Final answer:
To find the empirical formula, assume a 100 g sample and calculate the moles of C, H, O, and N, then divide to get a whole number ratio. For the molecular formula, compare the empirical formula mass to the compound's molecular mass.
Step-by-step explanation:
To determine the empirical formula of the compound, we will assume a 100 g sample, which means we have 67.31 g of carbon (C), 6.98 g of hydrogen (H), 21.10 g of oxygen (O), and 4.62 g of nitrogen (N). Next, we divide these masses by the respective atomic masses to find the moles of each element. We then divide by the smallest number of moles to get the simplest whole number ratio.
To find the molecular formula, we compare the molecular mass of the empirical formula to the given relative molecular mass of the compound (303 g/mol). By dividing the molecular mass of the compound by the empirical formula mass, we can determine the number of empirical formula units in the molecular formula.