partial pressure question?

Question

Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct?

a) it is equal to 1/3 the total pressure
b) it depends on the intermolecular forces of attraction between molecules of X, Y, and Z
c) it depends on the relative molecular masses of X, Y, and Z
d) it depends on the average distance traveled between molecular collisions
e) it can be calculated with knowledge only of the volume of the container

Thankss

Answer 1

C. It depends on the relative molecular masses of the 3 gases. The partial pressure that IDEAL gases exert on a container is proportional to their mole fraction not the mass fraction. In other words, it is proportional to the amount of molecules (or moles) of each gas in the container. For ideal gases the partial pressures add up to the total pressure.

Answer 2

Ans. a)....At STP, as 1 mole of all Ideal gases, each occupies a volume 22.4 litres.
Then a mixture of equal masses of 3 Ideal Gases will each make up 1/3rd of 22.4 Litres and therefore 1/3rd of the total pressure. (Almost forgot...Each gas will also have an equal No. of molecules).
IT IS A FACT THAT 1 MOLE OF ALL IDEAL GASES CONTAIN THE SAME NUMBER OF MOLECULES PER 22.4 LITRES

Answer 3

c is true.