Rate of Reaction of OH with HCN Between 298 and 563 K

1979 ◽  
Vol 32 (12) ◽  
pp. 2571 ◽  
Author(s):  
LF Phillips
Keyword(s):  
Numerical Integration ◽  
Rate Constant ◽  
Flow System ◽  
Rate Equations ◽  
Side Reactions ◽  
Resonance Fluorescence ◽  
Discharge Flow ◽  
Temperature Range ◽  
Rate Of Reaction ◽  
Estimated Error

Hyroxyl resonance fluorescence was used to study the reaction of OH with HCN in a discharge-flow system. The effect of side reactions involving OH was assessed by numerical integration of the rate equations for the system. The rate constant for the reaction: OH + HCN → products as measured at pressures above 10 Torr and under conditions where side reactions were believed to be unimportant, is given by the expression: k = 1.60 ° 10-11 T-1exp(-1.86 × 103/T) cm3 molecule -1 s-1 with an estimated error of � 20% over the temperature range from 298 to 563 K.

Rate of the OH + C6H6 + He reaction in the fall-off range by discharge flow and OH resonance fluorescence

1991 ◽  
Vol 69 (7) ◽  
pp. 1057-1064 ◽  
Author(s):  
A. Goumri ◽  
J. F. Pauwels ◽  
P. Devolder
Keyword(s):  
Rate Constant ◽  
Room Temperature ◽  
Flash Photolysis ◽  
Tropospheric Chemistry ◽  
Resonance Fluorescence ◽  
Discharge Flow ◽  
Gas Phase Kinetics ◽  
Radical Adduct ◽  
Fluorescence Reaction ◽  
Two Temperatures

The rate constant k1 of the reaction[Formula: see text]has been investigated by discharge flow resonance fluorescence of OH in the fall-off pressure range. From systematic measurements at five pressures between 0.5 and 9.5 torr, the Troe parameters k0 and k∞ (with Fc = 0.6) have been derived at two temperatures: room temperature and 353 K. For room temperature, (297 ± 3) K, these parameters are k0 = (1.7 ± 0.5) × 10−29 cm6 molecule−2 s−1, k∞, = (10 ± 2) × 10−13 cm3 molecule−1 s−1. Our experimental results are consistent with addition as the dominant path, in agreement with flash photolysis investigations and with the existence of a fast reaction with NO2 of the (OH—benzene) radical adduct. A numerical simulation shows that this latter reaction should have a rate constant of (4 ± 2) × 10−11 cm3 molecule−1 s−1 at 353 K. Key words: gas phase kinetics, discharge flow, resonance fluorescence, reaction of OH with benzene, tropospheric chemistry.

scholarly journals Kinetics of thiamin cleavage by sulphite

1969 ◽  
Vol 113 (4) ◽  
pp. 611-615 ◽  
Author(s):  
J. Leichter ◽  
M. A. Joslyn
Keyword(s):  
Aqueous Solutions ◽  
Rate Constant ◽  
Sulphur Dioxide ◽  
First Order ◽  
Ph Values ◽  
Rate Of Reaction ◽  
Kinetics Of

Results are presented on the rate of thiamin cleavage by sulphite in aqueous solutions as affected by temperature (20–70°), pH(2·5–7·0), and variation of the concentration of either thiamin (1–20μm) or sulphite (10–5000μm as sulphur dioxide). Plots of the logarithm of percentage of residual thiamin against time were found to be linear and cleavage thus was first-order with respect to thiamin. At pH5 the rate was also found to be proportional to the sulphite concentration. In the pH region 2·5–7·0 at 25° the rate constant was 50m−1hr.−1 at pH5·5–6·0, and decreased at higher or lower pH values. The rate of reaction increased between 20° and 70°, indicating a heat of activation of 13·6kcal./mole.

THE THERMAL DECOMPOSITION OF PERACETIC ACID IN AROMATIC SOLVENTS

1963 ◽  
Vol 41 (7) ◽  
pp. 1826-1831 ◽  
Author(s):  
F. W. Evans ◽  
A. H. Sehon
Keyword(s):  
Thermal Decomposition ◽  
Rate Constant ◽  
Peracetic Acid ◽  
First Order ◽  
Aromatic Solvents ◽  
Temperature Range ◽  
Polymeric Compounds

The thermal decomposition of peracetic acid in toluene, benzene, and p-xylene was studied over the temperature range 75–95°C. The main products of decomposition were found to be CH4, CO2, CH3COOH; small amounts of methanol, phenols, and polymeric compounds were also detected.The rate of the overall decomposition was first order with respect to peracetic acid, and the results could be explained by postulating the participation of the two simultaneous reactions:[Formula: see text] [Formula: see text]The rate constant of reaction (1) was independent of the solvent, whereas k2 was dependent on the solvent. The ratio k2/k1 was about 10.

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