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!?