1. Determine the moles of each element:

* Nitrogen (N):

* Molar mass of N = 14.01 g/mol

* Moles of N = 6.08 g / 14.01 g/mol = 0.434 mol

* Oxygen (O):

* Molar mass of O = 16.00 g/mol

* Moles of O = 13.92 g / 16.00 g/mol = 0.870 mol

2. Find the mole ratio:

* Divide the moles of each element by the smallest number of moles (0.434 mol in this case):

* N: 0.434 mol / 0.434 mol = 1

* O: 0.870 mol / 0.434 mol ≈ 2

3. Determine the empirical formula:

* The mole ratio indicates that the compound has 1 nitrogen atom for every 2 oxygen atoms.

* The empirical formula is N₂O₄, which is dinitrogen tetroxide.

Important Note: Dinitrogen tetroxide is a highly reactive compound. In the real world, it's likely to be in equilibrium with nitrogen dioxide (NO₂).