4. The following two step mechanism has been proposed for the reaction: Overall:

Question

4. The following two step mechanism has been proposed for the reaction:

            Overall:          2 NO(g) + H2(g) ? N2O(g) + H2O(g)

            1st step:         NO(g) + NO(g) ? N2O2(g)

            2nd step:        N2O2(g) + H2(g) ? N2O(g) + H2O(g)

a) Show that the elementary steps of the proposed mechanism add up to provide the balanced equation for the reaction.

b) Write a rate law for each step of the reaction.

1st step:

2nd step:

c) List all intermediates in the reaction.

d) If the first step was known to be much slower than the second step, what is the rate law for the reaction?

Explanation / Answer

Answer:
a). Balanced equation for the reaction:
2NO? N2O2
N2O2 +H2 ? N2O + H2O
Combing above two equations
2NO + N2O2 + N2O+2H2 ? N2O2 + N2O + N2 + 2H2O
Similar terms on bothsides get cancelled
2 NO (g) + 2 H2 (g) ? N2 (g) + 2 H2O (g)

b) If second step is the rate determining step then
Rate = k[N2O2][H2] (This cannot be rate determing step as N2O2 is intermediate formed in the reaction.

C) N2O2 is the intermediate formed in the reaction.

d). If first step is rate determining step:
Rate = k[NO]2

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