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.

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

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:

Two flasks, A and B, of equal volume are connected by a narrow tube of negligible volume. Flask A contains $CO_2$ at 1 atm, while flask B contains $N_2$ at 2 atm. If the stopcock connecting the flasks is opened, and the gases are allowed to mix at constant temperature, what is the partial pressure of $CO_2$ in the final mixture?

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.

Which of the following equations does NOT correctly represent Dalton's Law of Partial Pressures for a mixture of three gases A, B, and C, where $p$ is the total pressure?

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 $N = 14, Ar = 40$]

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:

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:

${O_2}$ is collected over water at 20\,^\circ C. The pressure inside shown by the gas is 740 mm of Hg. What is the pressure due to ${{\rm{O}}_2}$ alone if vapour pressure of ${{\rm{H}}_2}{\rm{O}}$ is 18 mm at 20\,\,^\circ C ?