Lab 3 - Ryan O'Hearn Chemical Principles II Lab -...

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Chemical Principles II Lab - 1011.206.43 Lab #3: Kinetics of Reaction between Oxalic Acid and Potassium Permanganate 01:57:11 Purpose Because chemicals react at all different rates, we need to know the rates of these reactions in order to control them for practical purposes. An example would be the rusting of metal in a car, in order for the car to last as long as possible, we need to know how long it takes for this reaction between metal and oxygen to take place, and also ways to slow it down. In this experiment, we will figure out the rate that potassium permanganate (KMnO 4 ) and oxalic acid (H 2 C 2 O 4 ) react together by measuring dependency on concentrations at a constant temperature. Procedure See “Chemistry 206 Lab: Chemical Principles II Laboratory,” Lab #3: “Kinetics of Reaction between Oxalic Acid and Potassium Permanganate.” Data Tables, Graphs Set-ups for Three Experiments Reactants Experiment 1 Experiment 2 Experiment 3 Distilled Water 6.00 mL 1.00 mL 5.00 mL 0.130 M KMnO 4 1.00 mL 1.00 mL 2.00 mL 0.755 M H 2 C 2 O 4 5.00 mL 10.00 mL 5.00 mL Total Volume 12.00 mL 12.0 mL 12.00 mL [KMnO 4 ] 1 M 0.0108 M 0.0108 M 0.0217 M [H 2 C 2 O 4 ] 1 M 0.3146 M 0.6292 M 0.3146 M Experiment #1 Temp = 26°C [KMnO 4 ] 1 M [H 2 C 2 O 4 ] 1 M Time (s) Rate 1 Trial 1 0.0108 M 0.3146 M 159s 0.0000679 M/s Trial 2 0.0108 M 0.3146 M 130s 0.00008308 M/s
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Lab 3 - Ryan O'Hearn Chemical Principles II Lab -...

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