The proposed mechanism for a reaction is as follows [fast] (2) X(g) + C(g) K2, Y

Question

The proposed mechanism for a reaction is as follows [fast] (2) X(g) + C(g) K2, Y(g) [slow] (3) Y(g)-t, D(g) (a) What is the overall equation? (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) chemPad [fast] Help Greek- (b) Identify the intermediate(s), if any. (Select all that apply.) the intermediate(s), f any. A(g) B(g) C(g) D(9) x(g) Y(9) (c) what are the molecularity and the rate law for each step? (Rate equations take the general form rate-k·[A][Br.) Step 1 (forward step only): unimolecular O bimolecular

Explanation / Answer

(a) Overall reaction,

A(g) + B(g) + C(g) ---> D(g)

(b) Intermediate

X(g)

Y(g)

(c) For step 1

molecularity = Bimolecular

Rate law = rate = k1[A][B]

For step 2

molecularity = bimolecular

Rate law = rate = k2[C][X]

For step 3

molecularity = unimolecular

Rate law = rate = k3[Y]

(d) Yes the mechanism is consistent with the rate law

Yes

(e) Yes, the one step equation given is valid.

Yes

As X is formed by 1 mole each of A and B, it forms part of rate equation.

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