CHEM2 lab 3

CHEM2 lab 3 - 8000 10000 12000 1 / [H2O2] 1 / V Series1...

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Bobby Bardin II 10/3/07 Chem II experiment 3 Kinetics II: Catalysis Purpose: The purpose of this lab was to determine the rate of an enzyme-catalyzed reaction for the breakdown of H 2 O 2 . Procedure: Refer to Exp. #3 Kinetics II: Catalysis handout Data: 1 % H 2 O 2 4 % H 2 O 2 8 % H 2 O 2 12 % H 2 O 2 Rate from Trial 1 0.04017 0.2273 0.4485 0.57 Rate from Trial 2 0.04079 0.2571 0.4679 0.5220 Rate from Trial 3 0.03742 0.3323 0.4353 0.5402 Average Rate 0.03946 0.2722 0.4506 0.5441 The rate was a lot faster for higher concentrations of H 2 O 2 . Results and Calculations: Michaleis-Menten Plot 0 0.1 0.2 0.3 0.4 0.5 0.6 0 0.0002 0.0004 0.0006 0.0008 0.001 0.0012 0.0014 [H2O2] Reaction Rate (V) Series1
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V max = 0.5441 mol / s . K m = 0.0004 V = V max ([S] / [S] + K m ) V 1 = 0.5441 ( .0001 / .0001 + .0004 ) = 0.1088 V 2 = .5441 ( .0004 / .0004 + .0004) = 0.2721 V 3 = .5441 ( .0008 / .0008 + .0004) = 0.3627 V 4 = .5441 ( .0012 / .0012 + .0004) = 0.4081 Lineweaver-Burke Plot y = 0.0007x + 1.9299 R 2 = 0.995 0 1 2 3 4 5 6 7 8 9 10 -4000 -2000 0 2000 4000 6000
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Unformatted text preview: 8000 10000 12000 1 / [H2O2] 1 / V Series1 Linear (Series1) 1 / V = 1 / V max + ( K M / V max [S] ) 1 / V 1 = 1 / .5441 + (.0004 / .5441(.0001)) = 9.189 1 / V 2 = 3.667 1 / V 3 = 2.757 1 / V 4 = 2.45 -1 / K M = -2500 Discussion: During the completion of this lab the difference in the rate of a reaction using a catalyst and solutions of different concentration was found. The higher the concentration of H 2 O 2 used, the faster the rate of the reaction was. After thinking about the ideal gas law, PV = nRT, it would seem that the gas pressure sensor must work by determining the change in temperature of the flask. R is a constant, and the volume doesnt change. A set number of moles was put into the flask so the number moles doesnt change, but the temperature increases as the pressure increases proportionally....
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CHEM2 lab 3 - 8000 10000 12000 1 / [H2O2] 1 / V Series1...

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