4.4g of an oxide of nitrogen gives 2.24L of nitrogen. 60g of another oxide of nitrogen gives 22.4L of nitrogen at S.T.P. The data illustrates

Oxide I
4.4g liberate 2.24l of N₂ at STP (2.8g)
1g  liberate 'X' g of nitrogen.
$\mathrm{X}=\frac{2.8}{4.4} \mathrm{g} ;$

Oxide II
60g liberate 2.24l of N₂ at STP (2.8g)
1g  liberate 'Y'  g of nitrogen.
$\mathrm{Y}=\frac{20}{60}\mathrm{g} ;$

For fixed mass of oxide, X and Y liberated are in the ratio of 3:2.

It illustrates Law of multiple proportions.