Question

Which of the following rate laws is possible for the following two-step reaction?
1) NO(g) + NO(g) N2O2(g); FAST
2) N2O2(g) + O2(g) 2NO2(g); SLOW
Net: 2NO(g) + O2(g) 2NO2(g);

A. k[N2O2][NO]
B. k[NO]2
C. k[N2O2][O2]
D. k[NO][O2]


help!!!!! i don't know how to figure this out

Answer 1

Here is one of the best sites I've found that explains how to write the rate law. Be sure and read the first part in order to get the essentials but the second part is the one you want. It explains how to do problems in which the first step is fast and the second step is slow.
https://courses.lumenlearning.com/boundless-chemistry/chapter/reaction-mechanisms/

Post your work if you get stuck but remember that the rate law may NOT contain intermediates which means any equation containing (N2O2) isn't right.

Answer 2

Check your post and the problem you copied. I don't believe the correct answer is listed. Perhaps you made a typo.

Answer 3

These are the only options! Thank you anyway :)

Answer 4

k[NO]^2[O2]
Just took the quiz

Answer 5

you basically look at the reactants of the slow reaction they should always be in the rate law, their coifficient determines what order they are therefore A is the correct answer