0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI

0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What is the rate law for the following mechanism: A+B +C2D (fast equilibrium; rate of forward reaction: k1, rate of reverse reaction: k_1) A+D -E (slow, rate: k2) E +G - H (fast, rate: k3) OA Rate= k2 (k1 k.j) [A]²{B][C] Rate= k2 (k1/k-1)[A]D] oc Rate= k1 [A][B][C] OD, Rate= k2 [A]²B][C] O E. Rate= k2 (k1 /k-1) [A][B][C]
0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI
The starting concentration (time zero) of crystal violet is 1 x 10-4 M. Using the proper integrated rate law and the calculated value for k, calculate the concentration of crystal violet after 240 seconds. Look at the equation of the trend line for your lost linear graph and the beer-lambert law. Equation from graph from NaOH 0.0660M is y= -0.0105x-0.6277