Kinetics and mechanism of formaldehyde oxidation

Vardanyan, I.A.; Sachyan, G. A.; Philiposyan, A.G.; Nalbandyan, A.B.

doi:10.1016/s0010-2180(71)80053-6

Cited by 34 publications

(11 citation statements)

References 8 publications

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“…It is produced during the oxidation of most hydrocarbons, and is known to behave as a branching intermediate during the high temperature combustion of methane. The proposed reaction mechanism of combustion of formaldehyde [28,29] is shown in Table 3.…”

Section: Methanol Combustionmentioning

confidence: 99%

Review on Chemical Reactions of Burning Poly(methyl methacrylate) PMMA

Zeng

Chow

2002

Journal of Fire Sciences

108

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Chemical reactions of burning Poly(methyl methacrylate) (PMMA) are reviewed in this paper although kinetics of thermal decomposition are believed to be fairly simple. Basically, there are three stages in the combustion of PMMA. Firstly, PMMA decomposes to produce monomer methyl methacrylate (MMA). Secondly, monomer MMA decomposes to generate small gaseous molecules that are usually combustible. Finally, these small molecules undergo combustion. Recent studies on the thermal decomposition kinetics and thermal stability of PMMA are also introduced. Results are useful for understanding the heat released of burning PMMA per unit mass of oxygen. Finally, the effects of additives on thermal decomposition are also discussed.

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Section: Methanol Combustionmentioning

confidence: 99%

Review on Chemical Reactions of Burning Poly(methyl methacrylate) PMMA

Zeng

Chow

2002

Journal of Fire Sciences

108

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“…As before [4] the experiments were carried out in a flow system at atmospheric pressure, and the total rate of formation of COs, as well as the concentration of HOz, were determined.…”

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confidence: 99%

The rate constant of the reaction HO₂ + COCO₂ + OH

Vardanyan¹,

Sachyan²,

Nalbandyan³

1975

Int J of Chemical Kinetics

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The high-temperature oxidation of formaldehyde in the presence of carbon monoxide was investigated to determine the rate constant of the reaction HOZ + CO = CO:! + OH (10). In the temperature range of 878-952°K from the initial parts of the kinetic curves of the HOz radicals and CO, accumulation at small extents of the reaction, when the quantity of the reacted formaldehyde does not exceed lo%, it was determined that the rate constant klo isA computer program was used to solve the system of differential equations which correspond to the high-temperature oxidation of formaldehyde in the presence of carbon monoxide. The computation confirmed the experimental results. Also discussed are existing experimental data related to the reaction of HOt with CO.On the basis of our detailed knowledge of the mechanism of the oxidation of formaldehyde in a reactor treated with boric acid, it was possible to attempt to determine the rate constant of the elementary reaction HO2 + CO=CO2 + O H I n the reaction mixture, which contained 1% formaldehyde and 99% air, part of the nitrogen was replaced by carbon monoxide. The mechanism of the oxidation of formaldehyde in the presence of carbon monoxide may be represented by the following reactions (Table I). The units of the rate constants are given in sec-', cm3/molec.sec, and cm6/molec2.sec for the reactions of the first, second, and third orders, respectively.Reactions (1 1)- (22) have been included because reaction (9) generates H atoms. The reaction O H + HO2 = H2O + 0 2 has not been included in the scheme because its velocity is noticeably less than the velocities of reactions (5) and (8). It follows from this scheme that the rate of formation of carbon dioxide is equal to d(C02)/dt = k9(0H)(CO) + klo(HOz)(CO). To evaluate the contribution of reaction (9)

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“…The RO 2 radicals were directed through the reactor to the freezing unit, placed in the resonator of ESR spectrometer, and analyzed with a technique described in previous publications [15,16]. The precision of detection of relative concentrations of radicals by the ESR method was <10%.…”

Section: Resultsmentioning

confidence: 99%

Reactions of CH₃O₂ radicals on solid surface

Manucharova

Tsarukyan

Vardanyan

2004

Int J of Chemical Kinetics

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The reaction probability of CH 3 O 2 radicals with NO 2 , CH 4 , C 3 H 6 , and CH 3 CHO on the solid surface of KCl in flow at low pressure and temperature range of 297-353 K has been studied. The chosen conditions allowed excluding homogeneous interaction of radicals. The heterogeneous radical decay of peracetic acid served as a source of CH 3 O 2 radicals.On the basis of ESR measurements of CH 3 O 2 radicals with the above-mentioned compounds, a heterogeneous reaction mechanism has been identified.The reactivity of NO 2 was greatest for the compounds studied. The effective activation energy was evaluated to be 10.4 ± 0.8 kJ/mol for the reaction of RO 2 radicals with NO 2 and −21.3 ± 2.8 kJ/mol for methane. C

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Kinetics and mechanism of formaldehyde oxidation

Cited by 34 publications

References 8 publications

Review on Chemical Reactions of Burning Poly(methyl methacrylate) PMMA

Review on Chemical Reactions of Burning Poly(methyl methacrylate) PMMA

The rate constant of the reaction HO₂ + COCO₂ + OH

Reactions of CH₃O₂ radicals on solid surface

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Kinetics and mechanism of formaldehyde oxidation

Cited by 34 publications

References 8 publications

Review on Chemical Reactions of Burning Poly(methyl methacrylate) PMMA

Review on Chemical Reactions of Burning Poly(methyl methacrylate) PMMA

The rate constant of the reaction HO2 + COCO2 + OH

Reactions of CH3O2 radicals on solid surface

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The rate constant of the reaction HO₂ + COCO₂ + OH

Reactions of CH₃O₂ radicals on solid surface