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 $O_2$?

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 $N = 14, Ar = 40$]

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?

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 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

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 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:

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?

Dalton's Law of Partial Pressures states that the total pressure of a gaseous mixture is equal to: