The proposed mechanism for a reaction is 1) A(g) + B(g) `hArr ` X(g)       [fast] 2) X(g) +C(g) `->` Y(g)        [slow] 3) Y(g) `->`    D(g)               [fast]   What are...

The proposed mechanism for a reaction is

1) A(g) + B(g) `hArr ` X(g)       [fast]

2) X(g) +C(g) `->` Y(g)        [slow]

3) Y(g) `->`    D(g)               [fast]

 

What are the molecularity and the rate law for each step?

 

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The overall reaction for these proposed mechanisms is:

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

Y and X are the intermediates. 

The proposed mechanism is not a single step reaction that gives rise in the formation of the intermediates.

For the rate law; order of reaction; molecularity

1.` r = k[A][B]` ; second order reaction; bimolecular

2. `r = k[X][C]` ; second order reaction; bimolecular

3. `r = k[Y]` ; first order reaction; unimolecular

 

However since it is noted that the second reaction is the slow reaction, it is called the rate determining step

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