Kinetics in a Lean Formaldehyde Flame

Abstract The structure of a lean formaldehyde-oxygen flame burning at 22.5 Torr has been investigated experimentally using molecular beam sampling coupled with mass spectrometric analysis. Mole fraction profiles have been obtained for stable species as well as for atoms and radicals in a 17.9% CH2O-82.1% O2 flame. From data reduction it appears that about 80% of the formaldehyde is consumed in radical reactions and about 20% by bimolecular decomposition. The fast reactions of formaldehyde with atoms and hydroxyl radicals have the following rate constants: CH 2 +OH→CHO+HO 2 . k 3 =1.8×10 33 exp (−220/T) cm 3 mol −1 s −1 , CH 2 +OH→CHO+OH , xk 4 =6.0×10 13 exp (−1900/T) cm 3 mol −1 s −1 , CH 2 +OH→CHO+H 2 , k 5 =1.0×10 14 exp (−2480/T) cm 3 mol −1 s −1 , Besides these processes, the decomposition reaction of formaldehyde CH 2 +OH→CHO+H 2 +M , k 1 =2.5×10 14 exp (−14,250/T) cm 3 mol −1 s −1 , could play a role in the production of molecular hydrogen in this flame. Formyl radicals disappear mainly by CHO+O 2 +→CO 2 , k 7 =2.7×10 13 exp (−600/T) cm 3 mol −1 s −1 , and this reaction is the principal path for hydroperoxyl radical production. This last species reacts mainly with radicals and atoms (H, O, and OH). In the low temperature zone of the flame, CO2 is produced by CO+OH→CO 2 +H but also to some extent through CO+HO 2 →CO 2 +OH with a rate constant k10 = 3.5 × 1012 exp(−4125/T) cm3 mol−1 s−1

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