The mechanism for the reaction 2 H2O2(aq) → 2 H2O(1) + O2(g) in the presence of I (aq) is proposed to be: Step 1: Н202(аq) + Г(аq) > H20() + ОГ(аq) slow Step 2: H2O2(aq) + OI (aq) → H20(1) + O2(g) +I (aq) fast Which of the following species is an intermediate? A. This mechanism has no intermediates. B. H20 O C. H202 O D- O E. O

The mechanism for the reaction 2 H2O2(aq) → 2 H2O(1) + O2(g) in the presence of I (aq) is proposed to be: Step 1: Н202(аq) + Г(аq) > H20() + ОГ(аq) slow Step 2: H2O2(aq) + OI (aq) → H20(1) + O2(g) +I (aq) fast Which of the following species is an intermediate? A. This mechanism has no intermediates. B. H20 O C. H202 O D- O E. O

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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17a.)
The following mechanism is proposed: C6H5COOH ⇌ C6H5CO2H2+ (fast) C6H5CO2H2+ ⇌ C6H5CO+ + H2O (fast) C6H5CO+ + HX + H2O ⟶ C6H6NH2 + N2 + CO2 (slow) The overall rate constant for this reaction is 0.200x 10-3L mol-1 s-1. Is this value consistent with rate law r = kobs*[C6H5COOH]*[HX] ?
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