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?

The partial pressure of a dry gas is:

A container holds a mixture of $He$ and $Ne$ gases. The partial pressure of $He$ is 0.3 atm, and its mole fraction is 0.6. If 0.2 moles of $Ar$ is added to the mixture while keeping the temperature and volume constant, what will be the total pressure of the resulting mixture?

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 :

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 mixture of ${{\rm{N}}_{\rm{2}}}$ and ${\rm{Ar}}$ gases in a cylinder contains ${\rm{7 g}}$of ${{\rm{N}}_{\rm{2}}}$ and ${\rm{8 g}}$ of ${\rm{Ar}}$. If the total pressure of the mixture of the gases in the cylinder is ${\rm{27}}$ bar, the partial pressure of ${{\rm{N}}_{\rm{2}}}$ is :

[Use atomic masses ${\rm{N = 14,}}\,{\rm{Ar}}\,{\rm{ = 40}}$]

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

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 contains 56 g of ${N_2}$, 44 g of $C{O_2}$ and 16 g of $C{H_4}$. The total pressure of mixture is 720 mm of Hg. The partial pressure of methane is

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?

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?