Chemistry | VITEEE 2016 | Discussion Page

A reaction: A₂+B → products, involves the following mechanism

$A_{2}\rightleftharpoons 2A$ (fast)

(a being the intermediate)

A+B $\overrightarrow{k_{2}}$ Products (slow) The rate law consistent to this mechanism is

$rate =k[A_{2}][B]$

$rate =k[A_{2}]^{2}[B]$

$rate =k[A_{2}]^{1/2}[B]$

$rate =k[A_{2}][B]^{2}$

Option C

from slow step :

rate = k₂ [A][B] .............(i)

From fast step :

$K_{e}=\frac{[A]^{2}}{[A_{2}]} or [A] = K^{1/2}_{e}[A]^{1/2}$ ...........(ii)

From (i) and (ii)

rate = $k_{2}k_{e}^{1/2}[A_{2}]^{1/2}[B]=k[A_{2}]^{1/2}[B]$

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