1979
DOI: 10.1016/0009-2614(79)80349-8
|View full text |Cite
|
Sign up to set email alerts
|

An upper limit for the rate constant of the bimolecular reaction CH3 + → OH + H2CO at 368 K

Help me understand this report

Search citation statements

Order By: Relevance

Paper Sections

Select...
2
1
1

Citation Types

0
4
0

Year Published

1980
1980
2010
2010

Publication Types

Select...
6
1

Relationship

0
7

Authors

Journals

citations
Cited by 14 publications
(4 citation statements)
references
References 9 publications
0
4
0
Order By: Relevance
“…In the first reaction scheme CO + O 2 CO 2 + O the rate constant is 7.58 × 10 −47 cm 3 /molecule·s at 300 K . In contrast, the second scheme CH 2 ( 3 B 1 ) + O 2 CO 2 + H 2 with exothermicity of 186 kcal/mol has a much larger rate constant of 2 × 10 −12 cm 3 /molecule·s at 298 K. , The reaction between CH 3 and O 2 does not lead to CO 2 but follows the scheme CH 3 + O 2 CH 2 O + OH with a small rate constant of <3 × 10 −16 cm 3 /molecule·s at 298 K . As shown in Figure , a time dependence of production yield of CO 2 is derived from Figure .…”
Section: Resultsmentioning
confidence: 97%
See 1 more Smart Citation
“…In the first reaction scheme CO + O 2 CO 2 + O the rate constant is 7.58 × 10 −47 cm 3 /molecule·s at 300 K . In contrast, the second scheme CH 2 ( 3 B 1 ) + O 2 CO 2 + H 2 with exothermicity of 186 kcal/mol has a much larger rate constant of 2 × 10 −12 cm 3 /molecule·s at 298 K. , The reaction between CH 3 and O 2 does not lead to CO 2 but follows the scheme CH 3 + O 2 CH 2 O + OH with a small rate constant of <3 × 10 −16 cm 3 /molecule·s at 298 K . As shown in Figure , a time dependence of production yield of CO 2 is derived from Figure .…”
Section: Resultsmentioning
confidence: 97%
“…There are two reaction schemes to produce CO 2 . In the first reaction scheme the rate constant is 7.58 × 10 -47 cm 3 /molecule • s at 300 K. 23 In contrast, the second scheme with exothermicity of 186 kcal/mol has a much larger rate constant of 2 × 10 -12 cm 3 /molecule • s at 298 K. 24,25 The reaction between CH 3 and O 2 does not lead to CO 2 but follows the scheme with a small rate constant of <3 × 10 -16 cm 3 /molecule • s at 298 K. 26 As shown in Figure 11, a time dependence of production yield of CO 2 is derived from Figure 10. According to mass balance, the total [CH 2 ] o produced initially in eq 5 equals…”
Section: Rotational and Vibrational Energy Deposition In Comentioning
confidence: 99%
“…(72) are given in Equations [59] and [60], k^3 = Tol4'G7(TOOO/T)T"9 cm^/mole^ sec, KGG = 1. Substitution of (I)^ from Equation [62] into Equation [56] followed by integration from t=0 to t=tgyg yields Equation [63] MCH3I) = k4o(C"4)o(I)eq ave . [63] amounts of methyl iodide.…”
Section: Derivation Of Rate Equationsmentioning
confidence: 99%
“…Substitution of (I)^ from Equation [62] into Equation [56] followed by integration from t=0 to t=tgyg yields Equation [63] MCH3I) = k4o(C"4)o(I)eq ave . [63] amounts of methyl iodide. This result indicates that the rate of formation of methyl iodide was determined mainly by the rate of the chain-initiation step of the free-radical mechanism.…”
Section: Derivation Of Rate Equationsmentioning
confidence: 99%