An organic compound contains $20.0\mathrm{\%}\mathrm{C}, 6.66\mathrm{\%}\mathrm{H}, 47.33\mathrm{\%} \mathrm{N}$ and the rest was oxygen. Its molar mass is $60 g {\mathrm{mol}}^{-1}$. The molecular formula of the compound is

$\mathrm{C}:\mathrm{N}:\mathrm{O}:\mathrm{H}::\frac{20}{12}:\frac{47.33}{14}:\frac{26.01}{16}:\frac{6.66}{1}::1.667:3.381:1.626:6.66::1:2:1:4$

Empirical formula ${\mathrm{CN}}_2{\mathrm{OH}}_4$

Molar empirical mass is $60 \mathrm{g} {\mathrm{mol}}^{-1}$( same as the given molar mass ). Hence, Molecular formula is ${\mathrm{CN}}_2{\mathrm{OH}}_4$.