4.The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thoughtto proceed by a two step mechanism:H2O2(aq) + I (aq) → H2O(1) + IO(aq)IO (aq) + H2O2(aq) → H2O (1) + O2(g) + I(aq)(slow)(fast)a) Write the chemical equation for the overall process.b) Identify any intermediates, if any, in the mechanism.c) Assuming the first step is the rate determining step, predict the rate law for the overallprocess.

The question is based on chemical kinetics. we have been given mechanism for the reaction. We need…

ne decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought eed by a two step mechanism: H2O2(aq) + I (aq) → H,0(1) + IO'(aq) IO (aq) + H,O2(aq) → H2O (1) + O2(g) + I(aq) (slow) (fast) Write the chemical equation for the overall process. dentify any intermediates, if any, in the mechanism. Assuming the first step is the rate determining step, predict the rate law for the overall orocess.

ne decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought eed by a two step mechanism: H2O2(aq) + I (aq) → H,0(1) + IO'(aq) IO (aq) + H,O2(aq) → H2O (1) + O2(g) + I(aq) (slow) (fast) Write the chemical equation for the overall process. dentify any intermediates, if any, in the mechanism. Assuming the first step is the rate determining step, predict the rate law for the overall orocess.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.30PAE: The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion...

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