Verified answer

moles N2: 1.19 g/28 g/mole=0.0425

moles O2: 0.90 g/ 32 g/mole=0.0281

total moles=0.0706

mole fraction N2: 0.0425/0.0706= 0.6, therefore mole fraction O2= 0.4

N2: 0.6 x 1.63 L=0.978 L

O2: 0.4 x 1.63 L=0.652

I see the question and think, PV=nRT will be involved.

First thing is

Solve for n moles of each element. Periodic table

now you have n(O2) and n(N2)

Add them to get n(total)

mole fraction of N2 = n(N2)/n(total)

mole fraction of O2 = n(O2)/n(total)

note that mole fraction of N2 and mole fraction of O2 add up to 1.

Solve PV=nRT for P and ...

P=nRT/V

This give you the total pressure, P(total).

The partial pressure of the two gasses, P(N2) and P(O2) sum to P(total).

P(N2)=mole fraction of N2 time P(total) = X-N2 x P(total)

That'll do for now... lets see if you can finish.

Good luck