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JEE MainChemistrySome Basic Concepts of Chemistry

Complete combustion of 1.80 g of an oxygen-containing organic compound yielded 2.64 g of carbon dioxide and 1.08 g of water. If the molar mass of the compound is 60 g/mol , its molecular formula is :

Options

  1. AC ₂ H ₄ O ₂
  2. BCH ₂ O
  3. CC ₃ H ₈ O
  4. DC ₂ H ₂ O ₂

Correct answer

A. C ₂ H ₄ O ₂

Step-by-step solution

First, calculate the mass of carbon and hydrogen in the given compound from the combustion products. Moles of CO ₂ produced = 2.64 44 = 0.06 mol Since each mole of CO ₂ contains one mole of carbon, moles of C = 0.06 mol . Mass of C = 0.06 12 = 0.72 g Moles of H ₂ O produced = 1.08 18 = 0.06 mol Since each mole of H ₂ O contains two moles of hydrogen, moles of H = 0.06 2 = 0.12 mol . Mass of H = 0.12 1 = 0.12 g The total mass of the compound is 1.80 g . By conservation of mass, the mass of oxygen in the compound is:

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