Thesis (M. Eng.(Industrial Engineering))-Universiteit van Pretoria, 2007. / Abstract in English. Includes bibliographical references.

Thesis (Ph. D.)--University of Adelaide, Dept. of Chemical Engineering, 1999. / Includes bibliographical references (leaves 322-335).

Thesis (M.S.)--West Virginia University, 2008. / Title from document title page. Document formatted into pages; contains x, 67 p. : ill. (some col.). Includes abstract. Includes bibliographical references (p. 63-67).

Thesis (M.S.)--West Virginia University, 2009. / Title from document title page. Document formatted into pages; contains v, 126 p. : ill. (some col.). Includes abstract. Includes bibliographical references (p. 59-69).

Thesis (Ph. D.)--Brigham Young University Dept. of Chemical Engineering, 2006. / Includes bibliographical references (p. 141-150).

Thesis (Ph.D.)(Chemistry)--University of Pretoria, 2007. / Includes summary. Includes bibliographical references. Available on the Internet via the World Wide Web.

Thesis. 1978. Sc.D.--Massachusetts Institute of Technology. Dept. of Chemical Engineering. / MICROFICHE COPY AVAILABLE IN ARCHIVES AND SCIENCE. / Bibliography: leaves 382-396. / by Eric M. Suuberg. / Sc.D.

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Thermodynamic calculations are used to study the alkali reactions in coal gasifier atmospheres. The reactive alkali and sulfur species released from coal are first calculated at temperatures from 800 K to 1900 K and pressures from 1 atm to 100 atm. Four P-T diagrams are constructed for the stable alkali and/or alkali-sulfur species at differ-ent temperatures and pressures. Alkali vapors are generated by the reactions Na₂CO₃_(s) + 2C_(s) = 2Na_(g) + 3CO_(g) Na₂CO₃_(s) + H₂O_(g) + C_(s) = 2NaOH_(g) + 2CO_(g) or K₂CO₃_(s) + 2C_(s) = 2K_(g) + 3CO_(g) K₂CO₃_(s) + H₂O_(g) + C_(s) = 2KOH_(g) + 2CO_(g) The phases formed from alkali-cement, and alkali-sulfur-cement reaction are also predicted. For both 53% and 72% alumina cement, calcium aluminate (CaO•Al₂O₃) is decomposed by the reactions CaO•Al₂O₃ + 2Na + 1/20₂ = Na₂O•Al₂O₃ + CaO CaO•Al₂O₃ + 2K + 1/20₂ = K₂O•Al₂O₃ + CaO or CaO•Al₂O₃ + 2Na + l/2S₂ = Na₂0•Al₂O₃ + CaS CaO•Al₂O₃ + 2K + 1/2S₂ = K₂•Al₂O₃ + CaS / M.S.

This paper examines an overview of the economic and environmental aspects of Underground Coal Gasification (UCG) as a viable option to the above ground Surface Coal Gasification (SCG). In addition, some highlights, hurdles and opportunities from early investment to successful commercial application of some worldwide UCG projects will be discussed. Global energy demands have prompted continual crude oil consumption at an astronomical pace. As such, the most advanced economies are looking for local and bountiful resources to challenge crude oil's dependence for which coal provides the best alternative so far. In the U.S, the Department of Energy (DOE), the National Energy Transportation Laboratory (NETL) along with the Lawrence Livermore National Laboratory (LLNL) continue to support pilot programs that develop improved methods for clean coal technologies to produce coal derived fuels competitive with crude oil fuels at about $30 per barrel. Lignite, the softest of the four types of coal, is the best candidate for underground coal gasification due to its abundance, high volatility and water to carbon content in its rock formation. The biggest challenge of modern humans is to find a balance of energy consumption, availability of resources, production costs and environmental conservation. Additionally, UCG has environmental benefits that include mitigating CO₂ emissions through Carbon Capture and Storage (CCS) and reduced overall surface pollutants, making it the preferred choice over SCG. / text