Kinetics and Catalysis

Venugopalan M and Veprek S 1983 Kinetics and catalysis in plasma chemistry Top. Curr. Chem 107 1-58... 

M. Grat2el and K. Kalyanasundaram, eds.. Kinetics and Catalysis in Microheterogenous Systems, Marcel Dekker, New York, 1991. 

Panchenkov and Lebedev, Chemical Kinetics and Catalysis, Mir Publishers, 1976. 

Effects of transport processes cannot be ignored in investigations aimed at more fundamental aspects of kinetics and catalysis. The interaction of chemical and physical processes was noticed a long time ago. M. V. Lomonosov mentioned in 1745 ... 

Kinetics and Catalysis in Microheterogeneous Systems, edited by M. Gratzel and K. Kalyanasundaram... 

T.I. Politova, V.A. Sobyanin, and V.D. Belyaev, Ethylene hydrogenation in electrochemical cell with solid proton-conducting electrolyte, Reaction Kinetics and Catalysis Letters 41(2), 321-326 (1990). 

Chemical, Biochemical, and Thermal Engineering Kinetics and Catalysis 2,841... 

Table 2.1. Historical development of kinetics in relation to catalysis. (From R.A. van Santen and J.W. Niemantsverdriet, Chemical Kinetics and Catalysis, Plenum, Ne A/ York, 1995.)...

A reaction at steady state is not in equilibrium. Nor is it a closed system, as it is continuously fed by fresh reactants, which keep the entropy lower than it would be at equilibrium. In this case the deviation from equilibrium is described by the rate of entropy increase, dS/dt, also referred to as entropy production. It can be shown that a reaction at steady state possesses a minimum rate of entropy production, and, when perturbed, it will return to this state, which is dictated by the rate at which reactants are fed to the system [R.A. van Santen and J.W. Niemantsverdriet, Chemical Kinetics and Catalysis (1995), Plenum, New York]. Hence, steady states settle for the smallest deviation from equilibrium possible under the given conditions. Steady state reactions in industry satisfy these conditions and are operated in a regime where linear non-equilibrium thermodynamics holds. Nonlinear non-equilibrium thermodynamics, however, represents a regime where explosions and uncontrolled oscillations may arise. Obviously, industry wants to avoid such situations ... 

We have now expressed liin terms of 2.2 but we still need to determine what A2 is-We can do this by relating the above equation to something known from thermodynamics. If we do so [see, for example, R.A. van Santen and J.W. Niemantsverdriet, Chemical Kinetics and Catalysis (1995), Plenum, New York, or P.W. Atkins, Physical Chemistry (1998) Oxford University Press, Oxford] we find that I2 equals 1/T and that the above quantity is simply the partition function q. For the interested reader we justify choosing 2.2 equal to 1/T in the following section. 

This book is based on courses, which the authors have taught at Lyngby and Eindhoven for many years. For example. Chapters 1-3 form the basis for a mandatory course Kinetics and Catalysis presented in the second year of the Bachelor s curriculum at Eindhoven, while Chapters 4,5 and 8-10 formed the basis for an optional course Introduction to Catalysis. In Lyngby, Chapters 1-7 have been used for an optional course in Chemical Reaction Kinetics and Catalysis in the Master s curriculum. At the end of the book we have added a list of questions for every chapter. 

E.Kh. Enikeev, Development in Kinetics and Catalysis, 10 (1960) Nauka Publ., Moscow, 88 - 113... 

A.M. Panesh and I.A. Myasnikov, Problems of Kinetics and Catalysis, Nauka Publ., Moscow, 14 (1970) 172. 

O. A. Hougen and K. M. Watson, Chemical Process Principles, Part 3, Kinetics and Catalysis, John Wiley, New York, 1947. 

Based on the results obtained in the investigation of the effects of modulation of the electron density by the nuclear vibrations, a lability principle in chemical kinetics and catalysis (electrocatalysis) has been formulated in Ref. 26. This principle is formulated as follows the greater the lability of the electron, transferable atoms or atomic groups with respect to the action of external fields, local vibrations, or fluctuations of the medium polarization, the higher, as a rule, is the transition probability, all other conditions being unchanged. Note that the concept lability is more general than... 

Dvorko and Shilov [Kinetics and Catalysis, 4 (212), 1964] have studied the iodine catalyzed addition of HI to cyclohexene in benzene solution. 

Tuulmets [Kinetics and Catalysis, 5 (59), 1964] has studied the kinetics of the reaction of ethyl magnesium bromide with pinacolin. He used a calorimetric technique to monitor the progress of the reaction. The overall temperature increase of the reaction mixture was less than a degree. Mixture temperatures were determined with a sensitive potentiometer. The data below... 

Mardaleishvilli, Sin-Chou, and Smorodin-skaya [Kinetics and Catalysis, 8 (664), 1967] have studied the catalytic decomposition of ammonia on quartz. The following initial rate data were obtained by these investigators at 951 C... 

The catalytic dehydrochlorination of tetra-chloroethane has been studied by Shvets, Lebedev, and Aver yanov [Kinetics and Catalysis, 10 (28), 1969]. 

Gulyaev and Polak [Kinetics and Catalysis, 6 (352), 1965] have studied the kinetics of the thermal decomposition of methane with a view toward developing a method for the commercial production of acetylene in a plasma jet. The following differential equations represent the time dependence of the concentrations of the major species of interest. 

The following values of the pseudo first-order rate constant /cx have been reported by Subbotin, Antonov, and Etlis [Kinetics and Catalysis, 7 (183), 1966]. 

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