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Unformatted text preview: Sam Eichenblatt Chem 1310 A2 Lab 12 Discussion In the first part of the experiment different levels of molarity for cyclohexanone, triiodide, and hydrochloric acid were mixed in solution until a stable number of products were formed. This occurred when the mixture became colorless. Using this information the rate of the reaction was calculated by taking the i 3- concentration and dividing it by the total time taken. Then using the equation ([a 1 ]/ [a 2 ]) reactionorderofa =rate 1 /rate 2 we could find the individual reaction orders of all three reactants. Once this is calculated the K value can be found in the equation rate=k[cyclohexanone] m [triiodide] n [hydrochloric acid] l where m, n and l are the reactions orders. It turned out that when half of the concentration of cyclohexanone and hydrocholoric acid was added into the reaction that the rate of the reaction also decreased by two, this gave these two reactants a reaction order of 1 but when half of the triiodide was added there was not a significant change in the rate of the reaction, this meant that the reaction order for...
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This note was uploaded on 09/07/2010 for the course CHEM 1310 taught by Professor Cox during the Fall '08 term at Georgia Institute of Technology.
- Fall '08