Final answer:
To find the empirical formula, convert the masses to moles using atomic weights. The ratio of moles of Na, S, and O in the compound is nearly 1:1:1.5, which leads to an empirical formula of Na2SO3.
Step-by-step explanation:
To find the empirical formula of the compound containing sodium, sulfur, and oxygen, we must first convert the given masses of each element to moles by using their atomic weights: sodium (Na) with an atomic weight of 22.99 g/mol, sulfur (S) with an atomic weight of 32.07 g/mol, and oxygen (O) with an atomic weight of 16.00 g/mol.
- For sodium:
9.2 g Na ÷ 22.99 g/mol = 0.400 moles Na
- For sulfur:
12.8 g S ÷ 32.07 g/mol = 0.399 moles S
- For oxygen:
9.6 g O ÷ 16.00 g/mol = 0.600 moles O
The mole ratio of Na to S to O is essentially 1:1:1.5 when we divide each mole quantity by the smallest number of moles, which in this case is around 0.4. However, we cannot have half an atom in an empirical formula, so we have to multiply each ratio by 2 to get whole numbers, resulting in a ratio of 2:2:3. This gives us the empirical formula of Na2SO3.
Therefore, the correct answer is c) Na2SO3.