Thesis (Ph. D.)--Catholic University of America.

Thesis (Ph. D.)--Catholic University of America.

Acetylene may be produced from methane in any process which raises the methane to a high temperature for a very short period followed by rapid cooling. There are three processes which accomplish these critical conditions of temperature and reaction time: A. By electric discharge through the gas B. By supplying heat from an auxilliary fuel either in direct heat exchange or in a regenerative type furnace C. By simultaneously burning some of the feed gas by the admixture of some oxygen The last of these processes was studied in this project in a flow type reactor. The process was studied at temperatures of 1000°C to 1300°C and reaction times of .01 to .03 seconds. An attempt was made to derive the mechanism for this process. A quartz reactor of special design was used in this study. It consisted of three zones: namely, the preheat zone where the oxygen, and methane were separately preheated, the reaction zone where the oxygen and methane were mixed and burned, and finally the quench zone where the reaction products were rapidly cooled and the reaction halted. The products were then analyzed for acetylene, carbon dioxide, carbon monoxide, hydrogen and methane. The mechanism for the partial oxidation of methane is believed to follow the following reactions. First there are the initial rapid oxidation reactions which supply the necessary heat to crack methane: CH₄ + ½O₂ → CO + 2H₂ ; CH₄ + 2O₂ → CO₂+ 2H₂O ; CH4 + O₂ → C + 2H₂O After the oxygen has been used up, methane decomposes into ethane, ethylene, acetylene, carbon and hydrogen by the following reactions: CH₄ ⇌ CH₂ + H₂ ; CH₄ + CH₂ ⇌ C₂H₆ ; C₂H₆ ⇌ C₂H₄ + H₂ ; C₂H₄ ⇌ C₂H₂ + H₂ ; C₂H₂ ⇌ 2C + H₂ The rate of formation of acetylene was found to depend upon the square of the methane concentration while the rate of decomposition of acetylene depended upon the concentration of the acetylene. As the reaction progresses the concentration of acetylene rises to a maximum and then decreases to zero. This was explained to occur because the methane concentration decreased with time. Further reaction follows between the products of combustion and the products of decomposition of methane. The most important of these is the water gas reaction: C + H2Q ⇌ CO + H₂ It was proven by stoichiometric considerations that this reaction takes place, and is the most important of the side reactions. The following reactions also take place to a small extent: C + CO₂ ⇌ 2CO ; CO + H₂O ⇌ C0₂ + H₂ / Applied Science, Faculty of / Chemical and Biological Engineering, Department of / Graduate

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Thesis (Ph. D.)--Hong Kong University of Science and Technology, 2004. / Includes bibliographical references (leaves 333-356). Also available in electronic version. Access restricted to campus users.

Reprint of one article by the author bound in back of publication / iii, 199 leaves : ill. ; 26 cm. / Title page, contents and abstract only. The complete thesis in print form is available from the University Library. / Thesis (Ph.D.1974) from the Dept. of Organic Chemistry, University of Adelaide

Thesis (Ph.D. 1974) from the Dept. of Organic Chemistry, University of Adelaide. / Reprint of one article by the author bound in back of publication.

Thesis (M.Sc.)--University of Adelaide, 1959. / [Typewr.].

Thesis (Master)--İzmir Institute of Technology, İzmir, 2004. / Includes bibliographical references (leaves. 76-86).

Thesis (Ph. D.)--University of Oregon, 2004. / Typescript. Includes vita and abstract. Includes bibliographical references (leaves 145-154). Also available for download via the World Wide Web; free to University of Oregon users.