1. Determine the empirical formula:

* Assume a 100 g sample: This makes the calculations easier. In a 100 g sample, you'll have 30.4 g of nitrogen (N) and 69.6 g of oxygen (O).

* Convert mass to moles:

* Moles of N = 30.4 g / 14.01 g/mol (molar mass of N) ≈ 2.17 mol

* Moles of O = 69.6 g / 16.00 g/mol (molar mass of O) ≈ 4.35 mol

* Find the simplest whole-number ratio: Divide both mole values by the smaller one (2.17 mol):

* N: 2.17 / 2.17 = 1

* O: 4.35 / 2.17 ≈ 2

* The empirical formula is NO₂.

2. Determine the molecular formula:

* Calculate the empirical formula mass: NO₂ has a mass of 14.01 g/mol + (2 x 16.00 g/mol) = 46.01 g/mol.

* Find the ratio between the molar mass and the empirical formula mass: 92.0 g/mol / 46.01 g/mol ≈ 2

* Multiply the subscripts in the empirical formula by this ratio: NO₂ * 2 = N₂O₄

Therefore, the molecular formula of the compound is N₂O₄.