Question

Two oxides of lead were separately reduced to metallic lead by heating in a current of, hydrogen and the following data obtained :
i) Mass of yellow oxide taken $=3.45g$ Loss in mass during reduction $=0.24g$
ii) Mass of brown oxide taken $=1.227g$, Loss in mass during reduction $=0.16g$
Show that the above data illustrate the Law of Multiple Proportions.

Answer 1

Mass of the yellow oxide of lead= $3.45g$

Loss in mass due to reduction= $0.24g$

Mass of lead in yellow oxide= $3.45-0.24=3.21g$

Mass of oxygen in yellow oxide= $0.24g$

Similarly,

Mass of lead in brown oxide= $1.227-0.16=1.07g$

Mass of oxygen in brown oxide= $0.16g$

In yellow oxide, the amount of $Pb$ that combines with $1g$ of oxygen= $3.21/0.24=13.37$

Similarly, in brown oxide, the amount of $Pb$ that combines with $1g$ of oxygen= $\frac{1.07}{0.16}=6.69$

$\therefore$ Ratio of mass of $Pb$ in yellow oxide to mass of $Pb$ in brown oxide= $13.37:6.69=1.998:1=2:1$ .

$\therefore$ It can be concluded that the data is agreement with law of multiple proportion.