A mixture of 0.5 moles of $O_2$ and 1 mole of $H_2$ is contained in a 1-litre flask at 273 K. Calculate the total pressure (in atm) inside the flask. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

A container holds 2 moles of helium and 3 moles of neon at a total pressure of 15 atm. What is the partial pressure of helium?

$32\,{\rm{g}}$ of oxygen and $3\,{\rm{g}}$ of hydrogen are mixed and kept in a vessel of $760\,{\rm{mm}}$ pressure and 0\,^\circ C. The total volume occupied by the mixture will be nearly:

Oxygen gas is collected by downward displacement of water in a jar. The level of water inside the jar is adjusted to the height of water outside the jar. When the adjustment is made, the pressure exerted by the oxygen is:

22 g solid ${\rm{C}}{{\rm{O}}_2}$ or dry ice is enclosed in a bottle of one litre properly closed. If temperature of bottle is raised to 25\,^\circ C to evaporate all the ${\rm{C}}{{\rm{O}}_2}$ the pressure in bottle is:

A mixture of nitrogen and oxygen gases has a total pressure of 750 mmHg. If the partial pressure of nitrogen is 450 mmHg, what is the partial pressure of oxygen?

Equal masses of ethane and hydrogen are mixed in an empty container at ${25^0}C$. The fraction of the total pressure exerted by hydrogen is

Two gases $A$ and $B$ having the mole ratio of $3:5$ in a container, exert a pressure of 8 atm. If $A$ is removed, what would be the pressure due to $B$ only, temperature remaining constant?

If 16 g of $O_2$ and 8 g of $H_2$ are present in a 4-litre container at $0^0C$, determine the total pressure (in atm) exerted by the gas mixture. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

Dalton's Law states that the total pressure of a mixture of gases is equal to:

Equal masses of ethane and ${H_2}$ are mixed in an empty container at ${25^0}C$, the fraction of the total pressure exerted by ${H_2}$ gas is