Question

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?