On the thermal decomposition of dimethyl ether

1937 ◽  
Vol 33 ◽  
pp. 756 ◽  
Author(s):  
P. F. Gay ◽  
Morris W. Travers
Keyword(s):  
Thermal Decomposition ◽  
Dimethyl Ether

Influence of Nitric Oxide on the Thermal Decomposition of Dimethyl Ether. Gaseous Catalysis

Nature ◽  
1936 ◽  
Vol 138 (3491) ◽  
pp. 546-547 ◽  
Author(s):  
P. F. GAY ◽  
MORRIS W. TRAVERS
Keyword(s):  
Nitric Oxide ◽  
Thermal Decomposition ◽  
Dimethyl Ether

scholarly journals Roaming radicals in the thermal decomposition of dimethyl ether: Experiment and theory

2011 ◽  
Vol 158 (4) ◽  
pp. 618-632 ◽  
Author(s):  
R. Sivaramakrishnan ◽  
J.V. Michael ◽  
A.F. Wagner ◽  
R. Dawes ◽  
A.W. Jasper ◽  
...  
Keyword(s):  
Thermal Decomposition ◽  
Dimethyl Ether

scholarly journals Thermal Decomposition of Dimethyl Ether in the Presence of Nitrogen Oxide

1976 ◽  
Vol 49 (9) ◽  
pp. 2403-2406
Author(s):  
Kohji Tadasa ◽  
Naomi Imai ◽  
Tetsuo Inaba ◽  
Yutaka Kubokawa
Keyword(s):  
Thermal Decomposition ◽  
Nitrogen Oxide ◽  
Dimethyl Ether

KINETICS AND MECHANISMS OF THE PYROLYSIS OF DIMETHYL ETHER: II. THE REACTION INHIBITED BY NITRIC OXIDE AND PROPYLENE

1963 ◽  
Vol 41 (8) ◽  
pp. 1993-2008 ◽  
Author(s):  
D. J. McKenney ◽  
B. W. Wojciechowski ◽  
K. J. Laidler
Keyword(s):  
Nitric Oxide ◽  
Thermal Decomposition ◽  
Dimethyl Ether ◽  
Chain Process ◽  
Maximal Inhibition ◽  
First Order ◽  
Temperature Range ◽  
Maximum Inhibition ◽  
A Chain

The thermal decomposition of dimethyl ether, inhibited by nitric oxide and by propylene, was studied in the temperature range of 500 to 600 °C. About 1.5 mm of nitric oxide gave maximal inhibition, the rate then being approximately 8% of the uninhibited rate. With propylene, approximately 70 mm gave maximal inhibition, the rate being slightly higher than that using nitric oxide (~12.5% of the uninhibited rate). In both cases the degree of inhibition was independent of the ether pressure. In the maximally inhibited regions both reactions are three-halves order with respect to ether pressure. As the pressure of nitric oxide was increased beyond 10–15 mm, the overall rate increased, and in this region the reaction is first order with respect to both nitric oxide and ether. A 50:50 mixture of CH3OCH3 and CD3OCD3, with enough NO to ensure maximum inhibition, was pyrolyzed. Even at very low percentage decomposition the CD3H/CD4 ratio was approximately the same as that in the uninhibited decomposition, proving that the inhibited reaction is largely a chain process. Detailed inhibition mechanisms are proposed in which the inhibitor is involved both in initiation and termination reactions.

Thermal decomposition reaction and a comprehensive kinetic model of dimethyl ether

2008 ◽  
Vol 40 (1) ◽  
pp. 1-18 ◽  
Author(s):  
Zhenwei Zhao ◽  
Marcos Chaos ◽  
Andrei Kazakov ◽  
Frederick L. Dryer
Keyword(s):  
Thermal Decomposition ◽  
Kinetic Model ◽  
Dimethyl Ether ◽  
Decomposition Reaction

KINETICS AND MECHANISMS OF THE PYROLYSIS OF DIMETHYL ETHER: I. THE UNINHIBITED REACTION

1963 ◽  
Vol 41 (8) ◽  
pp. 1984-1992 ◽  
Author(s):  
D. J. McKenney ◽  
K. J. Laidler
Keyword(s):  
Experimental Study ◽  
Thermal Decomposition ◽  
Kinetic Parameters ◽  
Dimethyl Ether ◽  
Rate Constant ◽  
Hydrogen Sulphide ◽  
Pressure Range ◽  
Significant Contribution ◽  
Surface Effect ◽  
Elementary Processes

An experimental study has been made of the thermal decomposition of dimethyl ether, the temperature range being 500 to 550 °C and the pressure range 100 to 700 mm Hg. A considerable surface effect was noted, and the results were not very reproducible. The reaction was of the three-halves order and the rate constant could be expressed as 2.98 × 1014e−54,900/RT cc1/2 mole−1/2 sec−1. On the basis of the results obtained in the presence of hydrogen sulphide (D. J. McKenney and K. J. Laidler. Can. J. Chem. 41, 2009 (1963)) it is concluded that the initiating step, the dissociation of CH3OCH3 into CH3O and CH3, is in its second-order region. In order for the overall order to be three-halves the main terminating step must be either of the type ββM or βμ. The concentrations of the various radicals, and the rates of the various chain-ending steps, are calculated from known or estimated kinetic parameters for the elementary processes. It is concluded that the predominant chain-ending step is probably CH3 + CH3 + M → C2H6 + N, but that there may be a significant contribution from CH3 + CHO + M → CH3CHO + M and from CH3 + CH2OCH3 + M → C2H5OCH3 + M.

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