An organic compound containing carbon, hydrogen, and oxygen has a vapour density of 44 . Complete combustion of 0.88 g of this compound produces 1.76 g of CO ₂ and 0.72 g of H ₂ O . The number of oxygen atoms present in one molecule of the compound is ________.

Step-by-step solution

Molar mass of the compound = 2 Vapour density = 2 44 = 88 g mol ⁻¹ Moles of the compound burnt = 0.88 88 = 0.01 mol Moles of CO ₂ produced = 1.76 44 = 0.04 mol Moles of carbon in 0.01 mol of compound = 0.04 mol Number of carbon atoms per molecule = 0.04 0.01 = 4 Moles of H ₂ O produced = 0.72 18 = 0.04 mol Moles of hydrogen in 0.01 mol of compound = 2 0.04 = 0.08 mol Number of hydrogen atoms per molecule = 0.08 0.01 = 8 Let the molecular formula be C ₄ H ₈ O _x . Molar mass = (4 12) + (8 1) + (x 16) = 88 48 + 8 + 1