OXYGEN FROM - OXYGEN FROM WATER By Jorge Arias Justin Brown Dustin Duke Anh Nguyen Juste Nijadeu Barry Orendorff Capstone Design Project University

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OXYGEN FROM WATER By: Jorge Arias, Justin Brown, Dustin Duke, Anh Nguyen, Juste Nijadeu, Barry Orendorff Capstone Design Project- University of Oklahoma - Spring 2003 Water to Breathe? A new technology may make it possible… A recently discovered technology facilitates the chemical breakdown of water into its elemental components, hydrogen and oxygen, by using a manganese-containing compound. The compound, chemical formula: [H 2 O(terpy)Mn(O) 2 Mn(terpy)OH 2 ](NO 3 ) 3 acts as a catalyst in a chemical reaction that produces hydrogen and oxygen gas from liquid water. The task assigned to our group was to develop a profitable process using this oxygen-evolving complex (OEC) to produce oxygen from water. Several potential applications of this process were identified and research and economic analyses were conducted to determine which of these applications could warrant further attention. As a result of this analysis, applications for processes that require mass production of oxygen on an industrial-scale were eliminated. These processes would require plants comprised of costly equipment and very expensive chemicals that would make them economically inferior to current oxygen production methods. In the case of smaller-scale applications, especially those for use in space, this process is a more cost effective alternative than other competing technologies for the same environment. After extensive research and analysis our group has developed a process that is tailored specifically to meet all the needs of the application that was determined to be most profitable. The following is our proposal for a process that will use the OEC with a series of reactors, hydrogen-oxygen separation equipment and solar power to provide life- supporting oxygen on manned Mars exploration missions. Chemistry In this process a catalyst discovered by a chemistry professor at Yale University is used 19 . An illustration of the dehydrated form of the catalyst can be seen in Fig. 1. This process proceeds through three major reactions. The first of these major reactions is the production of oxygen and hydrogen along with the decomposition of the catalyst. It is illustrated by Eq. 1. In equation 1 the overall reaction for the oxygen production consumes two moles of catalyst, C 30 H 26 Mn 2 N 6 O 4 , combined with 16 moles of water to produce two MnO 4 - ions, two Mn 3+ ions, four C 15 H 11 N 3 , or terpy, ligands, 8 moles of oxygen, and 17 moles of hydrogen.
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Figure 1: Illustration of the catalyst The next major reaction is responsible for the rebuilding of the catalyst. It is illustrated by Eq. 2. This reaction also uses some of the hydrogen ions and electrons created by the primary reaction. It is important to note that this reaction is also the culmination of several individual redox reactions that have been left out for simplicity. In equation 2 the overall reaction for the regeneration of the catalyst uses the MnO 4 - , and Mn 3+ ions along with the terpy ligands, hydrogen gas, and water to regenerate the catalyst and produce H 2 SO 5 .
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This note was uploaded on 08/31/2011 for the course CHE 4273 taught by Professor Staff during the Spring '10 term at Oklahoma State.

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OXYGEN FROM - OXYGEN FROM WATER By Jorge Arias Justin Brown Dustin Duke Anh Nguyen Juste Nijadeu Barry Orendorff Capstone Design Project University

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