exp 15 - Discussion: Experiment #15 In part 1 of this...

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Discussion: Experiment #15 In part 1 of this experiment we tested the effects of various concentrations and their effects on the decomposition of hydrogen peroxide. The rate was .0294mL/s for solution 1 when we had the most DI water, and then increased by a factor of 2 for the next solution, which contained equal amounts of KI, water, and H 2 O 2 . For the last solution, the rate decreased a little to .0522mL/s, when we increased the KI, and decreased the water. We determined the rate law, by comparing the rates from the different solutions and finding the order by elimination of variables. The rate law was rate=k[H 2 O 2 ][I - ] which would be second order. The equation for this reaction is 2H 2 O 2 2H 2 O+O 2 , with Iodine as the catalyst and not included in the reaction. Part 2 consisted of testing the effects of temperature on the rate of decomposition of hydrogen peroxide. The rate increased by roughly a factor of 2 when we increased the temperature; it went from a .0294mL/s in part 1 to a .0616mL/s in part 2. This demonstrates that
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This note was uploaded on 05/12/2008 for the course CHEM 1CL taught by Professor Van koppen during the Spring '06 term at UCSB.

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exp 15 - Discussion: Experiment #15 In part 1 of this...

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