The reaction of nitric oxide (NO(g)) with molecular hydrogen (H2(g)) results in the production of molecular nitrogen and water as follows:

2NO(g) + 2H₂(g) †’ N₂O(g) + 2H₂O(g)

The experimentally determined rate law expression for this reaction is first order in H₂(g) and second order in NO(g).

a. Is the reaction as written consistent with the experimental order dependence for this reaction?

b. One potential mechanism for this reaction is as follows:

Is this mechanism consistent with the experimental rate law?

c. An alternative mechanism for the reaction is:

Show that this mechanism is consistent with the experimental rate law.

Transcribed Image Text:

H2(g) + 2NO(g)– →N,O(g) + H20(g) (3)0'H + (3)'N,(3)o°N + (3)H 2NO(3)N,0,(3) (fast) 2N,02(8) (fast) k1 H2 (g) + N202(g)-* N20(g) + H,0(g) H2(g) + N20(g)– k »N2(g) + H2O(g)