In a reaction,A + B rightarrow product,the ra | vedclass

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(D) Let the order of reaction with respect to $A$ and $B$ be $x$ and $y$ respectively.So,the rate law can be given as:$R = k[A]^{x}[B]^{y} \dots (i)$W

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rate $= k[A]^2[B]$

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(D) Let the order of reaction with respect to $A$ and $B$ be $x$ and $y$ respectively.So,the rate law can be given as:$R = k[A]^{x}[B]^{y} \dots (i)$When the concentration of only $B$ is doubled,the rate is doubled:$2R = k[A]^{x}[2B]^{y} \dots (ii)$Dividing $(ii)$ by $(i)$:$2 = 2^{y} \Rightarrow y = 1$When concentrations of both $A$ and $B$ are doubled,the rate increases by a factor of $8$:$8R = k[2A]^{x}[2B]^{y} \dots (iii)$Dividing $(iii)$ by $(i)$:$8 = 2^{x} 	imes 2^{y}$Substituting $y = 1$:$8 = 2^{x} 	imes 2^{1}$ $\Rightarrow 4 = 2^{x}$ $\Rightarrow x = 2$Thus,the rate law is $R = k[A]^{2}[B]$.

Initial Pressure $p$ (torr)	$707$	$79$	$37.5$
Half-life $t_{1/2}$ (min)	$84$	$84$	$84$

In a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:

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