Mechanism of the Pyrolysis of Acetylene

1971 ◽  
Vol 49 (13) ◽  
pp. 2199-2204 ◽  
Author(s):  
M. H. Back
Keyword(s):  
Free Radical ◽  
Chain Mechanism ◽  
Kinetic Characteristics ◽  
Radical Chain ◽  
Temperature Range ◽  
Decomposition Reactions ◽  
Radical Chain Mechanism ◽  
Initiation Reaction ◽  
Kinetics Of ◽  
Subsequent Addition

A free radical chain mechanism is presented to describe the kinetics of the pyrolysis of acetylene over the temperature range 700–2400 °K. The mechanism is based on the following initiation reaction[Formula: see text]and subsequent addition, abstraction, and decomposition reactions of the radicals involved are shown to account for the products observed and for the kinetic characteristics of the reaction.

Metal ion initiated halogenation reaction of N-haloamines

1970 ◽  
Vol 48 (4) ◽  
pp. 544-545 ◽  
Author(s):  
F. Minisci ◽  
G. P. Gardini ◽  
F. Bertini
Keyword(s):  
Free Radical ◽  
Radical Cation ◽  
Chlorine Atom ◽  
Metal Ion ◽  
Chain Mechanism ◽  
Radical Chain ◽  
Radical Chain Mechanism ◽  
Halogenation Reaction ◽  
Amino Radical Cation ◽  
Methyl Heptanoate

The metal ion catalyzed chlorination of 1-chlorobutane, 1-chlorohexane, methyl-pentanoate, and methyl-heptanoate by protonated N-chloroamines proceeds by a free radical chain mechanism and the chain carrying species was shown not to be a chlorine atom, but an amino radical cation.

Catalysis of hydrogen peroxide dceomposition by 2-electron oxidation and reduction

1959 ◽  
Vol 12 (2) ◽  
pp. 147 ◽  
Author(s):  
NK King ◽  
ME Winfield
Keyword(s):  
Hydrogen Peroxide ◽  
Free Radical ◽  
Radical Formation ◽  
Single Electron ◽  
Chain Mechanism ◽  
Radical Chain ◽  
Radical Chain Mechanism ◽  
Free Radical Formation ◽  
Decomposition Of H2o2

A thermodynamical argument is used to support the suggestion made elsewhere that the more common radical chain mechanism for catalysed decomposition of H2O2 need not predominate if the catalyst can readily undergo a reversible 2-electron oxidation. How complete the exclusion of free radical formation may be depends upon the redox characteristics of the catalyst and on whether its oxidation by two single-electron steps is readily reversible along the same path.

Insight into the free-radical chain mechanism of gold-catalyzed hydrocarbon oxidation reactions in the liquid phase

2007 ◽  
Vol 122 (3-4) ◽  
pp. 284-291 ◽  
Author(s):  
Pascal Lignier ◽  
Franck Morfin ◽  
Laurent Piccolo ◽  
Jean-Luc Rousset ◽  
Valérie Caps
Keyword(s):  
Free Radical ◽  
Liquid Phase ◽  
Hydrocarbon Oxidation ◽  
Chain Mechanism ◽  
Oxidation Reactions ◽  
Radical Chain ◽  
Radical Chain Mechanism ◽  
Insight Into

Kinetics of the thermal reactions of ethylene. Part II. Ethylene–ethane mixtures

1968 ◽  
Vol 46 (14) ◽  
pp. 2427-2433 ◽  
Author(s):  
M. L. Boyd ◽  
M. H. Back
Keyword(s):  
Free Radical ◽  
Product Formation ◽  
Radical Chain ◽  
Thermal Reactions ◽  
Temperature Range ◽  
Initiation Step ◽  
Chain Polymerization ◽  
Main Effects ◽  
Kinetics Of ◽  
Simplified Mechanism

Mixtures of ethane and ethylene have been pyrolyzed in the temperature range 563–600 °C and at pressures from 30–60 cm. The products were similar to those obtained from the pyrolysis of ethylene by itself, described m Part I, with a marked increase in the yields of the saturated products. The initial rates of product formation and the dependence of these rates on the concentration of ethane suggest that the initiation step is the same as that proposed in the pyrolysis of ethylene alone, viz.[Formula: see text]and that the reaction[Formula: see text]is not an important source of radicals. A simplified mechanism is outlined to account for the main effects of ethane on the free radical chain polymerization.

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