Physical chemistry : how chemistry works /: how chemistry works. (2016)

• Record Type: Book
• Further Information: Note: Kurt W. Kolasinski.
• Authors: Kolasinski, Kurt W
• Contents: Preface xv About the companion website xvii 1 Introduction 1 1.1 Atoms and molecules 1 1.2 Phases 2 1.3 Energy 3 1.4 Chemical reactions 4 1.5 Problem solving 5 1.6 Some conventions 7 Exercises 11 Further reading 14 2 Ideal gases 15 2.1 Ideal gas equation of state 16 2.2 Molecular degrees of freedom 18 2.3 Translational energy: Distribution and relation to pressure 21 2.4 Maxwell distribution of molecular speeds 23 2.5 Principle of equipartition of energy 24 2.6 Temperature and the zeroth law of thermodynamics 25 2.7 Mixtures of gases 27 2.8 Molecular collisions 27 Exercises 29 Further reading 30 3 Non-ideal gases and intermolecular interactions 31 3.1 Non-ideal behavior 31 3.2 Interactions of matter with matter 32 3.3 Intermolecular interactions 34 3.4 Real gases 39 3.5 Corresponding states 42 3.6 Supercritical fluids 43 Exercises 43 Further reading 44 4 Liquids, liquid crystals, and ionic liquids 45 4.1 Liquid formation 45 4.2 Properties of liquids 45 4.3 Intermolecular interaction in liquids 47 4.4 Structure of liquids 50 4.5 Internal energy and equation of state of a rigid sphere liquid 52 4.6 Concentration units 53 4.7 Diffusion 55 4.8 Viscosity 57 4.9 Migration 59 4.10 Interface formation 60 4.11 Liquid crystals 62 4.12 Ionic liquids 64 Exercises 66 Further reading 67 5 Solids, nanoparticles, and interfaces 68 5.1 Solid formation 68 5.2 Electronic structure of solids 70 5.3 Geometrical structure of solids 72 5.4 Interface formation 76 5.5 Glass formation 78 5.6 Clusters and nanoparticles 78 5.7 The carbon family: Diamond, graphite, graphene, fullerenes, and carbon nanotubes 80 5.8 Porous solids 83 5.9 Polymers and macromolecules 84 Exercises 86 Endnotes 86 Further reading 86 6 Statistical mechanics 87 6.1 The initial state of the universe 88 6.2 Microstates and macrostates of molecules 89 6.3 The connection of entropy to microstates 91 6.4 The constant : Introducing the partition function 93 6.5 Using the partition function to derive thermodynamic functions 94 6.6 Distribution functions for gases 96 6.7 Quantum statistics for particle distributions 98 6.8 The Maxwell–Boltzmann speed distribution 102 6.9 Derivation of the ideal gas law 103 6.10 Deriving the Sackur–Tetrode equation for entropy of a monatomic gas 104 6.11 The partition function of a diatomic molecule 106 6.12 Contributions of each degree of freedom to thermodynamic functions 106 6.13 The total partition function and thermodynamic functions 111 6.14 Polyatomic molecules 113 Exercises 115 Endnotes 116 Further reading 116 7 First law of thermodynamics 117 7.1 Some definitions and fundamental concepts in thermodynamics 118 7.2 Laws of thermodynamics 118 7.3 Internal energy and the first law 119 7.4 Work 121 7.5 Intensive and extensive variables 123 7.6 Heat 124 7.7 Non-ideal behavior changes the work 125 7.8 Heat capacity 126 7.9 Temperature dependence of Cp 127 7.10 Internal energy change at constant volume 129 7.11 Enthalpy 130 7.12 Relationship between CV and Cp and partial differentials 131 7.13 Reversible adiabatic expansion/compression 133 Exercises 136 Endnotes 138 Further reading 138 8 Second law of thermodynamics 139 8.1 The second law of thermodynamics 140 8.2 Thermodynamics of a hurricane 141 8.3 Heat engines, refrigeration, and heat pumps 145 8.4 Definition of entropy 148 8.5 Calculating changes in entropy 150 8.6 Maxwell’s relations 152 8.7 Calculating the natural direction of change 154 Exercises 157 Endnotes 159 Further reading 159 9 Third law of thermodynamics and temperature dependence of heat capacity, enthalpy and entropy 160 9.1 When and why does a system change? 160 9.2 Natural variables of internal energy 161 9.3 Helmholtz and Gibbs energies 162 9.4 Standard molar Gibbs energies 163 9.5 Properties of the Gibbs energy 164 9.6 The temperature dependence of ΔrCp and H 168 9.7 Third law of thermodynamics 170 9.8 The unattainability of absolute zero 171 9.9 Absolute entropies 172 9.10 Entropy changes in chemical reactions 173 9.11 Calculating ΔrS◦ at any temperature 175 Exercises 177 Further reading 180 10 Thermochemistry: The role of heat in chemical and physical changes 181 10.1 Stoichiometry and extent of reaction 181 10.2 Standard enthalpy change 182 10.3 Calorimetry 184 10.4 Phase transitions 187 10.5 Bond dissociation and atomization 190 10.6 Solution 191 10.7 Enthalpy of formation 192 10.8 Hess’s law 192 10.9 Reaction enthalpy from enthalpies of formation 193 10.10 Calculating enthalpy of reaction from enthalpies of combustion 194 10.11 The magnitude of reaction enthalpy 195 Exercises 196 Further reading 200 11 Chemical equilibrium 201 11.1 Chemical potential and Gibbs energy of a reaction mixture 201 11.2 The Gibbs energy and equilibrium composition 202 11.3 The response of equilibria to change 204 11.4 Equilibrium constants and associated calculations 209 11.5 Acid–base equilibria 212 11.6 Dissolution and precipitation of salts 216 11.7 Formation constants of complexes 219 11.8 Thermodynamics of self-assembly 222 Exercises 224 Endnote 228 Further reading 228 12 Phase stability and phase transitions 229 12.1 Phase diagrams and the relative stability of solids, liquids, and gases 229 12.2 What determines relative phase stability? 232 12.3 The p–T phase diagram 234 12.4 The Gibbs phase rule 237 12.5 Theoretical basis for the p–T phase diagram 238 12.6 Clausius–Clapeyron equation 240 12.7 Surface tension 242 12.8 Nucleation 246 12.9 Construction of a liquid–vapor phase diagram at constant pressure 250 12.10 Polymers: Phase separation and the glass transition 252 Exercises 254 Endnotes 255 Further reading 256 13 Solutions and mixtures: Nonelectrolytes 257 13.1 Ideal solution and the standard state 258 13.2 Partial molar volume 258 13.3 Partial molar Gibbs energy = chemical potential 259 13.4 The chemical potential of a mixture and ΔmixG 261 13.5 Activity 263 13.6 Measurement of activity 264 13.7 Classes of solutions and their properties 269 13.8 Colligative properties 273 13.9 Solubility of polymers 277 13.10 Supercritical CO2 279 Exercises 281 Endnote 282 Further reading 282 14 Solutions of electrolytes 283 14.1 Why salts dissolve 283 14.2 Ions in solution 284 14.3 The thermodynamic properties of ions in solution 287 14.4 The activity of ions in solution 289 14.5 Debye–Hu¨ ckel theory 290 14.6
• Edition: 1st
• Publisher Details: Hoboken, New Jersey : John Wiley & Sons, Inc
• Publication Date: 2016
• Extent: 1 online resource, illustrations
• Subjects: 541; Chemistry, Physical and theoretical
• Languages: English
• ISBNs: 9781118751206; 9781118751213
• Related ISBNs: 9781118751121
• Notes: Note: Description based on CIP data; item not viewed.
• Access Rights: Legal Deposit; Only available on premises controlled by the deposit library and to one user at any one time; The Legal Deposit Libraries (Non-Print Works) Regulations (UK).
• Access Usage: Restricted: Printing from this resource is governed by The Legal Deposit Libraries (Non-Print Works) Regulations (UK) and UK copyright law currently in force.