1. Law of multiple proportions.
When two elements combine to form more than one compound the different mass of one of the elements which combine with the fixed mass of the other element bear a simple ratio.
2.
Oxides |
Mass of N |
Mass of O |
Ratio |
Formula |
Oxide I |
14 |
16 |
1:1 |
NO |
Oxide II |
14 |
32 |
1:2 |
NO2 |
Oxide III |
28 |
16 |
2:1 |
N2O |
Oxide IV |
28 |
48 |
2:3 |
N2O3 |
In NO and NO2 , the masses of oxygen combining with a fixed mass (14 g) of nitrogen are in the ratio, 16:32 = 1:2. Similarly, in N2O and N2O3 , the masses of oxygen combining with a fixed mass (28 g) of nitrogen are in the ratio, 16:48 = 1:3. These are simple whole number ratios. Hence, the law of multiple proportions is verified.