EXP 2 - KINETICS - Monday Wednesday 7:40-10:30 Experiment#2...

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04/28/2010 Experiment #2 – Kinetics of the Decomposition of Hydrogen Peroxide Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen dioxide with the following reaction: 2 H 2 0 2 (aq) 4 2 H 2 0 (l) + 0 2 (g) We can trap the oxygen gas created into a container thus showing the extent of the reaction and this will show the rate in which oxygen is created and how the rate will change when we use different initial concentrations. We do use a catalyst in this reaction to speed up the process and lower the activation energy needed to run the reaction. The catalyst is the Iodide ion that will be used in the form of potassium iodide (KI). Results at the end of the trails will be used to compose a rate of law for the reactions. This law will show the “dependence of the rate on the concentration of both H 2 0 2 and I-. The rate of reaction
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EXP 2 - KINETICS - Monday Wednesday 7:40-10:30 Experiment#2...

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