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Jan 6th, 2015
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Question description

The decomposition of hydrogen peroxide:  2H2O2(aq) → 2H2O(l) + O2(g) is catalyzed by I(aq). The following mechanism has been proposed to explain the experimental rate law:

 (1) H2O2 + I ⇌ H2O + IO slow
 (2) H2O2 + IO → H2O + O2 + I fast

Write the rate law for the above chemical reaction derived from the proposed mechanism. Use the format k*x^(m)*y^(n)..., where x = [H2O2], y = [H2O], z = [O2], u = [I], v = [IO]. 

5Br-(aq) + BrO3-(aq) + 6H+(aq) " src=""> 3Br2(l) + 3H2O(l)

The above reaction is expected to obey the mechanism:

BrO3-(aq) + H+(aq) HBrO3(aq)  Fast equilibrium
HBrO3(aq) + H+(aq) H2BrO3+(aq)  Fast equilibrium
H2BrO3+(aq) + Br-(aq) " src=""> (Br-BrO2)(aq) + H2O(l)  Slow
(Br-BrO2)(aq) + 4H+(aq) + 4Br-(aq) " src=""> products  Fast
Choose, from the list below, correct expressions for the overall rate law which are completely consistent with the above mechanism.

-d[Br-]/dt = k[Br-][BrO3-][H+]2
-d[Br-]/dt = k[Br-][BrO3-][H+]
k[H+][Br-][BrO3-]2 = -d[BrO3-]/dt
-d[BrO3-]/dt = k[Br-]
k[BrO3-][Br-][H+]2 = -d[H+]/dt
-d[H+]/dt = k[Br-][BrO3-]2[H+]

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