The range of courses requiring a good basic understanding of chemical kinetics is extensive, ranging from chemical engineers and pharmacists to biochemists and providing the fundamentals in chemistry. Due to the wide reaching nature of the subject readers often struggle to find a book which provides in-depth, comprehensive information without focusing on one specific subject too heavily.
Here Dr Margaret Wright provides an essential introduction to the subject guiding the reader through the basics but then going on to provide a reference which professionals will continue to dip in to through their careers. Through extensive worked examples, Dr Wright, presents the theories as to why and how reactions occur, before examining the physical and chemical requirements for a reaction and the factors which can influence these.
* Carefully structured, each chapter includes learning objectives, summary sections and problems.
* Includes numerous applications to show relevance of kinetics and also provides plenty of worked examples integrated throughout the text.
Rezensionen / Stimmen
"...no other undergraduate kinetics treatment provides such a comprehensive development of the various experimental approaches." (Journal of Chemical Education, January 2005)
Produkt-Info
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Maße
Höhe: 244 mm
Breite: 170 mm
Dicke: 25 mm
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ISBN-13
978-0-470-09059-6 (9780470090596)
Schweitzer Klassifikation
Margaret Robson Wright is the author of Introduction to Chemical Kinetics, published by Wiley.
Autor*in
Formerly of St. Andrews University, UK
Preface.
List of Symbols.
1. Introduction.
2. Experimental Procedures.
2.1 Detection, Identification and Estimation of Concentration of Species Present.
2.2 Measuring the Rate of a Reaction.
2.3 Conventional Methods of Following a Reaction.
2.4 Fast Reactions.
2.5 Relaxation Methods.
2.6 Periodic Relaxation Techniques: Ultrasonics.
2.7 Line Broadening in NMR and ESR Spectra.
3. The Kinetic Analysis of Experimental Data.
3.1 The Experimental Data.
3.2 Dependence of Rate on Concentration.
3.3 Meaning of the Rate Expression.
3.4 Units of the Rate Constant, k.
3.5 The Significance of the Rate Constant as Opposed to the Rate.
3.6 Determining the Order and Rate Constant from Experimental Data.
3.7 Systematic Ways of Finding the Order and Rate Constant from Rate/Concentration Data.
3.8 Drawbacks of the Rate/Concentration Methods of Analysis.
3.9 Integrated Rate Expressions.
3.10 First Order Reactions.
3.11 Second Order Reactions.
3.12 Zero Order Reaction.
3.13 Integrated Rate Expressions for Other Orders.
3.14 Main Features of Integrated Rate Equations.
3.15 Pseudo-order Reactions.
3.16 Determination of the Product Concentration at Various Times.
3.17 Expressing the Rate in Terms of Reactants or Products for Non-simple Stoichiometry.
3.18 The Kinetic Analysis for Complex Reactions.
3.19 The Steady State Assumption.
3.20 General Treatment for Solving Steady States.
3.21 Reversible Reactions.
3.22 Pre-equilibria.
3.23 Dependence of Rate on Temperature.
4. Theories of Chemical Reactions.
4.1 Collision Theory.
4.2 Modified Collision Theory.
4.3 Transition State Theory.
4.4 Thermodynamic Formulations of Transition State Theory.
4.5 Unimolecular Theory.
4.6 The Slater Theory.
5. Potential Energy Surfaces.
5.1 The Symmetrical Potential Energy Barrier.
5.2 The Early Barrier.
5.3 The Late Barrier.
5.4 Types of Elementary Reaction Studied.
5.5 General Features of Early Potential Energy Barriers for Exothermic Reactions.
5.6 General Features of Late Potential Energy Surfaces for Exothermic Reactions.
5.7 Endothermic Reactions.
5.8 Reactions with a Collision Complex and a Potential Energy Well
6. Complex Reactions in the Gas Phase.
6.1 Elementary and Complex Reactions.
6.2 Intermediates in Complex Reactions.
6.3 Experimental Data.
6.4 Mechanistic Analysis of Complex Non-chain Reactions.
6.5 Kinetic Analysis of a Postulated Mechanism: Use of the Steady State Treatment.
6.6 Kinetically Equivalent Mechanisms.
6.7 A Comparison of Steady State Procedures and Equilibrium Conditions in the Reversible Reaction.
6.8 The Use of Photochemistry in Disentangling Complex Mechanisms.
6.9 Chain Reactions.
6.10 Inorganic Chain Mechanisms.
6.11 Steady State Treatments and Possibility of Determination of All the Rate Constants.
6.12 Stylized Mechanisms: A Typical Rice-Herzfeld Mechanism.
6.13 Special Features of the Termination Reactions: Termination at the Surface.
6.14 Explosions.
6.15 Degenerate Branching or Cool Flames.
7. Reactions in Solution.
7.1 The Solvent and its Effect on Reactions in Solution.
7.2 Collision Theory for Reactions in Solution.
7.3 Transition State Theory for Reactions in Solution.
7.4 S61/4 and Pre-exponential A Factors.
7.5 H61/4 Values.
7.6 Change in Volume on Activation, V61/4.
7.7 Terms Contributing to Activation Parameters.
8. Examples of Reactions in Solution.
8.1 Reactions Where More than One Reaction Contributes to the Rate of Removal of Reactant.
8.2 More Complex Kinetic Situations Involving Reactants in Equilibrium with Each Other and Undergoing Reaction.
8.3 Metal Ion Catalysis.
8.4 Other Common Mechanisms.
8.5 Steady States in Solution Reactions.
8.6 Enzyme Kinetics.
Answers to Problems.
List of Specific Reactions.
Index.
