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)

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

The partial pressure of a dry gas is:

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

A gaseous mixture of 2 moles of A, 3 moles of B, 5 moles of C and 10 moles of D is contained in a vessel. Assuming that gases are ideal and the partial pressure of $C$ is 1.5 atm, total pressure is

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 $N = 14, He = 4$]

In which one of the following does the given amount of chlorine exert the least pressure in a vessel of capacity $1\,\,{\rm{d}}{{\rm{m}}^3}{\rm{at}}273\,{\rm{K}}?$

If the total pressure of a mixture of two gases is 1 atm and the partial pressure of one gas is 0.4 atm, what is the mole fraction of the other gas?

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?

$32\,{\rm{g}}$ of oxygen and $3\,{\rm{g}}$ of hydrogen are mixed and kept in a vessel of $760\,{\rm{mm}}$ pressure and 0\,^\circ C. The total volume occupied by the mixture will be nearly:

Dalton’s law of partial pressure is applicable to which one of the following systems