In an experiment, 2.4 g of iron oxide on reduction with hydrogen yield 1.68 g of iron. In another experiment. 2.9 g of iron oxide give 2.03 g of iron on reduction with hydrogen show that the above data illustrate the law of constant proportions.

In an experiment, 2.4 g of iron oxide on reduction with hydrogen yield

1.	In an experiment, 2.4 g of iron oxide on reduction with hydrogen yield 1.68 g of iron. In another experiment. 2.9 g of iron oxide give 2.03 g of iron on reduction with hydrogen show that the above data illustrate the law of constant proportions.
Answer» Solution :In the first experiment The mass of IRON OXIDE =2.4g The mass of iron after reduction =1.68g The mass of oxygen =Mass of iron oxide-Mass of iron `=(2.4-1.68)=0.72g` RATIO of oxygen and iron `=0.72:1.68=1:2.33` In the second experiment The mass of iron oxide =2.9g The mass of iron after reduction =2.03 g The mass of oxygen `=(2.9-2.03)=0.87g` Ratio of oxygen and iron =`0.87:2.03=1:2.33` Thus, the DATA illustrate the law of constant proportions, as in both the experiments the ratio of oxygen and iron is the same.