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<p><b>Preface xvii</b></p> <p><b>PART 1. BASIC CONCEPTS OF CHEMICAL KINETICS 1</b></p> <p><b>Chapter 1. Chemical Reaction and Kinetic Quantities 3</b></p> <p>1.1. The chemical reaction 3</p> <p>1.2. Homogeneous and heterogeneous reactions 8</p> <p>1.3. Extent and speed of a reaction 9</p> <p>1.4. Volumetric and areal speed of a monozone reaction 12</p> <p>1.5. Fractional extent and rate of a reaction 14</p> <p>1.6. Reaction speeds and concentrations 18</p> <p>1.7. Expression of volumetric speed according to variations in concentration in a closed system 19</p> <p>1.8. Stoichiometric mixtures and progress 20</p> <p>1.9. Factors influencing reaction speeds 21</p> <p><b>Chapter 2. Reaction Mechanisms and Elementary Steps 25</b></p> <p>2.1. Basic premise of kinetics 25</p> <p>2.2. Reaction mechanism 26</p> <p>2.3. Reaction intermediates 29</p> <p>2.4. Reaction sequences and Semenov representation 32</p> <p>2.5. Chain reactions 34</p> <p>2.6. Catalytic reactions 37</p> <p>2.7. Important figures in reaction mechanisms 41</p> <p><b>Chapter 3. Kinetic Properties of Elementary Reactions 43</b></p> <p>3.1. Space function of an elementary reaction 43</p> <p>3.2. Reactivity and rate of an elementary step 44</p> <p>3.3. Kinetic constants of an elementary step 45</p> <p>3.4. Opposite elementary reactions 47</p> <p>3.5. Influence of temperature on the reactivities of elementary steps 49</p> <p>3.6. Modeling of a gas phase elementary step 51</p> <p>3.7. A particular elementary step: diffusion 58</p> <p>3.8. Gases adsorption onto solids 64</p> <p>3.9. Important figures in the kinetic properties of elementary reactions 71</p> <p><b>Chapter 4. Kinetic Data Acquisition 73</b></p> <p>4.1. Experimental kinetic data of a reaction 73</p> <p>4.2. Generalities on measuring methods 74</p> <p>4.3. Chemical methods 74</p> <p>4.4. Physical methods 75</p> <p>4.5. Researching the influence of various variables 87</p> <p><b>Chapter 5. Experimental Laws and Calculation of Kinetic Laws of Homogeneous Systems 91</b></p> <p>5.1. Experimental laws in homogeneous kinetics 91</p> <p>5.2. Relationship between the speed of a reaction and the speeds of its elementary steps 95</p> <p>5.3. Mathematical formulation of speed from a mechanism and experimental conditions 96</p> <p>5.4. Mathematical formulation of a homogeneous reaction with open sequence 99</p> <p>5.5. Mathematical formulation of chain reactions 101</p> <p><b>Chapter 6. Experimental Data and Calculation of Kinetic Laws of Heterogeneous Reactions 109</b></p> <p>6.1. Heterogeneous reactions 109</p> <p>6.2. Experimental kinetic data of heterogeneous reactions 112</p> <p>6.3. Involvement of diffusion in matter balances 119</p> <p>6.4. Example of mathematical formulation of a heterogeneous catalytic reaction 124</p> <p>6.5. Example of the mathematical formulation of an evolution process of a phase 127</p> <p><b>Chapter 7. Pseudo- and Quasi-steady State Modes 135</b></p> <p>7.1. Pseudo-steady state mode 135</p> <p>7.2. Pseudo-steady state sequences with constant volume (or surface) – quasi-steady state 147</p> <p>7.3. Pseudo- and quasi-steady state of diffusion 150</p> <p>7.4. Application to the calculation of speeds in pseudo-steady state or quasi-steady state 151</p> <p>7.5. Pseudo-steady state and open or closed systems 159</p> <p>7.6. Conclusion 162</p> <p>7.7. Important figure in pseudo-steady state 163</p> <p><b>Chapter 8. Modes with Rate-determining Steps 165</b></p> <p>8.1. Mode with one determining step 166</p> <p>8.2. Pseudo-steady state mode with two determining steps 185</p> <p>8.3. Generalization to more than two determining steps 189</p> <p>8.4. Conclusion to the study of modes with one or several rate-determining steps 190</p> <p>8.5. First order mode changes 190</p> <p>8.6. Conclusion 191</p> <p><b>PART 2. REACTION MECHANISMS AND KINETIC PROPERTIES 193</b></p> <p><b>Chapter 9. Establishment and Resolution of a Reaction Mechanism 195</b></p> <p>9.1. Families of reaction mechanisms 195</p> <p>9.2. Different categories of elementary steps 196</p> <p>9.3. Establishment of a reaction mechanism 201</p> <p>9.4. Research into a mechanism: intermediary reactions 205</p> <p>9.5. Back to the modes and laws of kinetics 210</p> <p>9.6. Experimental tests 212</p> <p>9.7. Looking for the type of rate law 218</p> <p><b>Chapter 10. Theory of the Activated Complex in the Gas Phase 223</b></p> <p>10.1. The notion of molecular energy: the energy of a group of atoms 223</p> <p>10.2. Bimolecular reactions in the gas phase 227</p> <p>10.3. Monomolecular reactions in the gas phase 243</p> <p>10.4. Photochemical elementary reactions 248</p> <p>10.5. The theory of activated complexes 252</p> <p><b>Chapter 11. Modeling Elementary Reactions in Condensed Phase 253</b></p> <p>11.1. Elementary reaction in the liquid phase 253</p> <p>11.2. Elementary reaction in the solid state 268</p> <p>11.3. Interphase reactions 276</p> <p>11.4. Electrochemical reactions 280</p> <p>11.5. Conclusion 290</p> <p><b>Chapter 12. The Kinetics of Chain Reactions 291</b></p> <p>12.1. Definition of a chain reaction 291</p> <p>12.2. The kinetic characteristics of chain reactions 292</p> <p>12.3. Classification of chain reactions 293</p> <p>12.4. Chain reaction sequences 295</p> <p>12.5. Kinetic study of straight chain or non-branch chain reactions 299</p> <p>12.6. Kinetic study of chain reactions with direct branching 311</p> <p>12.7. Semenov and the kinetics of chain reactions 321</p> <p><b>Chapter 13. Catalysis and Catalyzed Reactions 323</b></p> <p>13.1. Homogenous catalysis 324</p> <p>13.2. Heterogeneous catalysis reactions 335</p> <p>13.3. Gas–solid reactions leading to a gas 351</p> <p>13.4. Conclusion on catalysis 352</p> <p>13.5. Langmiur and Hinshelwood 352</p> <p><b>Chapter 14. Kinetics of Heterogeneous Stoichiometric Reactions 353</b></p> <p>14.1. Extent versus time and rate versus extent curves 354</p> <p>14.2. The global model with two processes 355</p> <p>14.3. The ?ÖE law 356</p> <p>14.4. Morphological modeling of the growing space function 357</p> <p>14.5. The nucleation process 373</p> <p>14.6. Physico-chemical growth models 384</p> <p>14.7. Conclusion on heterogeneous reactions 386</p> <p>14.8. Important figures in reaction kinetics 387</p> <p><b>Chapter 15. Kinetics of Non-pseudo-steady State Modes 389</b></p> <p>15.1. Partial pseudo-steady state modes 389</p> <p>15.2. The paralinear law of metal oxidation 392</p> <p>15.3. Thermal runaway and ignition of reactions 395</p> <p>15.4. Chemical ignition of gaseous mixtures 397</p> <p><b>APPENDICES 405</b></p> <p>Appendix 1. Point Defects and Structure Elements of Solids 407</p> <p>Appendix 2. Notions of Microscopic Thermodynamics 413</p> <p>Appendix 3. Vibration Frequency of the Activated Complex 425</p> <p>Notations and Symbols 431</p> <p>Bibliography 439</p> <p>Index 441</p>

<p><strong>Michel Soustelle</strong> is a chemical engineer and Emeritus Professor at Ecole des Mines de Saint-Etienne in France. He taught chemical kinetics from postgraduate to Master's levels while also carrying out research in this topic.

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