For the reaction 2A + B rightarrow C,the rate | vedclass

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(D) $1$. The rate law is given as $	ext{Rate} = k[A][B]$.$2$. The overall order of the reaction is $1 + 1 = 2$ (second-order reaction).$3$. The rate

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The value of $k$ is independent of the initial concentrations of $A$ and $B$.

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(D) $1$. The rate law is given as $	ext{Rate} = k[A][B]$.$2$. The overall order of the reaction is $1 + 1 = 2$ (second-order reaction).$3$. The rate constant $k$ is a characteristic property of a specific reaction at a given temperature and is independent of the initial concentrations of the reactants.$4$. Therefore,statement $D$ is correct.$5$. For a second-order reaction,the half-life is inversely proportional to the initial concentration,so it is not constant.$6$. The unit of $k$ for a second-order reaction is $L \ mol^{-1} \ s^{-1}$,not $s^{-1}$.

$Expt.$	$[X]_0 / mol \ L^{-1}$	$[Y]_0 / mol \ L^{-1}$	$Rate / mol \ L^{-1} s^{-1}$
$1$	$0.25$	$0.25$	$1.0 \times 10^{-6}$
$2$	$0.50$	$0.25$	$4.0 \times 10^{-6}$
$3$	$0.25$	$0.50$	$8.0 \times 10^{-6}$

For the reaction $2A + B \rightarrow C$,the rate law is given by: $\text{Rate} = k[A][B]$. Which of the following statements is correct regarding this reaction?

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