(1) H₂O2(g) → 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O2(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question

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Chapter1: Chemical Foundations
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A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps:
(1)
H₂O2(g) →>> 2OH(g)
(2)
H₂O2(g) + OH(g) → H₂O(g) + HO₂(g)
(3) HO₂(g) + OH(g) → H₂O(g) + O₂(g)
If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining
step?
O Step 1
O None of the steps
O Step 3
O Impossible to determine
Steps 1 and 2
O All of the steps
O Step 2
Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can
write a rate-law expression.
Submit Question
Transcribed Image Text:A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question
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