of an unknown oxide of nitrogen gives of nitrogen gas at STP. of another oxide of nitrogen gives of — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question
Question
$4.4\text{ g}$ of an unknown oxide of nitrogen gives $2.24\text{ L}$ of nitrogen gas at STP. $60\text{ g}$ of another oxide of nitrogen gives $22.4\text{ L}$ of nitrogen gas at STP. This analytical data perfectly illustrates which of the following laws of chemical combination?
💡 Solution & Explanation
In the first oxide, $2.24\text{ L}$ of $N_2$ at STP ($0.1\text{ mole}$ or $2.8\text{ g}$) combines with $4.4 - 2.8 = 1.6\text{ g}$ of Oxygen. Ratio $N:O = 2.8:1.6 = 14:8$. In the second oxide, $22.4\text{ L}$ of $N_2$ at STP ($1.0\text{ mole}$ or $28\text{ g}$) combines with $60 - 28 = 32\text{ g}$ of Oxygen. Ratio $N:O = 28:32 = 14:16$. For a fixed mass of Nitrogen ($14\text{ g}$), the ratio of combining masses of Oxygen is $8:16 = 1:2$, which is a simple whole-number ratio, proving the Law of Multiple Proportions.