A mixture of nitrogen and oxygen gases exerts a total pressure of 1.2 atm. If the partial pressure of nitrogen is 0.8 atm, what is the partial pressure of oxygen according to Dalton's Law?

Two gases, $O_2$ (1 mole) and $H_2$ (0.5 moles), are mixed in a 2-litre vessel at a temperature of 273 K. Using the ideal gas constant $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$, find the total pressure (in atm) exerted by the mixture.

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 ${\rm{N = 14,}}\,{\rm{Ar}}\,{\rm{ = 40}}$]

10g each of $He$, $Ne$, and $Ar$ are mixed in a container of volume 'V' at 27°C. What is the total pressure exerted by the mixture? (Assume ideal gas behavior. Atomic masses: $He$=4, $Ne$=20, $Ar$=40, R= 0.0821 L atm/mol K)

The partial pressure of a dry gas is:

A mixture of gases contains 4 moles of $O_2$, 2 moles of $N_2$, and 1 mole of $CO_2$ at a total pressure of 2 atm. What is the mole fraction of $N_2$ and its partial pressure?

A container of volume 500 mL holds a mixture of 2 g of $O_2$ and 1 g of $H_2$ at $27^0C$. What is the total pressure (in atm) inside the container? (Use $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

If density of a gas in closed cylinder is $3.5g{L^{ - 1}}$ at 4.1 atm pressure and ${127^0}C$ temperature then molar mass of the gas will be $\left( {R = 0.082\,L\,atm\,{K^{ - 1}}\,mo{l^{ - 1}}} \right)$

A container holds a mixture of $He$ and $Ne$ gases. The partial pressure of $He$ is 0.3 atm, and its mole fraction is 0.6. If 0.2 moles of $Ar$ is added to the mixture while keeping the temperature and volume constant, what will be the total pressure of the resulting 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?

Two gases $A$ and $B$ having the same temperature $T$ same pressure $P$ and same volume $V$ are mixed. If the mixture is at the same temperature $T$ and occupies a volume $V$ the pressure of the mixture is: