Decomposition Of Hydrogen Peroxide Lab Report

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Kinetics of the Decomposition of Hydrogen Peroxide
Stephanie O’Brien
Anna Osatuke, Sean Ogurek,
Maia Popova, Yasmin Jessa,
Chem 145 section B, March 3, 2015 Abstract: One of the objectives of this experiment are to determine the kinetic order of a reaction from dependence of the rate on reactant concentrations. The method of completing this experiment is to run ten trials total and manipulate the amount of hydrogen peroxide and potassium iodine. For four trials H2O2 stayed constant and the KI was manipulated from the original amount and decreased by 25% each trial. The second four trials the exact opposite was done with KI and H2O2. Each trial runs for a total of 400 seconds. When both the KI and H2O2 were manipulated both final
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In this experiment potassium iodine and hydrogen peroxide are used. Hydrogen peroxide is an important oxidizing agent in the industry where it is used to bleach paper pulp, textiles and leather. Potassium iodine is used as catalysts in this experiment. Catalysts can speed up a decomposition reaction. They increase the rate of a reaction without undergoing a net change. The change in pressure will determined by the LabQuest. The objectives of this experiment are to monitor the rate of the chemical reaction, determine kinetic order of a reaction from the dependence of the rate on reactant concentrations. Kinetic order can be found by using this calculation Rate=k〖[H_2 O_2]〗^m 〖[KI]〗^n
Also determine the energy of activation. The energy can be calculated by using this equation ln(k_2/k_1 )=-(E_a/R)(1/T_2 -1/T_1 )
Lastly the objective is to understand the molecular components of the rate limiting step of the reaction. The hypothesis is that as temperature increases, the rate of reaction will as well. The method used for this experiment are to manipulate KI and H2O and run them through a total of 10
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I learned how to do new calculations and I got more practice with LoggerPro. I was not sure at first how this experiment would pan out, but I discovered that both reactants are first order and therefore are able to limit the reaction. From the experiment it was learned that the faster the rate the warmer the temperature. The calculations and the ten trials that were ran really helped me learn how rate, temperature and others work together. The objective of the experiment was to determine rate, kinetic order, and activation of energy and I feel that I learned and understand the experiment as a

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