The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism:

step 1 slow: H2O2 + I^- = H2O + OI^-
step 2 fast: H2O2 + OI^- = H2O + O2 + I^-

1) What is the equation for the overall reaction? Use the smallest integer coefficients possible.

I am not sure about this part.

2) Which species acts as a catalyst? Enter formula if there is one.

I think that I^- is the catalyst.

3) Which species acts as a reaction intermediate?

I think the H2O2 is the reaction intermediate.

4) Complete the rate law fot the overall reaction that is consistent with this mechanism.

I know that it would be k[][] but I am not sure what it is.

Thank you for your help!!

1) The overall reaction can be determined by adding step 1 and step 2 together, while cancelling out any intermediates that appear on both sides.

Step 1: H2O2 + I^- = H2O + OI^-
Step 2: H2O2 + OI^- = H2O + O2 + I^-

Adding these two equations gives us:

2H2O2 + 2I^- = 2H2O + O2 + 2I^-

Simplifying the equation, we get the overall reaction:

H2O2 + 2I^- = H2O + O2 + 2I^-

2) A catalyst is a species that is involved in the reaction but is regenerated at the end, without being consumed. From the given mechanism, it can be seen that I^- appears in step 1 and is regenerated in step 2. Thus, I^- acts as a catalyst in this reaction.

3) A reaction intermediate is a species that is formed during the reaction but consumed in a subsequent step, eventually leading to the formation of the products. From the given mechanism, it can be seen that H2O2 is consumed in step 1 and regenerated in step 2. Therefore, H2O2 acts as a reaction intermediate in this mechanism.

4) To complete the rate law for the overall reaction, we need to determine the rate-determining step. In this mechanism, step 1 is the slower, rate-determining step.

The rate law for the overall reaction will depend on the reactants involved in this step. From step 1, we can see that H2O2 and I^- are involved in this step. Therefore, the rate law for the overall reaction can be expressed as:

Rate = k [H2O2] [I^-]

Note that the specific values and orders of the rate constant (k) and the reactants cannot be determined solely from the given mechanism and would require experimental data.