## Help with finding molecular formula at a specific P, V, T

1. The problem statement, all variables and given/known data
A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25 g sample of the gas occupies a volume of 1.00 L and and exerts a pressure of 1.26 atm at -4.0C. Which of the following is its molecular formula?

Variables:
30.4% Nitrogen
69.6% Oxygen
M(sample)= 5.25g
P= 1.26 atm
V= 1.00 L
T= -4.0C = 269K

2. Relevant equations
PV= nRT

3. The attempt at a solution
1. I found the mass of each gas in the compound using the given % by mass.
I got:
mass of N2= .304*5.25= 1.596g
mass of O2= 5.25 - 1.596= 3.654g
2. I found the mol of each gas in the compound using the above masses convert to mol.
I got:
mol of N2 = 0.0570 mol
mol of O2 = 0.114 mol

That's all I have tried, but I stuck here, I didn't know what to do next, even not sure what I have tried was right. Can anyone help, please!?

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