What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass?

• A. SClO2
• B. S2OCl
• C. SO2Cl
• D. SOCl2

Answer: (D)

Verified step by step guidance

1. Convert the given mass percentages of each element to moles by dividing each percentage by the respective atomic mass: sulfur (S) = 32.07 g/mol, oxygen (O) = 16.00 g/mol, and chlorine (Cl) = 35.45 g/mol. Use the formula: \(\text{moles} = \frac{\text{mass percentage}}{\text{atomic mass}}\).
2. Calculate the mole ratio of each element by dividing all mole values by the smallest number of moles obtained among the elements. This step normalizes the mole quantities to the smallest whole number ratio.
3. If any of the mole ratios are not close to whole numbers, multiply all ratios by the smallest integer that converts them into whole numbers (e.g., 1.5 would be multiplied by 2 to get 3).
4. Write the empirical formula by using the whole number mole ratios as subscripts for each element symbol in the order given or commonly accepted order (S, O, Cl).
5. Verify that the empirical formula matches the given options and corresponds to the mole ratios calculated.