ON A SINGLE CHAIN MECHANISM FOR THE THERMAL DECOMPOSITION OF HYDROCARBONS

1967 ◽  
pp. 171-175
Author(s):  
V.A. POLTORAK ◽  
V.V. VOEVODSKY
Keyword(s):  
Thermal Decomposition ◽  
Chain Mechanism ◽  
Single Chain ◽  
Decomposition Of Hydrocarbons

scholarly journals Reaction chains in the thermal decomposition of hydrocarbons. A comparison of methane, ethane, propane and hexane

1938 ◽  
Vol 167 (931) ◽  
pp. 447-455 ◽  
Author(s):  
J. E. Hobbs ◽  
Cyril Norman Hinshelwood
Keyword(s):  
Nitric Oxide ◽  
Thermal Decomposition ◽  
Chain Length ◽  
Homologous Series ◽  
Normal Rate ◽  
Chain Mechanism ◽  
Reaction Proceeds ◽  
Decomposition Of Hydrocarbons ◽  
A Chain

The inhibition by nitric oxide of the thermal decomposition of ethane at 600° shows that the reaction proceeds partly by a chain mechanism, the apparent chain length, as measured by the ratio of the normal rate to that of the chain-free reaction, being of the order 5-15 over the range of pressure 50-500 mm., and falling with increasing pressure (Staveley 1937; Hobbs and Hinshelwood 1938). In passing up a homologous series of compounds the chain length may rise or fall. With the series of ethers, for examples, it decreases rapidly, whereas with the aldehydes it increases (Staveley and Hinshelwood 1937).

scholarly journals Thermal decomposition of ammonia. N2H4-an intermediate reaction product

2006 ◽  
Vol 4 (4) ◽  
pp. 666-673 ◽  
Author(s):  
Daniela Dirtu ◽  
Lucia Odochian ◽  
Aurel Pui ◽  
Ionel Humelnicu
Keyword(s):  
Thermal Decomposition ◽  
Chain Mechanism ◽  
Dynamic Conditions ◽  
Intermediate Reaction ◽  
Ft Ir ◽  
Branched Chain

AbstractThe paper reports the thermal decomposition of ammonia under dynamic conditions at 800°C in a quartz reactor. Its purpose is to confirm the homogeneous-heterogeneous degenerated branched chain mechanism established in previous studies, which assume the formation of N2H4 as a molecular intermediate; this paper identifies hydrazine as a product of thermal decomposition using FT-IR and UV-VIS spectroscopies.

The thermal decomposition of n-propyl bromide

1968 ◽  
Vol 21 (4) ◽  
pp. 973 ◽  
Author(s):  
JTD Cross ◽  
VR Stimson
Keyword(s):  
Thermal Decomposition ◽  
Rate Constant ◽  
Hydrogen Bromide ◽  
Bromine Atom ◽  
Order Reaction ◽  
Chain Mechanism ◽  
Initial Concentration ◽  
First Order ◽  
Reaction Proceeds ◽  
Atom Chain

Mechanisms already proposed or formally possible for the decomposition of n-propyl bromide as a 312-order reaction are shown to be unsatisfactory, and the reaction has been reinvestigated. Two reactions occur simultaneously: (a) a first-order reaction identifiable with the maximally inhibited reaction and presumably molecular; (b) a reaction second order in the initial concentration and somewhat autocatalysed as the reaction proceeds. The rate constant is given by k2 == 1018.1exp(-49300/RT)sec-1ml mole-1 Reaction (b) is catalysed by hydrogen bromide and inhibited by propene, and a bromine atom chain mechanism with hydrogen bromide catalysed initiation is proposed. Bromine-catalysed decomposition has also been studied. The mechanism of the inhibition is discussed.

scholarly journals The thermal decomposition of acetaldehyde

1935 ◽  
Vol 149 (867) ◽  
pp. 355-359 ◽  
Keyword(s):  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Condensation Reaction ◽  
Pressure Increase ◽  
Chain Mechanism ◽  
Vessel Size ◽  
Previous Evidence ◽  
Gaseous Products ◽  
A Chain ◽  
Effect Of Surface

This paper contains a more detailed study than has hitherto been made of the effect of surface and vessel size on the thermal decomposition of acetaldehyde. This was desirable in view of the suggestion recently made that the reaction might take place by a chain mechanism, and also because the validity of the previous evidence that the reaction is homogeneous has been called in question. In an unpacked silica between 500° and 600° the reaction is attended by a pressure increase which is about 98% of that corresponding to the equation CH 3 CHO = CH 4 + CO, and the gaseous products consists of equal parts of carbon monoxide and methane. When a packed vessel with very large surface is used the pressure increase is rather less than the theoretical, indicating that some condensation reaction occurs which is probably heterogeneous in contrast with the principal decomposition.

The thermal decomposition of trimethylacetyl bromide

1970 ◽  
Vol 23 (3) ◽  
pp. 525 ◽  
Author(s):  
BS Lennon ◽  
VR Stimson
Keyword(s):  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Hydrogen Bromide ◽  
Transition States ◽  
Volume Ratio ◽  
Reaction Vessel ◽  
Chain Mechanism ◽  
Radical Chain ◽  
First Order ◽  
Polar Transition

Trimethylacetyl bromide decomposes at 298-364� into isobutene, carbon monoxide, and hydrogen bromide in a first-order manner with rate given by k1 = 138 x 1014exp(-48920/RT) sec-1 The rate is unaffected by addition of the products or of inhibitors, or by increase of the surface/volume ratio of the reaction vessel. The likely radical chain mechanism is considered and rejected. The reaction is believed to be a molecular one, and possible cyclic and polar transition states are discussed.

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