S P Singh Solutions for Chapter: Mole Concept and Stoichiometry, Exercise 5: MISCELLANEOUS EXERCISE

$560 \mathrm{mL}$ of carbon monoxide is mixed with $500 \mathrm{mL}$ of oxygen and ignited. The chemical equation for the reaction is as follows:

$2\mathrm{CO}+{\mathrm{O}}_2\stackrel{ }{\to }2{\mathrm{CO}}_2$

Calculate the volume of oxygen used and carbon dioxide formed in the above reaction.

A gas cylinder of the capacity of $20 {\mathrm{dm}}^3$  is filled with gas $\mathrm{X}$ the mass of which is $10 \mathrm{g}$. When the same cylinder is filled with hydrogen gas at the same temperature and pressure the mass of the hydrogen is $2 \mathrm{g}$, hence the relative molecular mass of the gas is:

Calcium carbide is used for the artificial ripening of fruits. Actually, the fruit ripens because of the heat evolved while calcium carbide reacts with moisture. During this reaction calcium hydroxide and acetylene gas is formed. If $200 {\mathrm{cm}}^3$ of acetylene is formed from a certain mass of calcium carbide, find the volume of oxygen required and carbon dioxide formed during the complete combustion. The combustion reaction can be represented as below.

$2{\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{ }{\to }4{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

A gaseous compound of nitrogen and hydrogen contains $12.5\%$ hydrogen by mass. Find the molecular formula of the compound if its relative molecular mass is $37$.

A gas cylinder contains $24\times {10}^{24}$ molecules of nitrogen gas. If Avogadro’s number is $6\times {10}^{23}$  and the relative atomic mass of nitrogen is $14$, calculate the mass of nitrogen gas in the cylinder.

A gas cylinder contains $24\times {10}^{24}$ molecules of nitrogen gas. If Avogadro’s number is $6\times {10}^{23}$  and the relative atomic mass of nitrogen is $14$, calculate the volume of nitrogen at $\mathrm{STP}$ in ${\mathrm{dm}}^3$.

Commercial sodium hydroxide weighing $30 \mathrm{g}$ has some sodium chloride in it. The mixture on dissolving in water and subsequent treatment with excess of silver nitrate solution formed a precipitate weighing $14.3 \mathrm{g}$. What is the percentage of sodium chloride in the commercial sample of sodium hydroxide? The equation for the reaction is $\mathrm{NaCl}+{\mathrm{AgNO}}_3\stackrel{ }{\to }\mathrm{AgCl}+{\mathrm{NaNO}}_3$.

(Relative molecular mass of $\mathrm{NaCl}=58, \mathrm{AgCl}=143$)

A certain gas ‘$\mathrm{X}$’ occupies a volume of $100 {\mathrm{cm}}^3$ at $\mathrm{STP}$ and weighs $0.5 \mathrm{g}$. Find its relative molecular mass.