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The reactions between SO 2 and C 2 H 2 (and C 2 H 4 ) at elevated temperatures. A single‐pulse shock tube investigation
Author(s) -
Fifer R.,
Moreau R.,
Bauer S. H.
Publication year - 1971
Publication title -
international journal of chemical kinetics
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 0.341
H-Index - 68
eISSN - 1097-4601
pISSN - 0538-8066
DOI - 10.1002/kin.550030306
Subject(s) - chemistry , acetylene , ethylene , shock tube , sulfur dioxide , sulfur , argon , analytical chemistry (journal) , decomposition , kinetics , shock (circulatory) , sulfur hexafluoride , chemical kinetics , shock wave , inorganic chemistry , thermodynamics , organic chemistry , catalysis , medicine , physics , quantum mechanics
The high‐temperature reaction between sulfur dioxide and acetylene in an excess of argon was studied in a 1−in. i.d. single‐pulse shock tube. Mixtures ranging from 1.81% to 5.40% SO 2 and 1.60% to 4.90% C 2 H 2 were heated to reflected shock temperatures of 1550°–2150°K, for dwell times of about 0.6 msec and gas dynamically quenched. Total reaction densities were 0.89 to 5.4 × 10 −2 moles/1. The reaction products were analyzed by gas chromatography. A technique was developed for separating Ar, C 2 H 4 , C 2 H 2 , SO 2 , CO, CO 2 , H 2 S, COS, and CS 2 . The major products of the reaction are CO, H 2 , CS 2 , and sulfur. The products observed were compared with those predicted on the assumption that equilibrium was attained. Several preliminary experiments were carried out with ethylene‐sulfur dioxide mixtures, and the results indicated that for this combination the sulfur dioxide probably reacted with the acetylene generated from the decomposition of the ethylene, rather than directly with the ethylene. The rate of decline in the sulfur dioxide content in C 2 H 2 ‐SO 2 mixtures was found to be approximately second order (total) and can be empirically represented by\documentclass{article}\pagestyle{empty}\begin{document}$$- \Delta ({\rm SO}_2)/\Delta t = 3.1 \times 10^{10} T^{1/2} \exp (- 40,800/RT)[{\rm Ar}]^{0.83} [{\rm SO}_{\rm 2}]^{0.87} [{\rm C}_2 {\rm H}_{\rm 2}]^{0.25} {\rm mole cm}^{{\rm - 3}} \sec ^{ - 1}$$\end{document} A mechanism is proposed to account for the overall reaction kinetics.