Question

Determine the empirical formula of a compound containing 47.37 grams of carbon, 10.59 grams of hydrogen, and 42.04 grams of oxygen.

In an experiment, the molar mass of the compound was determined to be 228.276 g/mol. What is the molecular formula of the compound?

For both questions, show your work or explain how you determined the formulas by giving specific values used in calculations.

Answer 1

. C3H8O2C 47.37 g ×1 mol= 3.944 mol3.944 mol= 1.501 mol × 2 = 3.002 mol ≈ 3 mol12.01 g 2.6275H 10.59 g ×1 mol= 10.506 mol10.506 mol= 3.998 mol × 2 = 7.996 mol ≈ 8 mol1.008 g 2.6275O 42.04 g ×1 mol= 2.6275 mol2.6275 mol= 1.000 mol × 2 = 2.000 mol ≈ 2 mol16.00 g 2.6275