The mechanism of the reaction A + 2B to D is2 | vedclass

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(A) The rate of a reaction is determined by the slowest step in the mechanism,which is called the rate-determining step.In the given mechanism:Step $1

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$k[B]^2, 0, 2, 2$

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(A) The rate of a reaction is determined by the slowest step in the mechanism,which is called the rate-determining step.In the given mechanism:Step $1$: $2B \xrightarrow{k} B_2$ $[Slow]$Step $2$: $B_2 + A 	o D$ $[Fast]$The rate law is determined by the slow step: $	ext{Rate} = k[B]^2$.Comparing this to the general rate law expression $	ext{Rate} = k[A]^x[B]^y$:Order with respect to $A$ $(x)$ = $0$.Order with respect to $B$ $(y)$ = $2$.Overall order of reaction = $x + y = 0 + 2 = 2$.Thus,the rate law expression is $k[B]^2$,order with respect to $A$ is $0$,order with respect to $B$ is $2$,and overall order is $2$.

The mechanism of the reaction $A + 2B \to D$ is
$2B \xrightarrow{k} B_2$ $[Slow]$
$B_2 + A \to D$ $[Fast]$
The rate law expression,order with respect to $A$,order with respect to $B$ and overall order of reaction are respectively

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The mechanism of the reaction $A + 2B \to D$ is$2B \xrightarrow{k} B_2$ $[Slow]$$B_2 + A \to D$ $[Fast]$The rate law expression,order with respect to $A$,order with respect to $B$ and overall order of reaction are respectively