When 0.424 g of finely divided iron is burned 0.606 g of reddish brown oxide is obtained what is the empirical formula of the oxide?

The mass of oxygen can be calculated by subtracting the mass of iron from the mass of the oxide: 0.606g - 0.424g = 0.182g. Next, convert the masses to moles using the molar masses of iron (Fe) and oxygen (O). The molar ratio between iron and oxygen in the oxide is approximately 1:1, so the empirical formula is FeO.