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Complete combustion of 4.6 g of an oxygen-containing organic compound yields 8.8 g of CO ₂ and 5.4 g of H ₂ O . The vapour density of the compound is 23 . The number of moles of O ₂ gas required for the complete combustion of 2 moles of this compound is _______.

Correct answer

6

Step-by-step solution

First, we determine the mass of Carbon and Hydrogen in the organic compound. Moles of CO ₂ produced = 8.8 44 = 0.2 mol . Mass of Carbon = 0.2 12 = 2.4 g . Moles of H ₂ O produced = 5.4 18 = 0.3 mol . Moles of Hydrogen atoms = 0.3 2 = 0.6 mol . Mass of Hydrogen = 0.6 1 = 0.6 g . The total mass of the compound is 4.6 g . Mass of Oxygen in the compound = 4.6 - (2.4 + 0.6) = 1.6 g . Moles of Oxygen atoms = 1.6 16 = 0.1 mol . The mole ratio of C : H : O is 0.2 : 0.6 : 0.1 = 2 : 6 : 1 . The empirical formula is C ₂ H ₆ O

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