5.975 g of the higher oxide of metal gave 5.575 g of lower oxide on heating. The quantity of the lower oxide gave 5.175 g-of metal on reduction. Prove that these results are in accordance with the law of multiple proportions.

As 5.575 g of lower oxide on reduction gives 5.175 g of the metal, the mass of the oxygen is 5.575 - 5.175 = 0.4 g

For 1 g of metal, mass of oxygen is 0.5 / 0.175 = 0.077 g

In case of higher oxides, mass of metal is 5.175 g Mass of oxygen is 5.975 —5.175= 0.8 g

For 1 g of metal, mass of oxygen is

0.8 /5.175 = 0.155 g

For a given mass of metal, the ratio of oxygen is 0.777:0.155 or 1:2. Hence, the law of multiple proportion is proved.