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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 $0.125: 0.251=1: 2$