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 of partial pressure is applicable to which one of the following systems

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

A vessel has nitrogen gas and water vapours at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The contents of this vessel are transferred to another vessel having one third of the capacity of original volume, completely at the same temperature, the total pressure of the system in the new vessel is:

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 $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

A container holds two gases, A and B. The partial pressure of gas A is twice the partial pressure of gas B. If the total pressure is 600 mmHg, what is the partial pressure of gas B?

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.

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:

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:

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?

A mixture of ${{\rm{N}}_{\rm{2}}}$ and ${\rm{Ar}}$ gases in a cylinder contains ${\rm{7 g}}$of ${{\rm{N}}_{\rm{2}}}$ and ${\rm{8 g}}$ of ${\rm{Ar}}$. If the total pressure of the mixture of the gases in the cylinder is ${\rm{27}}$ bar, the partial pressure of ${{\rm{N}}_{\rm{2}}}$ is :

[Use atomic masses ${\rm{N = 14,}}\,{\rm{Ar}}\,{\rm{ = 40}}$]