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An introduction to chemical kinetics
Title statement An introduction to chemical kinetics / Claire Vallance. [elektronický zdroj] Publication San Rafael [California] (40 Oak Drive, San Rafael, CA, 94903, USA) : Morgan & Claypool Publishers, [2017] Distribution Bristol [England] (Temple Circus, Temple Way, Bristol BS1 6HG, UK) : IOP Publishing, [2017] Phys.des. 1 online resource (various pagings) : illustrations (some color). ISBN 9781681746647 (online) 9781681746661 mobi Edition [IOP release 3] IOP concise physics, ISSN 2053-2571 Note "Version: 20170901"--Title page verso. "A Morgan & Claypool publication as part of IOP Concise Physics"--Title page verso. Internal Bibliographies/Indexes Note Includes bibliographical references. Contents Preface -- 1. Elementary reactions -- 1.1. Introduction -- 1.2. Elementary reactions -- 1.3. The rates of elementary reactions : energetic considerations -- 1.4. The rates of elementary reactions : simple collision theory and the Arrhenius equation Content note 2. Rate laws : relating the reaction rate to reactant concentrations -- 2.1. Rate of reaction -- 2.2. Rate laws -- 2.3. The units of the rate constant -- 2.4. Integrated rate laws -- 2.5. Half lives. 3. Determining the rate law and obtaining mechanistic information from experimental data -- 3.1. Isolation method -- 3.2. Differential methods : determining reaction orders from the differential form of the rate law -- 3.3. Integral methods : determining reaction orders from the integrated form of the rate law -- 3.4. Determining orders and rate constants from a half life analysis -- 3.5. Some examples -- 3.6. Exploring the temperature dependence of the rate constant -- 3.7. Summary. 4. Experimental techniques for measuring reaction rates -- 4.1. Techniques for mixing the reactants and initiating reaction -- 4.2. Techniques for monitoring concentrations as a function of time -- 4.3. Temperature control and measurement. 5. Introduction to complex reactions -- 5.1. Consecutive reactions -- 5.2. Pre-equilibria -- 5.3. Moving on to more complicated mechanisms. 6. Using the steady-state approximation to derive rate laws for complex reactions -- 6.1. The steady-state approximation : a first example -- 6.2. The steady-state approximation : a general approach -- 6.3. ‘Unimolecular' reactions : the Lindemann-Hinshelwood mechanism -- 6.4. Third-order reactions -- 6.5. Enzyme reactions and the Michaelis-Menten mechanism. 7. Chain reactions and explosions -- 7.1. Chain reactions -- 7.2. Linear chain reactions -- 7.3. Comparison between the hydrogen-halogen reactions -- 7.4. Explosions and branched chain reactions -- 7.5. Concluding remarks -- 7.6. Further reading. Notes to Availability Přístup pouze pro oprávněné uživatele Audience The book will mainly be of interest to chemistry students, lecturers, tutors, and teachers, either at university level or possibly advanced high school level. It may also be of interest for professionals working in the chemical industry who would like a short, concise text to help them refresh their knowledge of chemical kinetics. Note Způsob přístupu: World Wide Web.. Požadavky na systém: Adobe Acrobat Reader, EPUB reader, or Kindle reader. Another responsib. Morgan & Claypool Publishers, Institute of Physics (Great Britain), Subj. Headings Chemical kinetics. * Chemical physics. * SCIENCE / Chemistry / General. Form, Genre elektronické knihy electronic books Country Kalifornie Language angličtina Document kind Electronic books URL Plný text pro studenty a zaměstnance UPOL 
book
The book is a short primer on chemical reaction rates based on a six-lecture first-year undergraduate course taught by the author at the University of Oxford. The book explores the various factors that determine how fast or slowly a chemical reaction proceeds and describes a variety of experimental methods for measuring reaction rates. The link between the reaction rate and the sequence of steps that makes up the reaction mechanism is also investigated. Chemical reaction rates is a core topic in all undergraduate chemistry courses.
Preface -- 1. Elementary reactions -- 1.1. Introduction -- 1.2. Elementary reactions -- 1.3. The rates of elementary reactions : energetic considerations -- 1.4. The rates of elementary reactions : simple collision theory and the Arrhenius equation2. Rate laws : relating the reaction rate to reactant concentrations -- 2.1. Rate of reaction -- 2.2. Rate laws -- 2.3. The units of the rate constant -- 2.4. Integrated rate laws -- 2.5. Half lives3. Determining the rate law and obtaining mechanistic information from experimental data -- 3.1. Isolation method -- 3.2. Differential methods : determining reaction orders from the differential form of the rate law -- 3.3. Integral methods : determining reaction orders from the integrated form of the rate law -- 3.4. Determining orders and rate constants from a half life analysis -- 3.5. Some examples -- 3.6. Exploring the temperature dependence of the rate constant -- 3.7. Summary4. Experimental techniques for measuring reaction rates -- 4.1. Techniques for mixing the reactants and initiating reaction -- 4.2. Techniques for monitoring concentrations as a function of time -- 4.3. Temperature control and measurement5. Introduction to complex reactions -- 5.1. Consecutive reactions -- 5.2. Pre-equilibria -- 5.3. Moving on to more complicated mechanisms6. Using the steady-state approximation to derive rate laws for complex reactions -- 6.1. The steady-state approximation : a first example -- 6.2. The steady-state approximation : a general approach -- 6.3. ‘Unimolecular' reactions : the Lindemann-Hinshelwood mechanism -- 6.4. Third-order reactions -- 6.5. Enzyme reactions and the Michaelis-Menten mechanism7. Chain reactions and explosions -- 7.1. Chain reactions -- 7.2. Linear chain reactions -- 7.3. Comparison between the hydrogen-halogen reactions -- 7.4. Explosions and branched chain reactions -- 7.5. Concluding remarks -- 7.6. Further reading.
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