If the partial pressures of gases in a mixture are 20 kPa, 30 kPa, and 50 kPa, what is the total pressure exerted by the mixture according to Dalton's Law?

A container holds 2 moles of helium and 3 moles of neon at a total pressure of 15 atm. What is the partial pressure of helium?

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?

Dalton’s law of partial pressure is not applicable to

A container holds a mixture of $N_2$ and $He$ gases. It contains $14$ g of $N_2$ and $2$ g of $He$. If the total pressure is $18$ bar, calculate the partial pressure of $N_2$. [Use atomic masses $N = 14, He = 4$]

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:

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?

In a scuba tank, $0.1$ moles of $He$ are mixed with $0.4$ moles of $N_2$. If the total pressure in the tank is $20$ atm, determine the partial pressure exerted by the $N_2$ gas. [Use atomic masses $He = 4, N = 14$]

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

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

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)