S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Some Basic Concepts of Chemistry, Exercise 6: PROBLEMS FOR PRACTICE

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$=3.45 \mathrm{g}$, Loss in mass during reduction$=0.24 \mathrm{g}$
(ii) Mass of brown oxide taken$=1.227 \mathrm{g}$, Loss in mass during reduction$=0.16 \mathrm{g}$
Show that the above data illustrate the law of Multiple Proportions.

Two oxides of lead were reduced to metallic lead by heating in a current of hydrogen and the following data obtained:

Mass of yellow oxide taken is $3.45 \mathrm{g}$, loss in mass during reduction is $0.24 \mathrm{g}$.

Mass of brown oxide taken is $1.227 \mathrm{g}$, loss in mass during reduction is $0.16 \mathrm{g}$.

Show that the above data illustrate the law of Multiple Proportions.

Copper gives two oxides. On heating $1.0$ g of each in hydrogen gas,$0.888$ g and $0.799$g of the metal are produced. Show that the results agree with the law of Multiple Proportions.

Two oxides of nitrogen contain the following percentage compositions:
(i) Oxide A contains $63.64\%$ nitrogen and $36.36\%$ oxygen.
(ii) Oxide B contains $46.67\%$ nitrogen and $53.33\%$  nitrogen

Establish the Law of Multiple Proportions.

A metal forms two oxides. One contains $46.67$ % of the metal and another, $63.94$ % of the metal. Show that these results are in accordance with the law of multiple proportions.

Nitrogen forms five compounds with oxygen in which$1.0 \mathrm{g}$ of nitrogen combines with$0.572, 1.14, 1.73, 2.28$ and $2.85 \mathrm{g}$ of oxygen respectively. Show that these figures agree with law of multiple proportions.

Elements $\mathrm{X}$ and $\mathrm{Y}$ form two different compounds. In the first, $0.324 \mathrm{g}$ of $\mathrm{X}$ is combined with $0.471 \mathrm{g}$ of $\mathrm{Y}$. In the second, $0.117 \mathrm{g}$ of $\mathrm{X}$ is combined with $0.509 \mathrm{g}$ of $\mathrm{Y}$. Show that these data illustrate the law of Multiple Proportions.

If a certain oxide of nitrogen weighing $0.11 \mathrm{g}$ gives $56 \mathrm{mL}$ of nitrogen and another oxide of nitrogen weighing $0.15 \mathrm{g}$ gives the same volume of nitrogen (both at $\mathrm{STP}$), show that these results support the law of multiple proportions.