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  4. Two oxides of a certain metal were separately heated in a current of hydrogen until constant weights were obtained. The water produced in each case was carefully collected and weighed. 2 g of each oxide gave, respectively 0.2517 g and 0.4526 g of water. This observation illustrates

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Q. Two oxides of a certain metal were separately heated in a current of hydrogen until constant weights were obtained. The water produced in each case was carefully collected and weighed. 2 g of each oxide gave, respectively 0.2517 g and 0.4526 g of water. This observation illustrates

Some Basic Concepts of Chemistry

Solution:

Weight of $H _{2} O$ from oxides give weight of oxygen and metal in oxide.
$0.2517 g H _{2} O$ contains oxygen $=\frac{16}{18} \times 0.2517=0.2237 g$
Mass of metal $=2-0.2237=1.7763 g$
$0.4526 g H _{2} O$ contains oxygen $=\frac{16}{18} \times 0.4526=0.4023 g$
Mass of metal $=2-0.4023=1.5977 g$
Thus, we can get the weight of oxygen with constant weight of metal
$(1 g )$ for other oxides, which two are in simple ratio of
$0.125: 0.251=1: 2$