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ki C2O4 Step 1: 2 ClO2 (fast equilibrium) k-1 k2 Step 2: C2O4 + OH¯ → ClO;¯+HC1O2 (slow) k3 Step 3: HCIO2 + OH- → ClO2¯+H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer.

ki C2O4 Step 1: 2 ClO2 (fast equilibrium) k-1 k2 Step 2: C2O4 + OH¯ → ClO;¯+HC1O2 (slow) k3 Step 3: HCIO2 + OH- → ClO2¯+H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer.

Chemistry
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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rate law is r=k[ClO2][OH-]

ki 2 ClO2 2 C2O4 k-1 k2 C2O4 + OH¯ → ClO;¯+HCIO2 Step 1: (fast equilibrium) Step 2: (slow) k3 Step 3: HCIO2 + OH- → ClO2¯+H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C»O4 k-1 k2 Step 1: (fast equilibrium) Step 2: C2O4 + OH¯ → ClO;¯+HCIO2 (slow) k3 Step 3: HC1O2 + OH- → ClO2¯+H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
Transcribed Image Text:ki 2 ClO2 2 C2O4 k-1 k2 C2O4 + OH¯ → ClO;¯+HCIO2 Step 1: (fast equilibrium) Step 2: (slow) k3 Step 3: HCIO2 + OH- → ClO2¯+H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C»O4 k-1 k2 Step 1: (fast equilibrium) Step 2: C2O4 + OH¯ → ClO;¯+HCIO2 (slow) k3 Step 3: HC1O2 + OH- → ClO2¯+H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
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