Part A, B, and C are based upon the following mechanism proposed forthe decomposition of hydrogen peroxide using potassium bromide. Step 1: H2O2 (aq) + Br- (aq) --> H2O(aq) + OBr- (aq) Slow Step 2: H2O2 (aq) + OBr- (aq) --> H2O(aq) + Br- (aq) + O2 (g) Fast A) What is the overall reaction? B) What is the rate law? C) Why is Br- the catalysts?

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12 Dec 2019

Part A, B, and C are based upon the following mechanism proposed forthe decomposition of hydrogen peroxide using potassium bromide.

Step 1: H₂O₂ (aq) + Br^- (aq) --> H₂O(aq) + OBr^- (aq) Slow

Step 2: H₂O₂ (aq) + OBr^- (aq) --> H₂O(aq) + Br^- (aq) + O₂ (g) Fast

A) What is the overall reaction?

B) What is the rate law?

C) Why is Br^- the catalysts?

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Hubert KochLv2

13 Dec 2019

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The decomposition of hydrogen peroxide can be catalyzed byiodide ion. The catalyzed reaction is thought to proceed by a twostep mechanism.

step 1 H₂O₂(aq) + I^-(aq) => H₂O(l) + IO^-(aq)

step 2 IO^-(aq) +H₂O₂(aq) => H₂O(l) +I^-(aq)

a. Write the rate law for each of the elementary processes ofthe mechanism.

b. Write the chemical equation for the overall reaction.

c. Identify the intermediate, if any, in the mechanism.

d. If the rate law is Rate= k [H₂O₂][I^-] which step is slow?

azurecrow764

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:
H₂O₂(aq) + I^– (aq) H₂O(l) + IO^– (aq) (slow)
IO^– (aq) + H₂O₂(aq) H₂O(l) + O₂(g) + I^– (aq) (fast)

(a) Write the chemical equation for the overall process. (b) Identify the intermediate, if any, in the mechanism. (c) Assuming that the first step of the mechanism is rate determining, predict the rate law for the overall process.