Chemical Kinetics

Chemical Kinetics - Chemistry 107 November 9, 2007...

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Chemistry 107 November 9, 2007 Experiment 9: Chemical Kinetics: Experimental Determination of a Rate Summary: First, the computer was turned on and the logger pro program was opened up. The file experiment 11 was then opened up. Next, the colorimeter was calibrated using a cuvette filled ¾ of the way with water. A graduated cylinder was then filled with 10 mL of .2 M NaOH solution. Another was filled with 10 mL of 8 x 10^(-5) M crystal violet solution. After this was accomplished, these two solutions were combined to start a reaction. Next, the solution was placed in a cuvette and then data began to be recorded. The equation of the line produced was then determined. It was a second order. In part B, the same experiment was conducted except that a different value of OH- was used. The value used this time was .2 M. Results: On Lab paper. Graphs and Calculations: (Graphs are attached) Pseudo rate Constant for Part A, Run 1: k= -.7406/second Pseudo rate Constant for Part A, Run 2: k= -.5662/second
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This note was uploaded on 04/27/2009 for the course CHEM 107 taught by Professor Generalchemforeng during the Spring '07 term at Texas A&M.

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Chemical Kinetics - Chemistry 107 November 9, 2007...

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