Rate constants for the reactions of OH radicals and Cl atoms with CH,CH,NO>, CH,CH,CH,NO,, CH3CH2CH2CHzN02, and CH,CH2CH2CH,CH2N02 have been determined at 295+3 K and a total pressure of approximately 1 atm. The OH rate data were obtained using both the absolute rate technique of pulse radiolysis co
A localized orbital study of the rearrangements CH3CH → CH2=CH2 and (CH3)2C → CH3CH=CH2
✍ Scribed by Mark S. Gordon; Patrick M. Saatzer; R.D. Koob
- Publisher
- Elsevier Science
- Year
- 1976
- Tongue
- English
- Weight
- 727 KB
- Volume
- 37
- Category
- Article
- ISSN
- 0009-2614
No coin nor oath required. For personal study only.
✦ Synopsis
The structures ofcthylidcne and propylidene in their lowest singlet states :ue considered using INDO lnd MIND 112 calculations. Using a gadicnt optimization method, it is found that R!INDO/Z predicts no encrg minimu.n f-or singlet ethylidenc, while INDO predicts non-&ssic4 bridged structures for the sinclcts of c-thylidene 2nd propylidclie-INDO barriers to conversion OF rhc cxbenes to the corresponding nlkenes are estimated to be 3.1 and 15.
3 kcal/molc for ethylidene and propylidene, respectively. The localized orbit& for these molecuics are followed through the "transirior! state" to the nlkene, and it is found that the carbene lone pair nnd thrce-xnter CCH bond transrorm into 2 CC "banana" bond and vinyl CH bond, respectively.
📜 SIMILAR VOLUMES
A study of the reaction initiated by the thermal decomposition of di-t-butyl peroxide (DTBP) in the presence of (CHa)?C=CHz (B) at 391-444 K has yielded kinetic data on a number of reactions involving CH3 (M.), (CH&CCHzCH3 (MB.) and ( C H ~) ~C C H ~C ( C H ~) Z C H ~C H ~ (MBB.) radicals. The cross
Excess molar volumes at the temperature 298.15 K were measured for , and {xCH3(CH2)4 CH3 +(1x)CH3(CH2)3OH}. Excess molar volumes were determined using an Anton Paar DMA 60/602 densimeter. The experimental values obtained in this work were compared with results obtained using methods which estimate
Excess molar enthalpies at the temperature 298.15 K were measured for CH2)n-2CH3}, (n = 10, 12), using a Calvet microcalorimeter. The experimental results were compared with those calculated by using the Nitta-Chao, UNIFAC I, and UNIFAC II models.