An organic compound containing C, H and O has 49.3% A carbon , 6.84% hydrogen and its vapour density is 73. Molecular formula of the compound is

$\text{ The empirical formula is }{\mathrm{C}}_3{\mathrm{H}}_5{\mathrm{O}}_2\text{. }$

Empirical formula weight = 3 x 12+ 5 x 1+ 2x 16 

                                    = 36+5+32=73

Molecular weight of the compound = 2x VD = 2x 73 = 146

$\mathrm{n}=\frac{\text{ mol. wt. }}{\text{ empirical formula wt. }}=\frac{146}{73}=2$

Molecular formula = Empirical formula x 2

                           = $\left({\mathrm{C}}_3{\mathrm{H}}_5{\mathrm{O}}_2\right) \times 2={\mathrm{C}}_6{\mathrm{H}}_{10}{\mathrm{O}}_4$