Carbon and oxygen combine to form two oxides, carbon monoxide and carbon dioxide in which the ratio of the weight of carbon and oxygen is respectively `12:16` and `12:32`. These figures illustrate the :
(a)law of multiple proportions
(b)law of reciprocal proportions
(c)law of conservation of mass
(d)law of constant proportions

Carbon and oxygen combine to from two oxides, carbon is respectively 12: 16 and 12 : 32 . These figures illustrate the :

Chemical equation is balanced according to the law of multiple proportions reciprocal proportions conservation of mass definite proportions.

Which one the following combinations illustrate law of reciprocal proportions ?

All samples of carbon dioxide contain carbon and oxygen in the mass ratio of 3:8 This is in agreement with the law of .

Hydrogen and oxygen combine to form two compounds, water and hydrogen peroxide. If the percentage of oxygen is 88.89 in water and 94.12 in hydrogen peroxide, show that the data support law of multiple proportions.

Hydrogen and oxygen are known to from two compounds. The hydrogen content in one one of these is 5.93% while in the other it is 11.2%. Show that this data illustrates the law of multiple proportions.

Can we apply Dalton's law of partial pressures to a mixture of carbon monoxide and oxygen ?

Carbon and oxygen react in ratio 3 : 8 by mass to form CO_(2) . What weight of carbon should be used to react completely with 32 g of oxygen ?

Carbon and oxygen react in ratio 3 : 8 by mass to form CO_(2) . What weight of carbon should be used to react completely with 32 g of oxygen ?

Nitrogen and oxygen combine to form many oxides. In some oxides, 14 g of nitrogen combine with either 16 g of oxygen or 32 g of oxygen. In some other oxides, 28 g of nitrogen combine with 16, 48, or 80 g of oxygen, (i) What are the formulae of the oxides ? (ii) What law of chemical combination does the formation of these compounds illustrate ?