Kinetics of the thermal decomposition of n-propyl and isopropyl formates
The thermal decomposition of n-propyl and isopropyl formates was studied at 360/sup 0/, 380/sup 0/, 400/sup 0/C, and at 310/sup 0/, 322.5/sup 0/, and 335/sup 0/C, respectively. In both cases the principal primary reactions were the decomposition to propene and formic acid. This reaction is followed by a rather complex decomposition of the formic acid, which may be expressed by the equations: HCOOH ..-->.. H/sub 2/ + CO/sub 2/, HCOOH ..-->.. H/sub 2/O + CO, 2HCOOH ..-->.. H/sub 2/O + CO/sub 2/ + HCHO. The results indicate that other primary reactions must occur to a slight extent. The rate of propene formation was of the first order, and the experimental activation energies for this step were calculated to be 39,660 cal for n-propyl formate and 44,230 cal for isopropyl formate. The velocity constants for these reactions can be expressed by the following equations: n-Propyl formate: k = 2.94 x 10/sup 9/e/sup -39,660/RT/, Isopropyl formate: k = 2.47 x 10/sup 12/e/sup -44,230/RT/.
- Research Organization:
- State Univ. of Iowa, Iowa City
- OSTI ID:
- 5426658
- Journal Information:
- J. Phys. Chem.; (United States), Vol. 47:6
- Country of Publication:
- United States
- Language:
- English
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