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# (Rate determining step): How to suggest possible mechanisms for the overall reaction? watch

1. I somewhat understand the worked example in the textbook... but I am so confused how to do this one from my homework pack. Please explain to me how to work this out!

Hydrogen, H2 reacts with nitrogen monoxide, NO, as shown in the equation below.
2H2(g) + 2NO (g) ---> N2(g) + 2H2O(g)
A chemist carries out a series of experiments and determines the rate equation for this reaction:
rate= k[H2(g)][NO(g)]^2

This overall reaction between hydrogen and nitrogen monoxide takes place by a two-step mechanism. The first step is much slower than the second step. Suggest a possible two-step mechanism for the overall reaction. (2)
Step 1:
Step 2:

Thank you very much! I can't find anything for this specific example anywhere D:
2. Step 1: 2NO + H2 → N2 +H2O2 <--slow step
Step 2: H
2O2 + H2 → 2H2O <--- fast step

3. (Original post by refinne)
Step 1: 2NO + H2 → N2 +H2O2 <--slow step
Step 2: H
2O2 + H2 → 2H2O <--- fast step
Please can you go through how you personally work it out please?

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Updated: October 15, 2013
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