If $0.0833 \, \text{mol}$ of a carbohydrate contains $1 \, \text{g}$ of hydrogen and its empirical formula is $CH_2O$,what is its molecular formula?

$A$ compound $X$ contains $32 \%$ of $A$,$20 \%$ of $B$,and the remaining percentage of $C$. Then,the empirical formula of $X$ is:
(Given atomic masses of $A = 64$,$B = 40$,$C = 32 \ u$)

An organic compound contains $C = 38.8\%$,$H = 16\%$ and $N = 45.2\%$. The empirical formula of the compound is:

Analysis of a $60 \, g$ compound gives $C = 24 \, g$,$H = 4 \, g$,and $O = 32 \, g$. What is its empirical formula?

The elemental composition of a compound is $54.2 \% C$,$9.2 \% H$,and $36.6 \% O$. If the molar mass of the compound is $132 \ g \ mol^{-1}$,the molecular formula of the compound is: [Given: The relative atomic mass of $C:H:O = 12:1:16$]

An organic compound containing carbon and hydrogen has an empirical formula of $CH_2$. The mass of $1 \ L$ of this organic gas is equal to the mass of $1 \ L$ of $N_2$ gas at the same temperature and pressure. What is the molecular formula of the organic gas?