When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced. What is the empirical formula of the compound

Question

Quizplus · Accepted Answer

1. Find the number of moles of each product: - Moles of COS: 1.35 g / 60.07 g/mol = 0.02248 mol - Moles of H2O: 0.826 g / 18.02 g/mol = 0.04587 mol 2. Find the number of moles of sulfur in each product: - Moles of sulfur in COS: 2 x 0.02248 mol = 0.04496 mol - Moles of sulfur in H2SO4: 1 x 0.04587 mol = 0.04587 mol 3. Find the number of moles of carbon and hydrogen in the original compound: - Moles of carbon: 0.04496 mol (since there's only one carbon in the product) - Moles of hydrogen: (2 x 0.04496) + 0.04587 = 0.13579 mol 4. Find the empirical formula: - Divide the number of moles of each element by the smallest number of moles: - Carbon: 0.04496 mol / 0.04496 mol = 1 - Hydrogen: 0.13579 mol / 0.04496 mol = 3.021 - Sulfur: 0.04496 mol / 0.04496 mol = 1 - Oxygen: (0.04587 mol - 2 x 0.04496 mol) / 0.04496 mol = 0.989 - Round the values to the nearest whole number: - Carbon: 1 - Hydrogen: 3 - Sulfur: 1 - Oxygen: 1 - The empirical formula is therefore CH₃O. Choice D is the only one that matches.

When a 0952 G Sample of an Organic Compound Containing C, H