For a chemical reaction,A + 2B to C + D,the r | vedclass

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(B) The rate law for the reaction $A + 2B 	o C + D$ can be written as $Rate = k[A]^x[B]^y$,where $x$ and $y$ are the orders with respect to $A$ and $

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$\frac{3}{2}$

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(B) The rate law for the reaction $A + 2B 	o C + D$ can be written as $Rate = k[A]^x[B]^y$,where $x$ and $y$ are the orders with respect to $A$ and $B$ respectively.According to the problem,when $[A]$ is increased $9$ times,the rate increases $3$ times:$3 	imes Rate = k(9[A])^x[B]^y$$3 = 9^x \implies 3 = (3^2)^x \implies 3^1 = 3^{2x} \implies x = \frac{1}{2}$.When $[B]$ is increased $2$ times,the rate increases $2$ times:$2 	imes Rate = k[A]^x(2[B])^y$$2 = 2^y \implies y = 1$.The total order of the reaction is $x + y = \frac{1}{2} + 1 = \frac{3}{2}$.

$Exp.$	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Initial rate $(mol \ L^{-1} \ s^{-1})$
$1$	$2.5 \times 10^{-4}$	$3 \times 10^{-5}$	$5 \times 10^{-4}$
$2$	$5 \times 10^{-4}$	$6 \times 10^{-5}$	$4 \times 10^{-3}$
$3$	$1 \times 10^{-3}$	$6 \times 10^{-5}$	$1.6 \times 10^{-2}$

For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:

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