Final answer:
To determine the empirical formula of a compound containing 50.05% sulfur and 49.95% oxygen by mass, convert the mass percentages to moles using the molar masses of sulfur and oxygen, then simplify to the smallest whole numbers to find the formula, which could be SO if the ratio is 1:1.
Step-by-step explanation:
The question requires us to determine the empirical formula of a compound with a given mass percent composition of sulfur and oxygen. The empirical formula of a compound represents the simplest whole number ratio of the elements present.
To find the empirical formula, assume we have 100 grams of the substance so that the percentages translate directly into grams. For sulfur (S), we have 50.05 grams, and for oxygen (O), we have 49.95 grams. Next, we convert the masses to moles by using the molar masses of the elements (S = 32.07 g/mol and O = 16.00 g/mol):
- Moles of S = 50.05 g / 32.07 g/mol
- Moles of O = 49.95 g / 16.00 g/mol
The resulting ratio of moles of S to O must be simplified to smallest whole numbers to get the empirical formula. If the smallest whole number ratio is 1:1, then the empirical formula is SO.