Kinetics of chemical processes

Boudart M 1968 Kinetics of Chemical Processes (New York Prentioe-Hall)... 

M. Boudart, Kinetics of Chemical Processes, Prentice-Hall, New York, 1968. 

For a complete development of these relationships, see M. Boudart, Kinetics of Chemical Processes. Prentice-Hall, Englewood Cliffs, New Jersey, 1968, pp. 35-46 I. Amdur and G. G. Hammes, Chemical Kinetics, Principles and Selected Topics, McGraw-Hill, New Vbrk, 1966, pp. 43-58 J. W. Moore and R. G. Pearson, Kinetics and Mechanism, John Wiley Sons, New Vbrk, 1981, pp. 159-169 M. M. Kreevoy and D. G. Truhlar, in Investigation ofRates and Mechanisms ofReaction, Techniques of Chemistry, 4th ed., Vol. VT, Part 1, C. F. Bemsscoai, ed., John Wiley Sons, New Ybrk, 1986. 

Boudart, M. Kinetics of Chemical Processes Prentice-Hall Englewood Cliffs, N.J., 1968. 

Morgan, J. J. and Stone, A. T. (1985). Kinetics of chemical processes of importance in lacustrine environments. In Chemical Processes in Lakes" (W. Stumm, ed.). Wiley, New York. 

Chemical dynamics and modeling were identified as important research frontiers in Chapter 4. They are critically important to the materials discussed in this chapter as well. At the molecular scale, important areas of investigation include studies of statistical mechaiucs, molecular and particle dynamics, dependence of molecular motion on intermolecular and interfacial forces, and kinetics of chemical processes and phase changes. 

Biesenherger, J. A., and Sebastian, D. H., Principles of Polymerization Engineering, Wiley 1983. Boudart, Michel, The Kinetics of Chemical Processes, Prentice Hall, 1968. 

Kinetics of chemical processes on well-defined surfaces. 

In this first chapter, we will outline the scope of this book on the kinetics of chemical processes in the solid state. They are often different from the kinetics of processes in fluids because of structural constraints. After a brief historical introduction, typical situations of non-equilibrium crystals will be described. These will illustrate some basic concepts and our approach to understanding solid state kinetics. 

Two reasons are responsible, for the greater complexity of chemical reactions 1) atomic particles change their chemical identity during reaction and 2) rate laws are nonlinear in most cases. Can the kinetic concepts of fluids be used for the kinetics of chemical processes in solids Instead of dealing with the kinetic gas theory, we have to deal with point, defect thermodynamics and point defect motion. Transport theory has to be introduced in an analogous way as in fluid systems, but adapted to the restrictions of the crystalline state. The same is true for (homogeneous) chemical reactions in the solid state. Processes across interfaces are of great... 

There is no generally accepted classification of elementary processes in heterogeneous catalysis. However, names for a few types of elementary processes are generally accepted and terminology for a partial classification [see M. Boudart, Kinetics of Chemical Processes, Chap. 2 (1968)] has received some currency. The particular reactions used below to exemplify this terminology are ones which have been proposed in the literature but some have not been securely established as occurring in nature at any important rate. 

Potential energy surface with a late transition state. (From Boudart, Mv Kinetics of Chemical Processes, Prentice Hall, Englewood Cliffs, NJ, 1968. With permission.)... 

ERTL, G., Kinetics of chemical processes on well-defined surfaces , in ANDERSON, J.R. and BOUDART, M. (editors), Catalysis-Science and Technology, 4, 209-282, Springer-Verlag (1983)... 

M Boudart, Kinetics of chemical processes, Butterworth-Heinemann, Boston, 1991... 

Boudart M, "Kinetics of Chemical Processes ", Prentice-Hall, Englewood, NJ, 1968. 

Kinetics of Chemical Processes, Michel Boudart, Butterworth-Heinmann, London, 1991. 

G. Ertl Kinetics of Chemical Processes on Well-defined Surfaces, in R. H, Anderson, M. Boudart (eds.) Catalysis Science and Technology, vol. 4, Springer-Verlag, Berlin-Heidel-berg-New York 1983, pp. 257 - 282. 

Below are listed general rules on the form of the reaction rate function (M. Boudart, Kinetics of Chemical Processes, Butterworth-Heinemann, 1991, pp. 13-16). The rules are of an approximate nature but are sufficiently general that exceptions to them usually reveal something of interest. It must be stressed that the utility of these rules is their applicabdity to many single reactions. 

Irradiation of water solutions with gamma rays can produce a very active intermediate known as a hydrated electron. This species can react with many different neutral and ionic species in solution. Devise an experiment to check the electrical charge of the hydrated electron. (Problem adapted from M. Boudart, Kinetics of Chemical Processes, Prentice Hall, Englewood Cliffs, NJ, 1968, p. 55.)... 

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