The results given in the below table were obtained during kinetic studies of the following reaction:

$2 A + B \longrightarrow C + D$

Experiment	$[ A ] / molL ^{-1}$	$[ B ] / molL ^{-1}$	Initial $rate/molL$ $^{-1}$ $\min ^{-1}$
$I$	$0.1$	$0.1$	$6.00 \times 10^{-3}$
$II$	$0.1$	$0.2$	$2.40 \times 10^{-2}$
$III$	$0.2$	$0.1$	$1.20 \times 10^{-2}$
$IV$	$X$	$0.2$	$7.20 \times 10^{-2}$
$V$	$0.3$	$Y$	$2.88 \times 10^{-1}$

$X$ and $Y$ in the given table are respectively :

 

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