Practice question
Question
A 0.56 g sample of a hydrocarbon produces 1.76 g of CO₂ and 0.72 g of H₂O on complete combustion. What is its molecular formula if its molar mass is 56 g/mol? (Atomic masses: C = 12, H = 1, O = 16)
Explanation
Mass of C = (12/44) × 1.76 ≈ 0.48 g; mass of H = (2/18) × 0.72 = 0.08 g. Total = 0.56 g (matches). Moles: C = 0.48/12 = 0.04, H = 0.08/1 = 0.08; ratio = 1 : 2; empirical formula = CH₂, mass = 14 g/mol. n = 56/14 = 4; molecular formula = C₄H₈.
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