log [S208^2-] (mol/L) Log In] mol/L a. Assuming the rate expression for this system is in the form, rate - k[I]*[S₂O,²], it should be possible to determine the values of x and y from the data obtained. Show why a plot of log(time) vs log[I] for runs 1-4 will give a slope of -x and log(time) vs. log[S₂Ox ] for runs 1, 5, 6, and 7 will give a slope of-y. b. Perform the graphing exercises listed above and determine the values of x and y. Insert your graphs from Excel here. Log (Time) vs Log [I] L 1.75 1.8 1.85 1.9 1.95 y=-1.7303x+1.7485 R=0.766 1.6 1.65 0.2 0.4 0.6 .0.8 1 1.2 1.4 -1.6 -1.8 D Log (Time) Log (time) vs. log [S208^2-] 0.5 -0.5 y=-0.8502x-0.0374 R² = 0.9882 -1.5 -25 2 14 1.52 -1.7 25 log (Time) 3. Based on your answers to a and b and the information in the procedure section, write down a mechanism consistent with your results and indicate which step is the rate determining step. 4. Did the copper (II) sulfate catalyze the reaction? Explain your answer.

log [S208^2-] (mol/L) Log In] mol/L a. Assuming the rate expression for this system is in the form, rate - k[I]*[S₂O,²], it should be possible to determine the values of x and y from the data obtained. Show why a plot of log(time) vs log[I] for runs 1-4 will give a slope of -x and log(time) vs. log[S₂Ox ] for runs 1, 5, 6, and 7 will give a slope of-y. b. Perform the graphing exercises listed above and determine the values of x and y. Insert your graphs from Excel here. Log (Time) vs Log [I] L 1.75 1.8 1.85 1.9 1.95 y=-1.7303x+1.7485 R=0.766 1.6 1.65 0.2 0.4 0.6 .0.8 1 1.2 1.4 -1.6 -1.8 D Log (Time) Log (time) vs. log [S208^2-] 0.5 -0.5 y=-0.8502x-0.0374 R² = 0.9882 -1.5 -25 2 14 1.52 -1.7 25 log (Time) 3. Based on your answers to a and b and the information in the procedure section, write down a mechanism consistent with your results and indicate which step is the rate determining step. 4. Did the copper (II) sulfate catalyze the reaction? Explain your answer.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.3CE

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