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28. The reaction 4 HBr(g) + O2(g) --> 2 H2O(g) + 2 Br2(g) proceeds through the following mechanism: HBr(g) + O2(g) --> HOOBr(g) HOOBr(g) + HBr(g) --> 2 HOBr(g) HOBr(g) + HBr(g) --> Br2(g) + H2O(g) (a) The first step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [HBr] [O2] Rate = k [HBr]2 [O2]     Rate = k [HBr] [O2]2 Rate = k [HBr]1/2 [O2] Rate = k [HBr] [O2]1/2 Rate = k [HBr]2 Rate = k [HBr]2 [O2]1/2 (b) What would the rate law be if the third step of this mechanism were rate-determining? Rate = k [HBr] [O2] Rate = k [HBr]2 [O2]     Rate = k [HBr] [O2]2 Rate = k [HBr]1/2 [O2] Rate = k [HBr] [O2]1/2 Rate = k [HBr]2 Rate = k [HBr]2 [O2]1/2 Rate = k [HBr]

28. The reaction 4 HBr(g) + O2(g) --> 2 H2O(g) + 2 Br2(g) proceeds through the following mechanism: HBr(g) + O2(g) --> HOOBr(g) HOOBr(g) + HBr(g) --> 2 HOBr(g) HOBr(g) + HBr(g) --> Br2(g) + H2O(g) (a) The first step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [HBr] [O2] Rate = k [HBr]2 [O2]     Rate = k [HBr] [O2]2 Rate = k [HBr]1/2 [O2] Rate = k [HBr] [O2]1/2 Rate = k [HBr]2 Rate = k [HBr]2 [O2]1/2 (b) What would the rate law be if the third step of this mechanism were rate-determining? Rate = k [HBr] [O2] Rate = k [HBr]2 [O2]     Rate = k [HBr] [O2]2 Rate = k [HBr]1/2 [O2] Rate = k [HBr] [O2]1/2 Rate = k [HBr]2 Rate = k [HBr]2 [O2]1/2 Rate = k [HBr]

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....
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28. The reaction 4 HBr(g) + O2(g) --> 2 H2O(g) + 2 Br2(g) proceeds through the following mechanism:

HBr(g) + O2(g) --> HOOBr(g)
HOOBr(g) + HBr(g) --> 2 HOBr(g)
HOBr(g) + HBr(g) --> Br2(g) + H2O(g)




(a) The first step of this mechanism is rate-determining (slow). What is the rate law for this reaction?


Rate = k [HBr] [O2]
Rate = k [HBr]2 [O2]    
Rate = k [HBr] [O2]2
Rate = k [HBr]1/2 [O2]
Rate = k [HBr] [O2]1/2
Rate = k [HBr]2
Rate = k [HBr]2 [O2]1/2





(b) What would the rate law be if the third step of this mechanism were rate-determining?

Rate = k [HBr] [O2]
Rate = k [HBr]2 [O2]    
Rate = k [HBr] [O2]2
Rate = k [HBr]1/2 [O2]
Rate = k [HBr] [O2]1/2
Rate = k [HBr]2
Rate = k [HBr]2 [O2]1/2
Rate = k [HBr]
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