A sealed container with a volume of 1 L contains a mixture of $O_2$ and $N_2$ at a total pressure of 2 atm and 27°C. The mole fraction of $O_2$ is 0.4. If the temperature is increased to 127°C, what will be the new partial pressure of $O_2$?

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:

A mixture of $N_2$ and $O_2$ gases has a total pressure of 1.2 atm. If the partial pressure of $N_2$ is 0.8 atm and the volume of the container is halved while maintaining a constant temperature, what will be the new partial pressure of $O_2$?

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:

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.

Two gases, A and B, are present in a container with partial pressures of 200 mmHg and 300 mmHg respectively. If another gas, C, is added to the container and the total pressure becomes 700 mmHg, what is the partial pressure of gas C?

Equal masses of nitrogen and ethylene are mixed in an empty container at 27\,^\circ C. The total pressure exerted by the gaseous mixture is $1\,\,{\rm{atm}}$. The partial pressure exerted by ethylene gas is :

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 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?

${O_2}$ 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 ?