One possible mechanism for the gas phase reaction of hydrogen with nitrogen monoxide is:

Question

One possible mechanism for the gas phase reaction of hydrogen with nitrogen monoxide is:

step 1  slow:  H₂(g) + 2 NO(g)  N₂O(g) + H₂O(g)

step 2  fast:   N₂O(g) + H₂(g)  N₂(g) + H₂O(g)

(1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank.

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(2) Which species acts as a catalyst? Enter formula. If none, leave box blank: 

(3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: 

(4) Complete the rate law for the overall reaction that is consistent with this mechanism.

(Use the form k[A]^m[B]ⁿ... , where '1' is understood (so don't write it) for m, n etc.)

Rate =

Answer 1

H₂(g) + 2 NO(g) ==> N₂O(g) + H₂O(g) ... slow

N₂O(g) + H₂(g)  <==> N₂(g) + H₂O(g) ... fast

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(1). 2H₂(g) + 2NO(g) ==> N₂(g) + 2H₂O(g) ... overall

(2). No catalyst

(3). N₂O is an intermediate

(4). Rate = k[H₂][NO]²