The mechanism for the reaction described by the equation CH3NC(g) yields CH3CN (

Question

The mechanism for the reaction described by the equation

CH3NC(g) yields CH3CN (g)

is suggested to be

1. A(g) + M(g) yields(double arrows), k1 on the top, and k-1 on the bottom A*(g) +M(g)

2. A*(g) k2 on the top yields B(g)

where A(g) is CH3NC(g), and M(g) is any gas molecule, A*(g) is CH3NC*(g) ( and energized gas molecule), and B(g) is CH3CN(g)

a) assuming that [A*] is governed by steady state conditions dervive the rate law for the production of CH3CN(g) in terms of [A] , [M], and the appropriate k values and enter it in the space below.

rate of reaction= delta[CH3CN]/delta t=? what is the rate of the reaction?

Explanation / Answer

Rate eq for 1:

rA*=k1[A][M]-(k-1+k2)[A*]

At steady state rA*=0

Now,

rB=k2[A*]=k2k1[A][M]/k-1+k2

or, K[A][M]

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