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) To determine the equation for the overall reaction, you need to sum up the individual steps of the mechanism while canceling out any common species. The given steps are:

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

By adding these two equations together, you can cancel out the H2O and I^- on both sides:

2H2O2 + 2I^- -> 2H2O + OI^- + H2O + O2 + I^-
Simplifying this equation, you get the overall reaction:

2H2O2(aq) + 2I^-(aq) -> 2H2O(l) + O2(g) + I2(aq)

So, the overall reaction is 2H2O2(aq) + 2I^-(aq) -> 2H2O(l) + O2(g) + I2(aq).

2) In the given mechanism, a catalyst is a species that is involved in a reaction but is not consumed or permanently changed by the reaction. Looking at the mechanism, you can see that I^- is not consumed in either step but gets regenerated, making it a catalyst.

So, the species acting as a catalyst in this reaction is I^-. (Note: Catalysts are typically written above the arrow in a chemical equation.)

3) A reaction intermediate is a species that is formed in one step of the mechanism but consumed in another. Since H2O2 is generated in step 1 and used up in step 2, it qualifies as a reaction intermediate in this mechanism.

So, the species acting as a reaction intermediate in this mechanism is H2O2.

4) To determine the rate law for the overall reaction, you need to consider the rate-determining step (which is usually the slowest step). In this case, step 1 is the slow step, so the rate law will be determined by the reactants involved in that step.

From step 1: H2O2 + I^- -> H2O + OI^-
Rate = k[H2O2][I^-]

So, the rate law for the overall reaction is Rate = k[H2O2][I^-].