{"product_id":"chemical-thermodynamics-basic-concepts-and-methods-hardback-9780471780151","title":"Chemical Thermodynamics; Basic Concepts and Methods (Hardback) 9780471780151","description":"\u003cfont face=\"Georgia\"\u003e\r\n\u003cp\u003e\u003cfont size=\"6\"\u003eChemical Thermodynamics\u003c\/font\u003e\u003cbr\u003e\r\n\u003cfont size=\"5\"\u003eBasic Concepts and Methods\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\r\n\r\n\r\n\u003cp\u003e\u003cfont size=\"4\"\u003eIrving M. Klotz (Author), Robert M. Rosenberg (Author)\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003e9780471780151, Wiley\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003eHardback, published 24 June 2008\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003e592 pages\u003cbr\u003e24.2 x 16.5 x 3.9 cm, 1.002 kg\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\r\n\r\n\u003cp align=\"justify\"\u003e\u003cem\u003e\u003cfont size=\"3\"\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)\u003c\/font\u003e\u003c\/em\u003e\u003c\/p\u003e\r\n\r\n\u003cp align=\"justify\"\u003e\u003cstrong\u003e\u003cfont size=\"3\"\u003e\u003cul\u003e \u003cli\u003eA completely updated, expanded edition of a longstanding and influential text on chemical thermodynamics\u003c\/li\u003e \u003cli\u003eCovers the logical foundations and interrelationships of thermodynamics and their application to problems that are commonly encountered by the chemist.\u003c\/li\u003e \u003cli\u003eExplanations of abstract concepts in a clear and simple, yet still rigorous fashion\u003c\/li\u003e \u003cli\u003eLogical arrangement of the material to facilitate learning, including worked out examples.\u003c\/li\u003e \u003cli\u003eComputational techniques, graphical, numerical, and analytical, are described fully and are used frequently, both in illustrative and in assigned problems.\u003c\/li\u003e \u003c\/ul\u003e\u003c\/font\u003e\u003c\/strong\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\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\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003eSubject Areas: Chemistry [\u003ca title=\"See our other books on Chemistry\" 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