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)
ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases
Section: Chapter Questions
Problem 2STP
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Transcribed Image Text:(d) Identify the catalyst in the reaction.
O H₂O
or
H₂O2
O HOI
(e) Identify a reactant in the reaction.
O H₂O2
Or
O HOI
H₂O
(f) Identify a product in the reaction.
H₂O2
O H₂O
O HOI
Or
![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]²
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.
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.
Or
O H₂O2
O HOI
O H₂O
H₂O₂(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)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2F27c782d9-530a-40c6-b7de-f00fd5ae6e35%2Fsdguu9r_processed.png&w=3840&q=75)
Transcribed Image Text: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]²
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.
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.
Or
O H₂O2
O HOI
O H₂O
H₂O₂(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)
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