Final answer:
The empirical formula of an iron oxide compound with 0.250 mole of iron atoms and 0.375 mole of oxygen atoms is Fe2O3. This is determined by creating the simplest whole number ratio, which, in this case, is found by multiplying the iron to oxygen mole ratio by two.
Step-by-step explanation:
To determine the empirical formula of an iron oxide compound with 0.250 mole of iron atoms and 0.375 mole of oxygen atoms, we need to find the simplest whole number ratio between the moles of iron to oxygen. First, we divide both values by the smallest of the moles to normalize the ratio.
- Fe: 0.250 / 0.250 = 1
- O: 0.375 / 0.250 = 1.5
Since oxygen's mole ratio is not a whole number, we then multiply both ratios by the smallest number that converts them to whole numbers. Multiplying both by 2 gives us Fe2O3. Therefore, the empirical formula of the compound is Fe2O3.