template_162_Exp_2_Report_Template_041108

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Unformatted text preview: Page 1 of 11 Name and ID: Lab Partner: Quiz Section: Grading: 60 pts. Experiment 2: Chemical Kinetics Part I: A Clock Reaction Part II: Crystal Violet-Hydroxide Reaction By signing below, you certify that you have not falsified data and that you have not plagiarized any part of this lab report. Signature: Purpose and Method Part I: Clock Reaction (3 pts) Part II: Crystal Violet-Hydroxide Reaction (3 pts) Page 2 of 11 Stock Solutions Soln. Conc. Units HCl Experiment Test Tube #1 Test Tube #2 Temp. Run Celsius Time Rate # ml ml ml ml ml C sec. M/s 1 2** 3 4 5 6** 7 8 9 10** 11 12 13 14* 15* * Measurements made with a drop of 1.0 mM Ammonium Molybdate ** Repeated measurements for calculating k and Ea A drop of 1% Starch indicator solution is included in each run. S 2 O 3 2- I- BrO 3- H 2 O S 2 O 3 2- I- BrO 3- H + Data, Calculations and Graphs Please provide a sample rate calculation here (NEATLY handwritten is fine): (2 pts) Page 3 of 11 Experiment Temp Initial Concentrations (M) Time Rate Run # Celsius sec M/sec Run 1 1 pt Run 2 Run 3 Run 4 1 pt X-axis Y-axis log(Rate) 2 pts 1 pt S 2 O 3 2- I- H + BrO 3- log(I- ) Reaction Order Determination for I- Provide an example concentration calculation (NEATLY handwritten is acceptable): HINT BOX Recall that since BrO3- and H+ where held constant, the rate law takes on the following form (see pg. 27 in the lab manual): Rate = B[I- ] i Therefore, a plot of log(Rate) vs. log(I- ) will yield a straight line with a slope equal to i, the order of the reaction with respect to I- . Place your plot relating to the reaction order for I- here. Refer to the box above for hints. Properly label your graph (labels for axes, including units, and a title). Include a trendline and its equation and R 2 value on your graph. This is done by right-clicking on one of the data points on your graph and choosing "Add Trendline" from the drop down menu. The first tab asks what type of trendline you wish to use, and the Options tab allows you to include the trendline equation and R 2 value. Order with respect to I- : Page 4 of 11 Experiment Temp Initial Concentrations (M) Time Rate Run # Celsius sec M/sec Run 5 2 pts Run 6 RUn 7 Run 8 X-axis Y-axis log(Rate) 2 pts 1 pt S 2 O 3 2- I- H + BrO 3- log(BrO 3- ) Reaction Order Determination for BrO 3- Place your plot relating to the reaction order for BrO 3- here....
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This note was uploaded on 05/08/2008 for the course CHEM 162 taught by Professor N. during the Spring '08 term at University of Washington.

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