“…The equation k, = 1013.93*0.14 exp( -(45.7 f 0.4)kcal/mole/ RT)sec-*) has been derived from the measurements at 10 torr. The values of the Arrhenius parameters are nearly identical with those found in the hightemperature study of Tsang [20] (k, = 1013.9 exp( -46.2 kcal/mole/RT)sec-l) and in the low-temperature studies performed by Maccoll and Wong [21] (k, = Holbrook and Marsh [5] reported pl/z = 2.8 torr at incorrect. We conclude that the high-pressure region was covered by our measurements at 10 torr, since the rate constant was unaffected by lowering the initial pressure to 3 torr even at the highest temperature involved.…”
The thermal decompositions of ethyl chloride, is0 propyl chloride, and tertiary butylThe folchloride were studied in a static system in the pressure range of 0.1-300 torr. lowing Arrhenius equations for the high-pressure limit were obtained:
“…The equation k, = 1013.93*0.14 exp( -(45.7 f 0.4)kcal/mole/ RT)sec-*) has been derived from the measurements at 10 torr. The values of the Arrhenius parameters are nearly identical with those found in the hightemperature study of Tsang [20] (k, = 1013.9 exp( -46.2 kcal/mole/RT)sec-l) and in the low-temperature studies performed by Maccoll and Wong [21] (k, = Holbrook and Marsh [5] reported pl/z = 2.8 torr at incorrect. We conclude that the high-pressure region was covered by our measurements at 10 torr, since the rate constant was unaffected by lowering the initial pressure to 3 torr even at the highest temperature involved.…”
The thermal decompositions of ethyl chloride, is0 propyl chloride, and tertiary butylThe folchloride were studied in a static system in the pressure range of 0.1-300 torr. lowing Arrhenius equations for the high-pressure limit were obtained:
“…Thus, the thermal and chemical activation experiments are in fundamental agreement for the threshold energy of the CH 3 /Cl interchange reaction in neopentyl chloride. The calculated pre-exponential factor in Arrhenius form is 6.7 × 10 14 s −1 , which is 2.5 times larger than the upper limit of the experimental result, − , A = 2.5 × 10 14 s −1 . The large pre-exponential factor is a consequence of the low bending vibrational frequencies associated with the weakly bound Cl and CH 3 groups of the transition state.…”
Section: Computational Resultscontrasting
confidence: 54%
“…The reaction path degeneracies favor 1,2-HCl by a factor of 3, but the 3,2-HCl elimination channel must have a slightly lower E 0 . In fact, 3,2-HCl elimination to give 2-methyl-2-butene was favored in pyrolysis of 2-chloro-2-methyl-butane, 8 which also suggests that the E 0 is lower for 3,2-HCl elimination than for 1,2-HCl elimination. This is supported by the DFT calculations of the threshold energies that give E 0 (1,2-HCl) ) 41.4 kcal mol -1 and E 0 (3,2-HCl) ) 40.4 kcal mol -1 , although the absolute values are too low, see the Supporting Information.…”
Section: Resultsmentioning
confidence: 99%
“…Reaction is exothermic by about 2 kcal mol −1 ; thus, 2-methyl-2-chlorobutane acquires an additional 2 kcal mol −1 of energy during the interchange in reaction . The threshold energy, E 0 , for the interchange reaction is ≈60 kcal mol −1 , based on our electronic structure calculations and the thermal activation studies of neopentyl chloride, whereas those for HCl elimination, reactions a and b, are ≈45 kcal mol −1 according to pyrolysis studies of 2-methyl-2-chlorobutane. Thus, the rearrangement process in is the rate-limiting step for all forms of activation of neopentyl chloride (or bromide) molecules.…”
Section: Introductionmentioning
confidence: 85%
“…The Cl/F, Br/Cl, and Br/F interchange reactions for haloalkanes with halogen atoms located on adjacent carbon atoms have been demonstrated and characterized in a series of recent studies from this laboratory. − These interchange reactions, which often are in competition with hydrogen halide elimination reactions, have threshold energies for dihaloethanes ranging from 43 (Br/Cl) to 60 (Cl/F) − kcal mol −1 . The Cl/methyl group and Br/methyl group interchange reactions are members of this genre of unimolecular reaction.…”
The recombination of chloromethyl and t-butyl radicals at room temperature was used to generate neopentyl chloride molecules with 89 kcal mol(-1) of internal energy. The observed unimolecular reactions, which give 2-methyl-2-butene and 2-methyl-1-butene plus HCl, as products, are explained by a mechanism that involves the interchange of a methyl group and the chlorine atom to yield 2-chloro-2-methylbutane, which subsequently eliminates hydrogen chloride by the usual four-centered mechanism to give the observed products. The interchange isomerization process is the rate-limiting step. Similar experiments were done with CD(2)Cl and C(CH(3))(3) radicals to measure the kinetic-isotope effect to help corroborate the proposed mechanism. Density functional theory was employed at the B3PW91/6-31G(d',p') level to verify the Cl/CH(3) interchange mechanism and to characterize the interchange transition state. These calculations, which provide vibrational frequencies and moments of inertia of the molecule and transition state, were used to evaluate the statistical unimolecular rate constants. Matching the calculated and experimental rate constants, gave 62 ± 2 kcal mol(-1) as the threshold energy for interchange of the Cl atom and a methyl group. The calculated models also were used to reinterpret the thermal unimolecular reactions of neopentyl chloride and neopentyl bromide. The previously assumed Wagner-Meerwein rearrangement mechanism for these reactions can be replaced by a mechanism that involves the interchange of the halogen atom and a methyl group followed by HCl or HBr elimination from 2-chloro-2-methylbutane and 2-bromo-2-methylbutane. Electronic structure calculations also were done to find threshold energies for several related molecules, including 2-chloro-3,3-dimethylbutane, 1-chloro-2-methyl-2-phenylpropane, and 1-chloro-2-methyl-2-vinylpropane, to demonstrate the generality of the interchange reaction involving a methyl, or other hydrocarbon groups, and a chlorine atom. The interchange of a halogen atom and a methyl group located on adjacent carbon atoms can be viewed as an extension of the halogen atom interchange mechanisms that is common in 1,2-dihaloalkanes.
Abstract3,3-Dimethylbutanol-2 (3,3-DMB-ol-2) and 2,3-dimethylbutanol-2 (2,3-DMB-ol-2)The have been decomposed in comparative-rate single-pulse shock-tube experiments. mechanisms of the decompositions are 2,3-DMB-ol-2 3 iC3H7.The rate expressions areThese data, in conjunction with reasonable assumptions, give
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