Lab 15 - Experiment 15: The Oxidation of Ethanol The...

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Experiment 15: The Oxidation of Ethanol The purpose of this experiment was to determine the rate constant and order of reaction for the oxidation of ethanol using potassium dichromate as the oxidizing agent. The rate constant is dependent on the concentration of the intermediate CH3CH2OCrO3H. This concentration cannot be measured directly so the absorbance is measured as a funtion of time using a spectrophotometer. The absorbance is then related to the concentration using Beer’s Law. A=bε[c]; b=thickness of sample, ε=absorbtivity Substituting into ln[C]= -kt +ln[Co] this gives ln(Ao/A)=kt Thus, the rate constant, k, cam be determined from the absorbance. Ethanol is oxidized by chromic acid according to the following reaction: 2CH3CH2OH +H2CrO4 → 3CH3COH + Cr(3+) + 4H2O. The second-order rate law for this reaction is Rate = k1k2[CH3CH2OH][H2CrO4]. The concentration of ethanol, however, is relatively constant so we can combine it with the k1 and k2 to give the “pseudo” first-order reaction
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This note was uploaded on 04/20/2010 for the course CHEM 1A/ 1 Chem Lab taught by Professor Van koppen during the Spring '10 term at UCSB.

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Lab 15 - Experiment 15: The Oxidation of Ethanol The...

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