6) The Rate of the Oxidation of Ethanol by Chromium(VI) (1)

6) The Rate of the Oxidation of Ethanol by Chromium(VI) (1)...

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INTRODUCTION In this experiment, we were to determine the rate of the oxidation of ethanol by Cr(VI) and the order of the reaction. The basic concept of this lab, chemical kinetics is the study of the rates and mechanisms of chemical reactions. The rate of a reaction always depends on the temperature at which it is run and usually depends on the concentrations of the reactants. Because of the latter fact, the rate of a reaction will usually change during the course of the reaction. The rate of a reaction at a particular temperature often depends solely on the concentrations of the reactants present. For a reaction, A + B → products Such a dependence on concentration would be described by the rate law: rate = k [A] x [B] y In this experiment, 4 CrO 3 Cl - + 3 C 2 H 6 O+ 12 H + 3C 2 H 4 O 2 + 4 Cr 3+ + 9H 2 O + 4 Cl - The rate law for this reaction might be written: rate = k [H + ] x [C 2 H 6 O] y [CrO 3 Cl - ] z However, if the concentration of both acid and ethanol are made much higher than the concentration of the CrO 3 Cl - , the rate law becomes: rate = k’ [CrO 3 Cl - ] z PROCEDURE A) Standardization of sodium thiosulfate solution 1) Fill buret with CrO 3 Cl - (aq) 2) Record the concentration 3) Fill second buret with S 2 O 3 2- (aq) 4) Measure out 10mL CrO 3 Cl - (aq) to Erlenmeyer flask 5) Record volume at least ± 0.2mL i. Solution should be brown-black 7) Titrate the solution with sodium thiosulfate to palegreen B) The kinetics of the reaction of Cr(VI) and Ethanol 1) 150mL of the reaction of(VI) and Ethanol 2) Add 2mL of ethanol in the solution 3) Record the exact time 4) Stir the solution 5) Drain the left over CrO 3 Cl - (aq) 6) Pour ethanol CrO
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6) The Rate of the Oxidation of Ethanol by Chromium(VI) (1)...

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