An organic compound contains 49.3% carbon, 6.84% hydrogen and its vapors density is 73 Molecular formula of compound is

Explanation

Here's how to solve the problem to find the molecular formula of the organic compound:Calculate the percentage of oxygen:% of oxygen = 100% - % of carbon - % of hydrogen = 100% - 49.3% - 6.84% = 43.86%Calculate the empirical formula:Assume 100g of the compound. This gives:49.3 g carbon (C)6.84 g hydrogen (H)43.86 g oxygen (O)Divide each mass by its respective atomic mass and express the results in the smallest whole-number ratio:C: 49.3 g / 12.01 g/mol ≈ 4.11 ≈ 4H: 6.84 g / 1.008 g/mol ≈ 6.79 ≈ 7O: 43.86 g / 16.00 g/mol ≈ 2.74 ≈ 2Therefore, the empirical formula is C₄H₇O₂Relate the empirical formula to the molecular formula:The vapor density of the compound is 73 g/mol.The empirical formula weight (sum of atomic masses in the empirical formula) is approximately 4(12) + 7(1) + 2(16) = 73 g/mol.This means the empirical formula is also the molecular formula, as the vapor density matches the empirical formula weight.Therefore, the molecular formula of the compound is C₄H₇O₂.