THE REACTION OF HYDROGEN ATOMS WITH KETENE

1964 ◽  
Vol 42 (1) ◽  
pp. 1-9 ◽  
Author(s):  
Nick Demchuk ◽  
H. Gesser
Keyword(s):  
Carbon Monoxide ◽  
Gas Phase ◽  
Surface Reaction ◽  
Flow System ◽  
Minor Amount ◽  
Phase Reaction ◽  
Hydrogen Atoms ◽  
A Chain ◽  
Fast Flow ◽  
A Minor

The gas-phase reaction of atomic hydrogen with ketene has been investigated over a temperature range of −130° to 232 °C using a low-pressure, fast-flow system. In most cases methane, carbon monoxide, and ethane were the major products, but trace amounts of glyoxal were also detected. Above −96 °C. considerable evidence exists for the occurrence of a chain reaction carried by HCO radicals. The surface reaction at −196 °C produced methane and glyoxal predominantly with only a minor amount of carbon monoxide.

Reaction of Hydrogen Atoms with Carbon Suboxide

1971 ◽  
Vol 49 (5) ◽  
pp. 803-806 ◽  
Author(s):  
Nick Demchuk ◽  
H. D. Gesser
Keyword(s):  
Gas Phase ◽  
Intermediate Formation ◽  
Phase Reaction ◽  
Hydrogen Atoms ◽  
Chain Reaction ◽  
Carbon Suboxide ◽  
Formyl Radical ◽  
Gas Phase Reaction ◽  
Temperature Range ◽  
A Chain

The gas phase reaction of hydrogen atoms with carbon suboxide was studied over the temperature range of−96 to 235 °C and was found to proceed via a chain reaction. The products found were CH4, CO, CH2CO, C2H6, (CHO)2, and polymer. A mechanism is proposed and the chain reaction is explained by the intermediate formation of ketene and the formyl radical.

Activation energy for the gas phase reaction of hydrogen atoms with carbon monoxide

1973 ◽  
Vol 59 (9) ◽  
pp. 5199-5200 ◽  
Author(s):  
H. Y. Wang ◽  
J. A. Eyre ◽  
Leon M. Dorfman
Keyword(s):  
Activation Energy ◽  
Carbon Monoxide ◽  
Gas Phase ◽  
Phase Reaction ◽  
Hydrogen Atoms ◽  
Gas Phase Reaction

ChemInform Abstract: GAS-PHASE REACTION OF HOT HYDROGEN ATOMS WITH SILANE

1976 ◽  
Vol 7 (39) ◽  
pp. no-no
Author(s):  
B. REIMANN ◽  
P. POTZINGER
Keyword(s):  
Gas Phase ◽  
Phase Reaction ◽  
Hydrogen Atoms ◽  
Gas Phase Reaction

CARBON MONOXIDE CHEMICAL LASER UTILIZING A FAST FLOW SYSTEM

1970 ◽  
Vol 16 (3) ◽  
pp. 117-118 ◽  
Author(s):  
Curt Wittig ◽  
J. C. Hassler ◽  
P. D. Coleman
Keyword(s):  
Carbon Monoxide ◽  
Flow System ◽  
Chemical Laser ◽  
Fast Flow

The Reaction of O3 with CCl2CH2

1973 ◽  
Vol 51 (10) ◽  
pp. 1504-1510 ◽  
Author(s):  
Leslie A. Hull ◽  
I. C. Hisatsune ◽  
Julian Heicklen
Keyword(s):  
Gas Phase ◽  
Infrared Absorption ◽  
Product Formation ◽  
Phase Reaction ◽  
Chain Mechanism ◽  
Rate Law ◽  
Gas Phase Reaction ◽  
Lower Olefin ◽  
Consumption Ratio ◽  
A Chain

The gas-phase reaction of O3 with CCl2CH2 at 25 °C was studied by monitoring O3 consumption by ultraviolet absorption and product formation and olefin consumption by infrared absorption. In the absence or presence of excess N2, and for initial olefin-to-O3 ratios, [CCl2CH2]0/[O3]0, in excess of 20 ([O3]0 ~ 1.0 Torr), the rate law is[Formula: see text]with k = 2.4 × 106 M−2 s−1. At lower olefin-to-O3 ratios, the rate is initially more rapid than predicted by the above equation, but follows the equation after the reaction has proceeded for some time. In the presence of excess O2, the rate is markedly reduced, and the rate law becomes[Formula: see text]with k′ = 2.2 M−1 s−1.The products of the reaction are CCl2O, HCOOH, CH2ClCCl(O), CO, O2, HCl, and presumably H2O. In the absence of O2, the CCl2CH2-to-O3 consumption ratio approaches 2, but the CCl2O produced per O3 consumed is between 0.25 and 0.4. With excess O2, the latter ratio becomes unity, but the CCl2CH2-to-O3 consumed approaches 5.The results are interpreted in terms of a chain mechanism with CCl2O2 as the chain carrier. The mechanism developed explains the main features of the reaction.

THE REACTION OF ACTIVE NITROGEN WITH ETHANOL

1965 ◽  
Vol 43 (4) ◽  
pp. 935-939 ◽  
Author(s):  
P. A. Gartaganis
Keyword(s):  
Flow System ◽  
Methyl Radicals ◽  
Kcal Mole ◽  
Hydrogen Atoms ◽  
Active Nitrogen ◽  
Condensed Discharge ◽  
Preliminary Study ◽  
Fast Flow ◽  
Ethyl Radicals ◽  
Water Hydrogen

The reaction of active nitrogen with ethanol has been investigated in the range 300 to 593 °K using a modified condensed-discharge Wood–Bonhoeffer fast-flow system. The only condensable products found in appreciable amounts were hydrogen cyanide and water. Hydrogen was the main noncondensable product. A very small amount of acetaldehyde was also formed along with traces of ethane, ethylene, methane, acetonitrile, cyanogen, and probably carbon monoxide. The overall activation energy is 3.4 kcal/mole. It is postulated that the mechanism consists of the formation of two fragments NC2H5 and OH, from which the condensable products result as follows:[Formula: see text]A number of products found in trace quantities are produced by concomitant reactions of the hydrogen atoms with methyl radicals, and with ethanol as well as by disproportionation of ethyl radicals to produce ethane and ethylene. A preliminary study of the reaction of active nitrogen with isopropanol indicated that the energy of activation is in line with the energies of activation of methanol and ethanol.

Gas-phase reaction of benzothiophene with hydrogen atoms

1979 ◽  
Vol 44 (19) ◽  
pp. 3321-3323 ◽  
Author(s):  
Nguyen Hieu Hanh ◽  
Junya Nishino ◽  
Muneyoshi Yamada ◽  
Osamu Horie ◽  
Akira Amano
Keyword(s):  
Gas Phase ◽  
Phase Reaction ◽  
Hydrogen Atoms ◽  
Gas Phase Reaction

Oxydation lente du cétène en phase gazeuse. I. Réaction à "hautes températures"

1971 ◽  
Vol 49 (2) ◽  
pp. 294-302 ◽  
Author(s):  
Pierre Michaud ◽  
Cyrias Ouellet
Keyword(s):  
Carbon Dioxide ◽  
Carbon Monoxide ◽  
Gas Phase ◽  
Static Method ◽  
Chain Reaction ◽  
Slow Combustion ◽  
Temperature Ranges ◽  
Higher Temperature ◽  
A Chain ◽  
Two Temperature

The slow combustion of ketene in the gas phase was studied by the static method in a 30 × 4 cm Vycor cylinder between 280 and 500 °C at pressures above 20 mm Hg. Extending the work of Barnard and Kirschner, we have established the existence of two types of slow combustion of ketene corresponding to two temperature ranges. In this first paper, we describe the kinetic and analytical results obtained in the higher temperature range (380–500 °C). The reaction is autocatalytic and shows a low temperature coefficient corresponding to a few kilocalories per mole. The main products are carbon monoxide, formaldehyde, water, and carbon dioxide. No ethylene was detected. We suggest a chain reaction in which formaldehyde is the intermediate responsible for degenerate branching:[Formula: see text]

Absolute rate constants for the gas-phase reaction of the nitrate radical with dimethyl sulfide, nitrogen dioxide, carbon monoxide and a series of alkanes at 298 .+-. 2 K

1986 ◽  
Vol 90 (19) ◽  
pp. 4640-4644 ◽  
Author(s):  
Timothy J. Wallington ◽  
Roger Atkinson ◽  
Arthur M. Winer ◽  
James N. Pitts
Keyword(s):  
Carbon Monoxide ◽  
Nitrogen Dioxide ◽  
Gas Phase ◽  
Rate Constants ◽  
Dimethyl Sulfide ◽  
Nitrate Radical ◽  
Phase Reaction ◽  
Absolute Rate ◽  
Gas Phase Reaction

ChemInform Abstract: GAS-PHASE REACTION OF BENZOTHIOPHENE WITH HYDROGEN ATOMS

1980 ◽  
Vol 11 (4) ◽  
Author(s):  
N. H. HANH ◽  
J. NISHINO ◽  
M. YAMADA ◽  
O. HORIE ◽  
A. AMANO
Keyword(s):  
Gas Phase ◽  
Phase Reaction ◽  
Hydrogen Atoms ◽  
Gas Phase Reaction
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