Consider the following for the mechanism oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Elementary Step 1 H* + H₂O₂ = {H₂O*- OH) (rapid equilibrium) Elementary Step 2 (H₂O*-OH) + Br¯ → HOBR + H₂O (slowest) Elementary Step 3 HOBr + H+ + Br¯ → Br₂ + H₂O (fast) Consider the reaction profile below. What is the approximate activation energy (Ea) for elementary step 2? >

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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L
Consider the following
mechanism for the
oxidation of bromide
ions by hydrogen
peroxide in aqueous
acid solution.
Elementary Step 1
H+ + H₂O₂ = {H₂O*-
OH) (rapid
equilibrium)
Elementary Step 2
(H₂O*-OH) + Br¨ →
HOBr + H₂O (slowest)
Elementary Step 3
HOBr+ H+ + Br¯ → Br₂ +
H₂O (fast)
Consider the reaction
profile below. What is
the approximate
activation energy (Ea)
for elementary step 2?
7
Transcribed Image Text:L Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Elementary Step 1 H+ + H₂O₂ = {H₂O*- OH) (rapid equilibrium) Elementary Step 2 (H₂O*-OH) + Br¨ → HOBr + H₂O (slowest) Elementary Step 3 HOBr+ H+ + Br¯ → Br₂ + H₂O (fast) Consider the reaction profile below. What is the approximate activation energy (Ea) for elementary step 2? 7
Potential Energy (
Potential Energy (kJ/mol)
Reacton Profile
360
280
160
140
100
60
0
Reaction Progress
Transcribed Image Text:Potential Energy ( Potential Energy (kJ/mol) Reacton Profile 360 280 160 140 100 60 0 Reaction Progress
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