Page 7 - Physical chemistry eng

vi CONTENTS

5.13 (Supplemental) The Dependence of S on 8.2 The Pressure–Temperature Phase Diagram 184
T and P 117 8.3 The Phase Rule 190
5.14 (Supplemental) The Thermodynamic 8.4 The Pressure–Volume and Pressure–Volume–
Temperature Scale 118 Temperature Phase Diagrams 191
8.5 Providing a Theoretical Basis for the P–T Phase
6 Chemical Equilibrium 125 Diagram 193

6.1 The Gibbs Energy and the Helmholtz Energy 125 8.6 Using the Clausius–Clapeyron Equation to
Calculate Vapor Pressure as a Function of T 194
6.2 The Differential Forms of U, H, A, and G 130
8.7 The Vapor Pressure of a Pure Substance Depends
6.3 The Dependence of the Gibbs and Helmholtz
on the Applied Pressure 196
Energies on P, V, and T 132
8.8 Surface Tension 197
6.4 The Gibbs Energy of a Reaction Mixture 134
8.9 (Supplemental) Chemistry in Supercritical Fluids 201
6.5 The Gibbs Energy of a Gas in a Mixture 135
8.10 (Supplemental) Liquid Crystal Displays 202
6.6 Calculating the Gibbs Energy of Mixing for Ideal
Gases 136
6.7 Calculating ¢G ° R for a Chemical Reaction 138
9 Ideal and Real Solutions 209
6.8 Introducing the Equilibrium Constant for a
Mixture of Ideal Gases 139 9.1 Defining the Ideal Solution 209
6.9 Calculating the Equilibrium Partial Pressures in a 9.2 The Chemical Potential of a Component in the
Mixture of Ideal Gases 141 Gas and Solution Phases 211
6.10 The Variation of K with Temperature 142 9.3 Applying the Ideal Solution Model to Binary
P
Solutions 212
6.11 Equilibria Involving Ideal Gases and Solid or
Liquid Phases 145 9.4 The Temperature–Composition Diagram and
Fractional Distillation 216
6.12 Expressing the Equilibrium Constant in Terms of
Mole Fraction or Molarity 146 9.5 The Gibbs–Duhem Equation 218
6.13 The Dependence of the Extent of Reaction on T 9.6 Colligative Properties 219
and P 147 9.7 The Freezing Point Depression and Boiling Point
6.14 (Supplemental) A Case Study: The Synthesis of Elevation 220
Ammonia 148 9.8 The Osmotic Pressure 222
6.15 (Supplemental) Expressing U and H and Heat 9.9 Real Solutions Exhibit Deviations from
Capacities Solely in Terms of Measurable Raoult’s Law 224
Quantities 153 9.10 The Ideal Dilute Solution 227
6.16 (Supplemental) Measuring ¢G for the Unfolding 9.11 Activities Are Defined with Respect to Standard
of Single RNA Molecules 157 States 229
6.17 (Supplemental) The Role of Mixing in Determining 9.12 Henry’s Law and the Solubility of Gases in
Equilibrium in a Chemical Reaction 158 a Solvent 232
9.13 Chemical Equilibrium in Solutions 233
7 The Properties of Real Gases 165 9.14 Solutions Formed from Partially Miscible
7.1 Real Gases and Ideal Gases 165 Liquids 237
7.2 Equations of State for Real Gases and Their 9.15 The Solid-Solution Equilibrium 238
Range of Applicability 166
7.3 The Compression Factor 170
10 Electrolyte Solutions 243
7.4 The Law of Corresponding States 173
10.1 The Enthalpy, Entropy, and Gibbs Energy of Ion
7.5 Fugacity and the Equilibrium Constant for
Formation in Solutions 243
Real Gases 175
10.2 Understanding the Thermodynamics of Ion
8 Phase Diagrams and the Relative Formation and Solvation 246
10.3 Activities and Activity Coefficients for
Stability of Solids, Liquids, and
Electrolyte Solutions 248
Gases 181
10.4 Calculating g ; Using the Debye–Hückel Theory 250
8.1 What Determines the Relative Stability of the 10.5 Chemical Equilibrium in Electrolyte
Solid, Liquid, and Gas Phases? 181 Solutions 254