Question

Two oxides of nitrogen A & B gave these results: 4.4 gm of ‘A’ gave 2.24 litre of nitrogen & 60 gm of ’B’ gave 22.4 litre of nitrogen at NTP. Show that these results illustrate the law of multiple proportions.

Answer 1

Answer:

n first oxide,

Mass of 2⋅24L of nitrogen at STP=2⋅8g

∴ Mass of oxygen =4⋅−2⋅=1⋅g

In second oxide

Mass of 22.4L of nitrogen at STP=28g

∴ Mass of oxygen =60−28=32g

∴ In second oxide 2⋅8g of nitrogen combines with 3⋅2g of oxygen

Keeping the mass of nitrogen same in both oxides, the different masses of oxygen which combines with 2⋅8g of nitrogen are 1⋅6g:3⋅2g or 1:2

This is a simple whole number ratio. This illustrates the law of multiple proportions

Explanation: