Lab 2 - Chemical Kinetics

Lab 2 - Chemical Kinetics - Page 1 of 11 Name and ID: Lab...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Page 1 of 11 Name and ID: Lab Partner: Quiz Section: Grading: 60 pts. (Lab notebook pages are worth 5 pts - total for report and notebook is 65 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, that you have not plagiarized any part of this lab report, and that all calculations and responses other than the reporting of raw data are your own independent work. Failure to sign this declaration will cost you 5 points. Signature: Purpose and Method Part I: Clock Reaction (3 pts) (purpose, reactions/rate law, method) Part II: Crystal Violet-Hydroxide Reaction (3 pts) (purpose, reactions/rate law, method) 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: (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 calculation for the concentration of S 2 O 3 2- : HINT BOX Recall that since BrO3- and H+ where held constant, the rate law takes on the following form: 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. (round to nearest whole number) 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....
View Full Document

This note was uploaded on 01/20/2010 for the course CHEM 162 taught by Professor N. during the Spring '08 term at University of Washington.

Page1 / 11

Lab 2 - Chemical Kinetics - Page 1 of 11 Name and ID: Lab...

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online