Below is a proposed mechanism for the decomposition of H2O2. H₂O₂ + H₂O + 10 SLOW H₂O₂ +10 → H₂O + O₂ +I FAST Which of the following statements is incorrect? The net reaction is 2H2O2 → 2H2O +02. The rate determining step depends on the rate law, r = k [H₂O₂][I]. I is a catalyst The rate law for the overall reaction is k [H202][10]. IO is an intermediate.
Below is a proposed mechanism for the decomposition of H2O2. H₂O₂ + H₂O + 10 SLOW H₂O₂ +10 → H₂O + O₂ +I FAST Which of the following statements is incorrect? The net reaction is 2H2O2 → 2H2O +02. The rate determining step depends on the rate law, r = k [H₂O₂][I]. I is a catalyst The rate law for the overall reaction is k [H202][10]. IO is an intermediate.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.51QP: In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were...
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![Below is a proposed mechanism for the decomposition of H2O2.
H₂O2 +
H₂O + 10¯ SLOW
H₂O₂ +10 → H₂O + O₂ +I FAST
Which of the following statements is incorrect?
The net reaction is 2H2O2 → 2H20 +02.
The rate determining step depends on the rate law, r = k [H₂O₂][I].
Or is a catalyst
The rate law for the overall reaction is k [H₂02][10].
10 is an intermediate.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fae5ac0fe-da7f-45ec-ae03-c91f17b6143c%2F73fa6d07-9ba3-4383-ada6-7a1d9174cea8%2Ftuqf31s_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Below is a proposed mechanism for the decomposition of H2O2.
H₂O2 +
H₂O + 10¯ SLOW
H₂O₂ +10 → H₂O + O₂ +I FAST
Which of the following statements is incorrect?
The net reaction is 2H2O2 → 2H20 +02.
The rate determining step depends on the rate law, r = k [H₂O₂][I].
Or is a catalyst
The rate law for the overall reaction is k [H₂02][10].
10 is an intermediate.
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