\u003c\/p\u003e \u003cp\u003e7.5 Useful Work and the Gibbs and Helmholtz Functions 175\u003c\/p\u003e \u003cp\u003eIsothermal Changes 175\u003c\/p\u003e \u003cp\u003eChanges at Constant Temperature and Pressure 177\u003c\/p\u003e \u003cp\u003eRelationship between Δ\u003ci\u003eH\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e and \u003ci\u003eQ\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e When Useful Work is Performed 178\u003c\/p\u003e \u003cp\u003eApplication to Electrical Work 179\u003c\/p\u003e \u003cp\u003eGibbs–Helmholtz Equation 180\u003c\/p\u003e \u003cp\u003eThe Gibbs Function and Useful Work in Biologic Systems 181\u003c\/p\u003e \u003cp\u003eExercises 185\u003c\/p\u003e \u003cp\u003eReferences 191\u003c\/p\u003e \u003cp\u003e\u003cb\u003e8 Application of the Gibbs Function and the Planck Function to Some Phase Changes 193\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e8.1 Two Phases at Equilibrium as a Function of Pressure and Temperature 193\u003c\/p\u003e \u003cp\u003eClapeyron Equation 194\u003c\/p\u003e \u003cp\u003eClausius–Clapeyron Equation 196\u003c\/p\u003e \u003cp\u003e8.2 The Effect of an Inert Gas on Vapor Pressure 198\u003c\/p\u003e \u003cp\u003eVariable Total Pressure at Constant Temperature 199\u003c\/p\u003e \u003cp\u003eVariable Temperature at Constant Total Pressure 200\u003c\/p\u003e \u003cp\u003e8.3 Temperature Dependence of Enthalpy of Phase Transition 200\u003c\/p\u003e \u003cp\u003e8.4 Calculation of Change in the Gibbs Function for Spontaneous Phase Change 202\u003c\/p\u003e \u003cp\u003eArithmetic Method 202\u003c\/p\u003e \u003cp\u003eAnalytic Method 203\u003c\/p\u003e \u003cp\u003eExercises 205\u003c\/p\u003e \u003cp\u003eReferences 210\u003c\/p\u003e \u003cp\u003e\u003cb\u003e9 Thermodynamics of Systems of Variable Composition 211\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e9.1 State Functions for Systems of Variable Composition 211\u003c\/p\u003e \u003cp\u003e9.2 Criteria of Equilibrium and Spontaneity in Systems of Variable Composition 213\u003c\/p\u003e \u003cp\u003e9.3 Relationships Among Partial Molar Properties of a Single Component 215\u003c\/p\u003e \u003cp\u003e9.4 Relationships Between Partial Molar Quantities of Different Components 216\u003c\/p\u003e \u003cp\u003ePartial Molar Quantities for Pure Phase 218\u003c\/p\u003e \u003cp\u003e9.5 Escaping Tendency 219\u003c\/p\u003e \u003cp\u003eChemical Potential and Escaping Tendency 219\u003c\/p\u003e \u003cp\u003e9.6 Chemical Equilibrium in Systems of Variable Composition 221\u003c\/p\u003e \u003cp\u003eExercises 223\u003c\/p\u003e \u003cp\u003eReference 226\u003c\/p\u003e \u003cp\u003e\u003cb\u003e10 Mixtures of Gases and Equilibrium in Gaseous Mixtures 227\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e10.1 Mixtures of Ideal Gases 227\u003c\/p\u003e \u003cp\u003eThe Entropy and Gibbs Function for Mixing Ideal Gases 228\u003c\/p\u003e \u003cp\u003eThe Chemical Potential of a Component of an Ideal Gas Mixture 230\u003c\/p\u003e \u003cp\u003eChemical Equilibrium in Ideal Gas Mixtures 231\u003c\/p\u003e \u003cp\u003eDependence of \u003ci\u003eK\u003c\/i\u003e on Temperature 232\u003c\/p\u003e \u003cp\u003eComparison of Temperature Dependence of Δ\u003ci\u003eG\u003c\/i\u003e°\u003csub\u003em\u003c\/sub\u003e and ln \u003ci\u003eK\u003c\/i\u003e 234\u003c\/p\u003e \u003cp\u003e10.2 The Fugacity Function of a Pure Real Gas 236\u003c\/p\u003e \u003cp\u003eChange of Fugacity with Pressure 237\u003c\/p\u003e \u003cp\u003eChange of Fugacity with Temperature 238\u003c\/p\u003e \u003cp\u003e10.3 Calculation of the Fugacity of a Real Gas 239\u003c\/p\u003e \u003cp\u003eGraphical or Numerical Methods 240\u003c\/p\u003e \u003cp\u003eAnalytical Methods 244\u003c\/p\u003e \u003cp\u003e10.4 Joule–Thomson Effect for a Van der Waals Gas 247\u003c\/p\u003e \u003cp\u003eApproximate Value of a for a Van der Waals Gas 247\u003c\/p\u003e \u003cp\u003eFugacity at Low Pressures 248\u003c\/p\u003e \u003cp\u003eEnthalpy of a Van der Waals Gas 248\u003c\/p\u003e \u003cp\u003eJoule–Thomson Coefficient 249\u003c\/p\u003e \u003cp\u003e10.5 Mixtures of Real Gases 249\u003c\/p\u003e \u003cp\u003eFugacity of a Component of a Gaseous Solution 250\u003c\/p\u003e \u003cp\u003eApproximate Rule for Solutions of Real Gases 251\u003c\/p\u003e \u003cp\u003eFugacity Coefficients in Gaseous Solutions 251\u003c\/p\u003e \u003cp\u003eEquilibrium Constant and Change in Gibbs Functions and Planck Functions for Reactions of Real Gases 252\u003c\/p\u003e \u003cp\u003eExercises 253\u003c\/p\u003e \u003cp\u003eReferences 256\u003c\/p\u003e \u003cp\u003e\u003cb\u003e11 The Third Law of Thermodynamics 259\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e11.1 Need for the Third Law 259\u003c\/p\u003e \u003cp\u003e11.2 Formulation of the Third Law 260\u003c\/p\u003e \u003cp\u003eNernst Heat Theorem 260\u003c\/p\u003e \u003cp\u003ePlanck’s Formulation 261\u003c\/p\u003e \u003cp\u003eStatement of Lewis and Randall 262\u003c\/p\u003e \u003cp\u003e11.3 Thermodynamic Properties at Absolute Zero 263\u003c\/p\u003e \u003cp\u003eEquivalence of \u003ci\u003eG\u003c\/i\u003e and \u003ci\u003eH\u003c\/i\u003e 263\u003c\/p\u003e \u003cp\u003eΔ\u003ci\u003eC\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e in an Isothermal Chemical Reaction 263\u003c\/p\u003e \u003cp\u003eLimiting Values of \u003ci\u003eC\u003csub\u003eP\u003c\/sub\u003e\u003c\/i\u003e and \u003ci\u003eC\u003c\/i\u003e\u003ci\u003e\u003csub\u003eV\u003c\/sub\u003e\u003c\/i\u003e  264\u003c\/p\u003e \u003cp\u003eTemperature Derivatives of Pressure and Volume 264\u003c\/p\u003e \u003cp\u003e11.4 Entropies at 298 K 265\u003c\/p\u003e \u003cp\u003eTypical Calculations 266\u003c\/p\u003e \u003cp\u003eApparent Exceptions to the Third Law 270\u003c\/p\u003e \u003cp\u003eTabulations of Entropy Values 274\u003c\/p\u003e \u003cp\u003eExercises 277\u003c\/p\u003e \u003cp\u003eReferences 280\u003c\/p\u003e \u003cp\u003e\u003cb\u003e12 Application of the Gibbs Function to Chemical Changes 281\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e12.1 Determination of Δ\u003ci\u003eG\u003c\/i\u003e°\u003csub\u003em\u003c\/sub\u003e from Equilibrium Measurements 281\u003c\/p\u003e \u003cp\u003e12.2 Determination of Δ\u003ci\u003eG\u003c\/i\u003e°\u003csub\u003em\u003c\/sub\u003e from Measurements of Cell potentials 284\u003c\/p\u003e \u003cp\u003e12.3 Calculation of Δ\u003ci\u003eG\u003c\/i\u003e°\u003csub\u003em\u003c\/sub\u003e from Calorimetric Measurements 285\u003c\/p\u003e \u003cp\u003e12.4 Calculation of a Gibbs Function of a Reaction from Standard Gibbs Function of Formation 286\u003c\/p\u003e \u003cp\u003e12.5 Calculation of a Standard Gibbs Function from Standard Entropies and Standard Enthalpies 287\u003c\/p\u003e \u003cp\u003eEnthalpy Calculations 287\u003c\/p\u003e \u003cp\u003eEntropy Calculations 290\u003c\/p\u003e \u003cp\u003eChange in Standard Gibbs Function 290\u003c\/p\u003e \u003cp\u003eExercises 293\u003c\/p\u003e \u003cp\u003eReferences 301\u003c\/p\u003e \u003cp\u003e\u003cb\u003e13 The Phase Rule 303\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e13.1 Derivation of the Phase Rule 303\u003c\/p\u003e \u003cp\u003eNonreacting Systems 304\u003c\/p\u003e \u003cp\u003eReacting Systems 306\u003c\/p\u003e \u003cp\u003e13.2 One-Component Systems 307\u003c\/p\u003e \u003cp\u003e13.3 Two-Component Systems 309\u003c\/p\u003e \u003cp\u003eTwo Phases at Different Pressures 312\u003c\/p\u003e \u003cp\u003ePhase Rule Criterion of Purity 315\u003c\/p\u003e \u003cp\u003eExercises 316\u003c\/p\u003e \u003cp\u003eReferences 316\u003c\/p\u003e \u003cp\u003e\u003cb\u003e14 The Ideal Solution 319\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e14.1 Definition 319\u003c\/p\u003e \u003cp\u003e14.2 Some Consequences of the Definition 321\u003c\/p\u003e \u003cp\u003eVolume Changes 321\u003c\/p\u003e \u003cp\u003eHeat Effects 322\u003c\/p\u003e \u003cp\u003e14.3 Thermodynamics of Transfer of a Component from One Ideal Solution to Another 323\u003c\/p\u003e \u003cp\u003e14.4 Thermodynamics of Mixing 325\u003c\/p\u003e \u003cp\u003e14.5 Equilibrium between a Pure Solid and an Ideal Liquid Solution 327\u003c\/p\u003e \u003cp\u003eChange of Solubility with Pressure at a Fixed Temperature 328\u003c\/p\u003e \u003cp\u003eChange of Solubility with Temperature 329\u003c\/p\u003e \u003cp\u003e14.6 Equilibrium between an Ideal Solid Solution and an Ideal Liquid Solution 332\u003c\/p\u003e \u003cp\u003eComposition of the Two Phases in Equilibrium 332\u003c\/p\u003e \u003cp\u003eTemperature Dependence of the Equilibrium Compositions 333\u003c\/p\u003e \u003cp\u003eExercises 333\u003c\/p\u003e \u003cp\u003eReferences 335\u003c\/p\u003e \u003cp\u003e\u003cb\u003e15 Dilute Solutions of Nonelectrolytes 337\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e15.1 Henry’s Law 337\u003c\/p\u003e \u003cp\u003e15.2 Nernst’s Distribution Law 340\u003c\/p\u003e \u003cp\u003e15.3 Raoult’s Law 341\u003c\/p\u003e \u003cp\u003e15.4 Van’t Hoff’s Law of Osmotic Pressure 344\u003c\/p\u003e \u003cp\u003eOsmotic Work in Biological Systems 349\u003c\/p\u003e \u003cp\u003e15.5 Van’t Hoff’s Law of Freezing-Point Depression and Boiling-Point Elevation 350\u003c\/p\u003e \u003cp\u003eExercises 353\u003c\/p\u003e \u003cp\u003eReferences 355\u003c\/p\u003e \u003cp\u003e\u003cb\u003e16 Activities, Excess Gibbs Functions, and Standard States for Nonelectrolytes 357\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e16.1 Definitions of Activities and Activity Coefficients 358\u003c\/p\u003e \u003cp\u003eActivity 358\u003c\/p\u003e \u003cp\u003eActivity Coefficient 358\u003c\/p\u003e \u003cp\u003e16.2 Choice of Standard States 359\u003c\/p\u003e \u003cp\u003eGases 359\u003c\/p\u003e \u003cp\u003eLiquids and Solids 360\u003c\/p\u003e \u003cp\u003e16.3 Gibbs Function and the Equilibrium Constant in Terms of Activity 365\u003c\/p\u003e \u003cp\u003e16.4 Dependence of Activity on Pressure 367\u003c\/p\u003e \u003cp\u003e16.5 Dependence of Activity on Temperature 368\u003c\/p\u003e \u003cp\u003eStandard Partial Molar Enthalpies 368\u003c\/p\u003e \u003cp\u003eEquation for Temperature Derivative of the Activity 369\u003c\/p\u003e \u003cp\u003e16.6 Standard Entropy 370\u003c\/p\u003e \u003cp\u003e16.7 Deviations from Ideality in Terms of Excess Thermodynamic Functions 373\u003c\/p\u003e \u003cp\u003eRepresentation of G E m as a Function of Composition 374\u003c\/p\u003e \u003cp\u003e16.8 Regular Solutions and Henry’s Law 376\u003c\/p\u003e \u003cp\u003e16.9 Regular Solutions and Limited Miscibility 378\u003c\/p\u003e \u003cp\u003eExercises 381\u003c\/p\u003e \u003cp\u003eReferences 384\u003c\/p\u003e \u003cp\u003e\u003cb\u003e17 Determination of Nonelectrolyte Activities and Excess Gibbs Functions From Experimental Data 385\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e17.1 Activity from Measurements of Vapor Pressure 385\u003c\/p\u003e \u003cp\u003eSolvent 385\u003c\/p\u003e \u003cp\u003eSolute 386\u003c\/p\u003e \u003cp\u003e17.2 Excess Gibbs Function from Measurement of Vapor Pressure 388\u003c\/p\u003e \u003cp\u003e17.3 Activity of a Solute from Distribution between Two Immiscible Solvents 391\u003c\/p\u003e \u003cp\u003e17.4 Activity from Measurement of Cell Potentials 393\u003c\/p\u003e \u003cp\u003e17.5 Determination of the Activity of One Component from the Activity of the Other 397\u003c\/p\u003e \u003cp\u003eCalculation of Activity of Solvent from That of Solute 398\u003c\/p\u003e \u003cp\u003eCalculation of Activity of Solute from That of Solvent 399\u003c\/p\u003e \u003cp\u003e17.6 Measurements of Freezing Points  400\u003c\/p\u003e \u003cp\u003eExercises  401\u003c\/p\u003e \u003cp\u003eReferences 406\u003c\/p\u003e \u003cp\u003e\u003cb\u003e18 Calculation of Partial Molar Quantities and Excess Molar Quantities from Experimental Data: Volume and Enthalpy 407\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e18.1 Partial Molar Quantities by Differentiation of \u003ci\u003eJ\u003c\/i\u003e as a Function of Composition 407\u003c\/p\u003e \u003cp\u003ePartial Molar Volume 409\u003c\/p\u003e \u003cp\u003ePartial Molar Enthalpy 413\u003c\/p\u003e \u003cp\u003eEnthalpies of Mixing 414\u003c\/p\u003e \u003cp\u003eEnthalpies of Dilution 417\u003c\/p\u003e \u003cp\u003e18.2 Partial Molar Quantities of One Component from those of Another Component by Numerical Integration 420\u003c\/p\u003e \u003cp\u003ePartial Molar Volume 421\u003c\/p\u003e \u003cp\u003ePartial Molar Enthalpy 421\u003c\/p\u003e \u003cp\u003e18.3 Analytic Methods for Calculation of Partial Molar Properties 422\u003c\/p\u003e \u003cp\u003ePartial Molar Volume 422\u003c\/p\u003e \u003cp\u003ePartial Molar Enthalpy 423\u003c\/p\u003e \u003cp\u003e18.4 Changes in J for Some Processes in Solutions 423\u003c\/p\u003e \u003cp\u003eTransfer Process 423\u003c\/p\u003e \u003cp\u003eIntegral Process 425\u003c\/p\u003e \u003cp\u003e18.5 Excess Properties: Volume and Enthalpy 426\u003c\/p\u003e \u003cp\u003eExcess Volume 426\u003c\/p\u003e \u003cp\u003eExcess Enthalpy 426\u003c\/p\u003e \u003cp\u003eExercises 427\u003c\/p\u003e \u003cp\u003eReferences 436\u003c\/p\u003e \u003cp\u003e\u003cb\u003e19 Activity, Activity Coefficients, and Osmotic Coefficients of Strong Electrolytes 439\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e19.1 Definitions and Standard states for Dissolved Electrolytes 440\u003c\/p\u003e \u003cp\u003eUni-univalent Electrolytes 440\u003c\/p\u003e \u003cp\u003eMultivalent Electrolytes 443\u003c\/p\u003e \u003cp\u003eMixed Electrolytes 446\u003c\/p\u003e \u003cp\u003e19.2 Determination of Activities of Strong Electrolytes 448\u003c\/p\u003e \u003cp\u003eMeasurement of Cell Potentials 449\u003c\/p\u003e \u003cp\u003eSolubility Measurements 453\u003c\/p\u003e \u003cp\u003eColligative Property Measurement: The Osmotic Coefficient 455\u003c\/p\u003e \u003cp\u003eExtension of Activity Coefficient Data to Additional Temperatures with Enthalpy of Dilution Data 460\u003c\/p\u003e \u003cp\u003e19.3 Activity Coefficients of Some Strong Electrolytes 462\u003c\/p\u003e \u003cp\u003eExperimental Values 462\u003c\/p\u003e \u003cp\u003eTheoretical Correlation 462\u003c\/p\u003e \u003cp\u003eExercises 464\u003c\/p\u003e \u003cp\u003eReferences 470\u003c\/p\u003e \u003cp\u003e\u003cb\u003e20 Changes in Gibbs Function for Processes in Solutions 471\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e20.1 Activity Coefficients of Weak Electrolytes 471\u003c\/p\u003e \u003cp\u003e20.2 Determination of Equilibrium Constants for Dissociation of Weak Electrolytes 472\u003c\/p\u003e \u003cp\u003eFrom Measurements of Cell Potentials 473\u003c\/p\u003e \u003cp\u003eFrom Conductance Measurements 475\u003c\/p\u003e \u003cp\u003e20.3 Some Typical Calculations for Δ\u003csub\u003ef\u003c\/sub\u003e\u003ci\u003eG\u003c\/i\u003e°\u003csub\u003em\u003c\/sub\u003e  480\u003c\/p\u003e \u003cp\u003eStandard Gibbs Function for Formation of Aqueous Solute: HCl 480\u003c\/p\u003e \u003cp\u003eStandard Gibbs Function of Formation of Individual Ions: HCl 482\u003c\/p\u003e \u003cp\u003eStandard Gibbs Function for Formation of Solid Solute in Aqueous Solution 482\u003c\/p\u003e \u003cp\u003eStandard Gibbs Function for Formation of Ion of Weak Electrolyte 484\u003c\/p\u003e \u003cp\u003eStandard Gibbs Function for Formation of Moderately Strong Electrolyte 485\u003c\/p\u003e \u003cp\u003eEffect of Salt Concentration on Geological Equilibrium Involving Water 486\u003c\/p\u003e \u003cp\u003eGeneral Comments 486\u003c\/p\u003e \u003cp\u003e20.4 Entropies of Ions 487\u003c\/p\u003e \u003cp\u003eThe Entropy of an Aqueous Solution of a Salt 488\u003c\/p\u003e \u003cp\u003eEntropy of Formation of Individual Ions 488\u003c\/p\u003e \u003cp\u003eIon Entropies in Thermodynamic Calculations 491\u003c\/p\u003e \u003cp\u003eExercises 491\u003c\/p\u003e \u003cp\u003eReferences 496\u003c\/p\u003e \u003cp\u003e\u003cb\u003e21 Systems Subject to a Gravitational or a Centrifugal Field 499\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e21.1 Dependence of the Gibbs Function on External Field 499\u003c\/p\u003e \u003cp\u003e21.2 System in a Gravitational Field 502\u003c\/p\u003e \u003cp\u003e21.3 System in a Centrifugal Field 505\u003c\/p\u003e \u003cp\u003eExercises 509\u003c\/p\u003e \u003cp\u003eReferences 510\u003c\/p\u003e \u003cp\u003e\u003cb\u003e22 Estimation of Thermodynamic Quantities 511\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e22.1 Empirical Methods 511\u003c\/p\u003e \u003cp\u003eGroup Contribution Method of Andersen, Beyer, Watson, and Yoneda 512\u003c\/p\u003e \u003cp\u003eTypical Examples of Estimating Entropies 516\u003c\/p\u003e \u003cp\u003eOther Methods 522\u003c\/p\u003e \u003cp\u003eAccuracy of the Approximate Methods 522\u003c\/p\u003e \u003cp\u003eEquilibrium in Complex Systems 523\u003c\/p\u003e \u003cp\u003eExercises 523\u003c\/p\u003e \u003cp\u003eReferences 524\u003c\/p\u003e \u003cp\u003e\u003cb\u003e23 Concluding Remarks 527\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003eReferences 529\u003c\/p\u003e \u003cp\u003eAppendix a Practical Mathematical Techniques 531\u003c\/p\u003e \u003cp\u003eA.1 Analytical Methods 531\u003c\/p\u003e \u003cp\u003eLinear Least Squares 531\u003c\/p\u003e \u003cp\u003eNonlinear Least Squares 534\u003c\/p\u003e \u003cp\u003eA.2 Numerical and Graphical Methods 535\u003c\/p\u003e \u003cp\u003eNumerical Differentiation 535\u003c\/p\u003e \u003cp\u003eNumerical Integration 538\u003c\/p\u003e \u003cp\u003eUse of the Digital Computer 540\u003c\/p\u003e \u003cp\u003eGraphical Differentiation 541\u003c\/p\u003e \u003cp\u003eGraphical Integration 542\u003c\/p\u003e \u003cp\u003eExercises 542\u003c\/p\u003e \u003cp\u003eReferences 543\u003c\/p\u003e \u003cp\u003eIndex 545\u003c\/p\u003e","brand":"John Wiley \u0026 Sons Inc","offers":[{"title":"Default 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