When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced. What is the empirical formula of the compound

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Quizplus · Accepted Answer

The empirical formula of the compound is CH₂O. This can be determined by calculating the moles of each element present in the compound. The moles of carbon are 1.64 g CO₂ / (44.01 g/mol CO₂) = 0.0373 mol C. The moles of hydrogen are 1.01 g H₂O / (18.02 g/mol H₂O) = 0.0561 mol H. The moles of oxygen are (0.860 g - 0.0373 mol C - 0.0561 mol H) / (16.00 g/mol O) = 0.0286 mol O. The empirical formula is therefore CH₂O.

When a 0860 G Sample of an Organic Compound Containing C, H