For the elementary reaction $2X + Y \rightarrow Z + W$,the molecularity is.....

During the kinetic study of the reaction,$2A + B \rightarrow C + D,$ the following results were obtained:

$Run$	$[A] / mol \ L^{-1}$	$[B] / mol \ L^{-1}$	Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$
$I.$	$0.1$	$0.1$	$6.0 \times 10^{-3}$
$II.$	$0.3$	$0.2$	$7.2 \times 10^{-2}$
$III.$	$0.3$	$0.4$	$2.88 \times 10^{-1}$
$IV.$	$0.4$	$0.1$	$2.40 \times 10^{-2}$

Based on the above data,which one of the following is correct?

For the reaction,$H_{2(g)} + Br_{2(g)} \longrightarrow 2 HBr_{(g)}$,$r = k[H_2][Br_2]^{\frac{1}{2}}$. What is the molecularity and order of reaction respectively?

Which of the following is an example of a second-order reaction?

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

The kinetic study of a reaction like $vA \rightarrow P$ at $300 \ K$ provides the following curve, where concentration is taken in $mol \ dm^{-3}$ and time in $min$. Identify the correct order $(n)$ and rate constant $(k)$.