One possible mechanism for the gas phase reaction of hydrogen with nitrogen mono

ID: 484922 • Letter: O

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) (dashes mean arrow)

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.

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=

Q1.

add both reactions

H2(g) + 2 NO(g) - N2O(g) + H2O(g)

N2O(g) + H2(g) - N2(g) + H2O(g)

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

H2(g) + 2 NO(g) + N2O(g) + H2(g) - N2O(g) + H2O(g) + N2(g) + H2O(g)

cancel common terms

2H2(g) + 2 NO(g) - 2H2O(g) + N2(g)

Q2.

catalyst --> is not consumed

so, in this specific case, there ar eno catalyst

Q3.

the reaction intermediate WILL be consumed

N2O is the intermediate, since it does not appears in th eend

Rate law ppaears o be --> SLOW step

Rate = k[H2][NO]^2

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