I am working on a five-part question and I just need help with the last part. I'm not sure where to begin with that one. I pasted the question and answers (for a-d) to the other parts below. Thank you!

Consider the proposed mechanism for the reaction between nitrogen monoxide and hydrogen gas. Assume the mechanism is correct.

Step 1: 2NO → N2O2 (fast)
Step 2: N2O2 + H2 → N2O + H2O (slow)
Step 3: N2O + H2 → N2 + H2O (fast)

a. Use the steps in the mechanism to determine the overall balanced equation for the reaction.

2NO + 2H2 → N2 + 2H2O

b. If Step 2 is the rate-determining step, write the rate law for the reaction.

Rate = K2[N2O2][H2]

c. If the observed rate law is rate = K[NO]2[H2]2, which step is rate-determining?

Step 3 because it is the slowest step.

d. Identify all of the intermediates in the mechanism.

N2O2 and N2O

e. If the first step is the rate-determining step, what is the order of the reaction with respect to each reactant?

To determine the order of the reaction with respect to each reactant, we need to understand the rate law for the reaction when the first step is the rate-determining step. In this case, we can assume that the rate law is determined solely by the reactants involved in the rate-determining step.

Since the first step is 2NO → N2O2, the rate law with respect to NO can be written as:

Rate = k[NO]²

This means that the reaction is second order with respect to NO.

Now, let's consider the overall balanced equation determined in part (a): 2NO + 2H2 → N2 + 2H2O

In the overall balanced equation, we can observe that the stoichiometric coefficient of H2 is 2. Therefore, the order of the reaction with respect to H2 would also be 2.

So, when the first step is the rate-determining step, the order of the reaction with respect to NO is 2 and the order of the reaction with respect to H2 is also 2.