Physical Chemistry 3: — Chemical Kinetics — - Christian-Albrechts ...
Physical Chemistry 3: — Chemical Kinetics — - Christian-Albrechts ... Physical Chemistry 3: — Chemical Kinetics — - Christian-Albrechts ...
1.3 Historical events 7 1.4 References Arrhenius 1889 S. A. Arrhenius, Über die Reaktionsgeschwindigkeit bei der Inversion von Rohrzucker durch Säuren, Z.Physik.Chem.4, 226 (1889). Bunker 1966 D. L. Bunker, Theory of Elementary Gas Reaction Rates, Pergamon, Oxford, 1966. Glasstone 1941 S. Glasstone, K. Laidler, H. Eyring, TheTheoryofRateProcesses, Mc Graw-Hill, New York, 1941. Homann 1975 K. H. Homann, Reaktionskinetik, Grundzüge der Physikalischen Chemie Bd. IV, R. Haase (Ed.), Steinkopf, Darmstadt, 1975. Houston 1996 P. L. Houston, Chemical Kinetics and Reaction Dynamics, McGraw- Hill, Boston, 2001. Johnston 1966 H. S. Johnston, Gas Phase Reaction Rate Theory, Ronald,NewYork, 1966. Kassel 1932 L. S. Kassel, The Kinetics of Homogeneous Gas Reactions, Chem.Catalog, New York, 1932. Logan 1996 S. R. Logan, Grundlagen der Chemischen Kinetik, Wiley-VCH, Weinheim, 1996. Pilling 1995 M. J. Pilling, P. W. Seakins, Reaction Kinetics, Oxford University Press, Oxford, 1995. Smith 1980 I. W. M. Smith, Kinetics and Dynamics of Elementary Gas Reactions, Butterworths, London, 1980. Steinfeld 1989 J. I. Steinfeld, J. S. Francisco, W. L. Haase, Chemical Kinetics and Dynamics, Prentice Hall, Englewood Cliffs, 1989.
1.4 References 8 2. Formal kinetics 2.1 Definitions and conventions 2.1.1 The rate of a chemical reaction I Rate of a simple reaction of type A + B → C+D: ≡− A = − B =+ C =+ D = − [A] = − [B] =+ [C] =+ [D] (2.1) (2.2) We will usually write the concentrations of a species A by using square brackets, i.e., [A] and understand that [A] is time dependent, i.e., [A ()]. I Definition of the rate of reaction: 12 Using the standard convention for the signs of the stoichiometric coefficients of the reactants (−1) and products (+1), we write a generic chemical reaction as 1 B 1 + 2 B 2 + → B + +1 B +1 + (2.3) I The progress of the reaction from reactants to products can be described using the reaction progress coordinate : = (2.4) The time dependence leads to the definition of the reaction rate. Definition 2.1: The reaction rate is defined as ≡ 1 (2.5) For the above reaction, therefore, = − 1 1 | 1 | = − 1 2 | 2 | = =+ 1 | | =+ 1 +1 | +1 | = (2.6) I Units: 13 • SI unit for the reaction rate: [] = mol m 3 s (2.7) 12 Reaction rate = Reaktionsgeschwindigkeit. Von manchen Schulen wird auch der Begriff “Reaktionsrate” verwendet. Die bevorzugte “einzig wahre korrekte Übersetzung” wird von der jeweils anderen Seite sehr ernst genommen, allerdings gilt in Kiel in dieser Hinsicht Waffenstillstand. 13 For general information on the SI system see (Mills 1988) or (Homann 1995).
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1.3 Historical events 7<br />
1.4 References<br />
Arrhenius 1889 S. A. Arrhenius, Über die Reaktionsgeschwindigkeit bei der Inversion<br />
von Rohrzucker durch Säuren, Z.Physik.Chem.4, 226 (1889).<br />
Bunker 1966 D. L. Bunker, Theory of Elementary Gas Reaction Rates, Pergamon,<br />
Oxford, 1966.<br />
Glasstone 1941 S. Glasstone, K. Laidler, H. Eyring, TheTheoryofRateProcesses,<br />
Mc Graw-Hill, New York, 1941.<br />
Homann 1975 K. H. Homann, Reaktionskinetik, Grundzüge der Physikalischen<br />
Chemie Bd. IV, R. Haase (Ed.), Steinkopf, Darmstadt, 1975.<br />
Houston 1996 P. L. Houston, <strong>Chemical</strong> <strong>Kinetics</strong> and Reaction Dynamics, McGraw-<br />
Hill, Boston, 2001.<br />
Johnston 1966 H. S. Johnston, Gas Phase Reaction Rate Theory, Ronald,NewYork,<br />
1966.<br />
Kassel 1932 L. S. Kassel, The <strong>Kinetics</strong> of Homogeneous Gas Reactions, Chem.Catalog,<br />
New York, 1932.<br />
Logan 1996 S. R. Logan, Grundlagen der Chemischen Kinetik, Wiley-VCH, Weinheim,<br />
1996.<br />
Pilling 1995 M. J. Pilling, P. W. Seakins, Reaction <strong>Kinetics</strong>, Oxford University Press,<br />
Oxford, 1995.<br />
Smith 1980 I. W. M. Smith, <strong>Kinetics</strong> and Dynamics of Elementary Gas Reactions,<br />
Butterworths, London, 1980.<br />
Steinfeld 1989 J. I. Steinfeld, J. S. Francisco, W. L. Haase, <strong>Chemical</strong> <strong>Kinetics</strong> and<br />
Dynamics, Prentice Hall, Englewood Cliffs, 1989.
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