What are you supposed to do for this type of problem?

Question

A mixture of Ne and Ar gases at 353 K contains twice as many moles of Ne as of Ar and has a total mass of 47.0 g. If the density of the mixture is 4.11 g/L, what is the partial pressure (in atm) of Ne?

Answer 1

You use a variation of the ideal gas equation (PV=nRT)

Answer 2

You can use this trick:
obtain an average molecular weight of the mixture by

MWav =(2* MW of Ne + MW of Ar)/3
Establish a base of 1 liter of mixture
Use density=mass/Volume to calculate the mass
calculate the number of moles n=m/MWav

Calcucate the total pressure by using the ideal gas law.

PV=nRT

Now

Partial pressure of Ne + Partial pressure of Ar = total pressure

and
Partial pressure of Ne = 2Partial pressure of Ar

finally, Use your algebra knowlege

Answer 3

For starters, tell us the total pressure.