The rate of decomposition of hydrogen peroxide can be increased by having the re

Question

The rate of decomposition of hydrogen peroxide can be increased by having the reaction occur in the presence of iodide ion. The reaction is thought to proceed by a two step mechanism. Step 1 H_2O_2 (aq) + I-(aq) rightarrow H_2O (l) + IO-(aq) Step 2 IO-(aq) + H_2O_2 (aq) rightarrow H_2O (l) + O_2(g) +I- (aq) Write the rate law for each of the elementary processes (steps) of the mechanism. If an intermediate appears in the rate law you must substitute for it. Write the chemical equation for the overall reaction. Identify the chemical species in the reaction that acts as a catalyst. Is the catalyst heterogeneous or homogeneous. Identify the chemical species in the reaction that is an intermediate. What is it about positions in the mechanistic steps of chemicals that allows you to distinguish between a catalyst and an intermediate If the reaction is first order in both hydrogen peroxide and iodide ion, which step is of the mechanism should be labeled as the rate determining (or slow) step

Explanation / Answer

7. for the given reaction,

7a. For step 1 reaction,

rate = k1[H2O2].[I-]

For step 2 reaction,

rate = k2[IO-][H2O2]

[IO-] = (k1/k2)[I-]

substituting,

rate = (1/k1)[[H2O2][I-]

7b. Overall equation : 2H2O2 ---> 2H2O + O2

7c. The catalyst in the reaction is I-. The catalyst is homogeneous.

The intermediate in the reaction is IO-.

7d. A catalyst remains unchanged during the course of a reaction, whereas an intermediate forms and then distintegrates in the reaction.

Thus I- is an catalyst and IO- is an intermediate

7e. If the reaction is first order,

the step 1 is slow step.

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