Question

$4.4$ g of an oxide of nitrogen gives $2.24$ L of nitrogen. $60$ g of another oxide of nitrogen gives $22.4$ L of nitrogen at STP. This data illustrates the law of:

• A. conservation of mass
• B. multiple proportions
• C. constant proportions
• D. gaseous volume

Answer 1

The correct option is B multiple proportions

For the first oxide, the ratio of the mass of the oxide to the volume of the nitrogen liberated is $\frac{4.4}{2.24}=1.96$

For the second oxide, the ratio of the mass of the oxide to the volume of the nitrogen liberated is $\frac{60}{22.4}=2.67$
These two are in the ratio $\frac{1.96}{2.67}=\frac{1}{1.33}=\frac{3}{4}$ or 3:4

Hence, this illustrates the Law of multiple proportions.

Note: In the above example, we have used volume of nitrogen which is proportional to the mass of nitrogen.