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The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: H2O2(aq) + I-(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) + I-(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [HOI] [H2O2] Rate = k [H2O2]2     Rate = k [I-] [H2O2] Rate = k [H2O2]2 [H2O2] Rate = k [I-] [HOI] Rate = k [H2O2] [H2O2] (b) Choose the correct chemical equation for the overall process. HOI(aq) + OH-(aq) --> H2O(l) + OI-(aq) H2O2(aq) + I-(aq) --> HOI(aq) + OH-(aq)     2 H2O2(aq) --> 2 H2O(l) + O2(g) (c) Identify an intermediate in the reaction. H2O HOI    H2O2 I- (d) Identify the catalyst in the reaction. H2O H2O2  HOI I- (e) Identify a reactant in the reaction. H2O2 HOI     H2O I- (f) Identify a product in the reaction. HOI H2O    H2O2 I-

The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: H2O2(aq) + I-(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) + I-(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [HOI] [H2O2] Rate = k [H2O2]2     Rate = k [I-] [H2O2] Rate = k [H2O2]2 [H2O2] Rate = k [I-] [HOI] Rate = k [H2O2] [H2O2] (b) Choose the correct chemical equation for the overall process. HOI(aq) + OH-(aq) --> H2O(l) + OI-(aq) H2O2(aq) + I-(aq) --> HOI(aq) + OH-(aq)     2 H2O2(aq) --> 2 H2O(l) + O2(g) (c) Identify an intermediate in the reaction. H2O HOI    H2O2 I- (d) Identify the catalyst in the reaction. H2O H2O2  HOI I- (e) Identify a reactant in the reaction. H2O2 HOI     H2O I- (f) Identify a product in the reaction. HOI H2O    H2O2 I-

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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The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism:

H2O2(aq) + I-(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) + I-(aq)



(a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process.


Rate = k [HOI] [H2O2]
Rate = k [H2O2]2    
Rate = k [I-] [H2O2]
Rate = k [H2O2]2 [H2O2]
Rate = k [I-] [HOI]
Rate = k [H2O2] [H2O2]





(b) Choose the correct chemical equation for the overall process.


HOI(aq) + OH-(aq) --> H2O(l) + OI-(aq)
H2O2(aq) + I-(aq) --> HOI(aq) + OH-(aq)  
  2 H2O2(aq) --> 2 H2O(l) + O2(g)





(c) Identify an intermediate in the reaction.


H2O
HOI   
H2O2
I-





(d) Identify the catalyst in the reaction.


H2O
H2O2 
HOI
I-





(e) Identify a reactant in the reaction.


H2O2
HOI    
H2O
I-





(f) Identify a product in the reaction.


HOI
H2O  
 H2O2
I-



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