(d) Identify the catalyst in the reaction.O H₂OorH₂O2O HOI(e) Identify a reactant in the reaction.O H₂O2OrO HOIH₂O(f) Identify a product in the reaction.H₂O2O H₂OO HOIOr The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism:(a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process.O Rate = k [I] [HO]O Rate = k [1] [H₂0₂]O Rate = k [H₂0₂]²O Rate = k [HOI] [H₂0₂]O Rate = k [H₂0₂] [H₂02]O Rate = k [H₂0₂]² [H₂0₂](b) Choose the correct chemical equation for the overall process.O 2 HzOz(aq) --> 2 HzO(l) + Oz(g)O HOI(aq) + OH(aq) --> H₂O(l) + 01 (aq)O H₂O₂(aq) + 1°(aq) --> HOI(aq) + OH (aq)(c) Identify an intermediate in the reaction.OrO H₂O2O HOIO H₂OH₂O₂(aq) + (aq) --> HOI(aq) + OH(aq) (slow)HOI(aq) + OH(aq) --> H₂O(l) + OI (aq)OI (aq) + H₂O₂(aq) --> HOOI(aq) + OH (aq)HOOI(aq) + OH(aq) --> H₂O(l) + O₂(g) + (aq)

Kindly repost d, e, f questions seperately.

The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. O Ratek [I] [HOT] O Rate = k [1] [H₂0₂] O Rate = k [H₂0₂1² O Rate = k [HOI] [H₂0₂] O Rate = k [H₂0₂] [H₂0₂] O Rate = k [H₂0₂]² [H₂0₂] (b) Choose the correct chemical equation for the overall process. O2 H2Oz(aq) -- 2 H2O(l) + O2(s) HOI(aq) + OH(aq) --> H₂O(l) + 01 (aq) O H₂O₂(aq) + 1'(aq) --> HOI(aq) + OH(aq) (c) Identify an intermediate in the reaction. Or O H₂02 O HOI O H2O H₂O₂(aq) + (aq) --> HOI(aq) + OH(aq) (slow) HOI(aq) + OH(aq) --> H₂O(1) + 01¹(aq) or (aq) + H₂O₂(aq) --> HOOI(aq) + OH (aq) HOOI(aq) + OH(aq) --> H₂O(l) + O₂(g) + (aq)

The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. O Ratek [I] [HOT] O Rate = k [1] [H₂0₂] O Rate = k [H₂0₂1² O Rate = k [HOI] [H₂0₂] O Rate = k [H₂0₂] [H₂0₂] O Rate = k [H₂0₂]² [H₂0₂] (b) Choose the correct chemical equation for the overall process. O2 H2Oz(aq) -- 2 H2O(l) + O2(s) HOI(aq) + OH(aq) --> H₂O(l) + 01 (aq) O H₂O₂(aq) + 1'(aq) --> HOI(aq) + OH(aq) (c) Identify an intermediate in the reaction. Or O H₂02 O HOI O H2O H₂O₂(aq) + (aq) --> HOI(aq) + OH(aq) (slow) HOI(aq) + OH(aq) --> H₂O(1) + 01¹(aq) or (aq) + H₂O₂(aq) --> HOOI(aq) + OH (aq) HOOI(aq) + OH(aq) --> H₂O(l) + O₂(g) + (aq)

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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