The reaction of nitric oxide (NO(g)) with molecular hydrogen (H2(g)) results in

ID: 1058938 • Letter: T

Question

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

2NO (g) + 2H2(g)...> N2(g) + 2H2O(g)

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

One potential mechanism for this reaction is as follows:

H2(g) + 2NO(g)...> N2O (g) + H2O (g) k1 H2(g) + N2O (g)...> N2(g) + H2O(g) k2

Is this mechanism consistent with the experimental rate law? If not, why?

I posted it many times, Please give me an accurate and detailed answer.

From the given data-

Mechanism of the reaction is -

H2(g) + 2NO(g)...> N2O (g) + H2O (g) k1

H2(g) + N2O (g)...> N2(g) + H2O(g) k2 (fast)

---------------------------------------------------------------

2NO (g) + 2H2(g)...> N2(g) + 2H2O(g)

But -

Rate law = k [H2] [NO]]2

The given mechanism is consistent with the rate law given in the reaction.

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