This law was proposed by Dalton in 1803 . According to this law , if two elements combune to form more than one compounds ,the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole number.
For exemple, hydrogen combines with oxygen to form two compounds ,namely, water and hydrogen peroxide.
Here, the masses of oxygen (i.e, 16g and 32g) which combine with a fixed mass of hydrogen (2g) bear a simple raio, i.e, 16 :32 or 1 :2
0.11 g of an oxide of nitrogen gives 56 Ml `N_(2)` at 273K and 1 atm. 0.15 g of another oxide of nitrogen gives 56mL `N_(2)` at 1 atm , 273K. Show that these data confirm the law of multiple proportion.

Answer

`0.11` gm oxide gives `=> 0.07` gm N, Hence; `0.07` gm N + `0.04` gm O
`0.15` gm oxide gives `=>0.07` gm N, Hence; `0.07` gm N + `0.08` gm O