What is the empirical formula for a compound that contains 50.05% sulfur and 49.95% oxygen by mass?

• A. S_2O
• B. SO
• C. S_2O_3
• D. SO_2

Answer: (B)

Verified step by step guidance

1. Step 1: Assume you have 100 grams of the compound. This means you have 50.05 grams of sulfur (S) and 49.95 grams of oxygen (O).
2. Step 2: Convert the mass of each element to moles by dividing by their respective atomic masses. Use the atomic mass of sulfur as approximately 32.07 g/mol and oxygen as approximately 16.00 g/mol. Calculate moles of sulfur: \(\frac{50.05}{32.07}\) and moles of oxygen: \(\frac{49.95}{16.00}\).
3. Step 3: Determine the simplest whole number ratio of moles of sulfur to moles of oxygen by dividing both mole values by the smaller of the two mole amounts.
4. Step 4: If the ratio is not a whole number, multiply both numbers by the smallest factor that converts them into whole numbers (e.g., 2, 3, 4, etc.).
5. Step 5: Write the empirical formula using the whole number mole ratios as subscripts for sulfur and oxygen, respectively.