HELP!!!

A gas mixture contains 1.35g N2 and 0.82g O2 in a 1.48-L container at 21∘C.

Calculate the partial pressure of O2 and N2

Question

HELP!!! 

A gas mixture contains 1.35g N2 and 0.82g O2 in a 1.48-L container at 21∘C.

Calculate the partial pressure of O2 and N2

anonymous · Answer

Are you given the total pressure?

anonymous · Answer

i have the mole fraction n2=.65 02=.35

anonymous · Answer

And they are not said to be in equilibrium?

anonymous · Answer

no

anonymous · Answer

Okay. I will try making my own assumptions and then if you manage confirm if are correct in case you have the marking scheme.

anonymous · Answer

Total pressure = nRT/V= 1*8.31*(21+273)/1.48*10^-3=1.65*10^6 Pa.
Partial pressure of x= mole of x*total pressure/total number of moles.
For n2= 0.65*1.65*10^6/1=962000Pa
For O2= 0.35*1.65*10^6/1= 518000Pa.