A vessel contains $28$ g of $N_2$ gas and $4$ g of $He$ gas. The total pressure within the vessel is measured to be $30$ bar. What is the partial pressure exerted by the $He$ gas? [Use atomic masses $N = 14, He = 4$]

The partial pressure of a dry gas is:

The circulation of blood in human body supplies $\;{{\rm{O}}_2}$ and releases ${\rm{C}}{{\rm{O}}_2}$. The concentration of ${{\rm{O}}_2}$ and ${\rm{C}}{{\rm{O}}_2}$ is variable but on the average, $100\,\,{\rm{mL}}$ blood contains $0.02{\rm{g}}$ of ${{\rm{O}}_2}$ and $0.08{\rm{g}}\,\,{\rm{C}}{{\rm{O}}_2}$. The volume of ${{\rm{O}}_2}$ and ${\rm{C}}{{\rm{O}}_2}$ at 1 atm and body temperature ${37^0}C$, assuming 10 litre blood in human body is:

If 10g of hydrogen and 64g of oxygen are mixed in a container at 25°C and exert a total pressure of 760 mmHg, what is the partial pressure of hydrogen?

In a mixture of three gases with partial pressures of 200 mmHg, 300 mmHg, and 500 mmHg, what is the total pressure of the gas mixture?

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?

A mixture of $N_2$ and $Ar$ gases in a cylinder contains $7$ g of $N_2$ and $8$ g of $Ar$. If the total pressure of the mixture of the gases in the cylinder is $27$ bar, the partial pressure of $N_2$ is: [Use atomic masses $N = 14, Ar = 40$]

To which of the following gaseous mixtures is Dalton’s law not applicable?

The density of oxygen gas at ${25^0}C$ is $1.458{\rm{mg}}/{\rm{litre}}$ at one atmosphere. At what pressure will oxygen have the density twice the value?

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

Calculate the total pressure in a 10.0 L cylinder which contains 0.4 g helium, 1.6 g oxygen and 1.4 g nitrogen at 27\,^\circ C.