An organic compound contains carbon,hydrogen,and oxygen. Its elemental analysis gives $38.71 \%$ of $C$ and $9.67 \%$ of $H$. The empirical formula of the compound would be $:-$

At $STP$,$2.8 \, L$ of a gaseous substance weighs $5.5 \, g$. If the compound contains $N$ and $O$ atoms,its molecular formula will be ..............

$0.5 \ g$ of hydrocarbon gave $0.9 \ g$ of water on combustion. The percentage of carbon in the hydrocarbon is:

The empirical formula of a compound is $CH_2O$ and its molecular weight is $120$. The molecular formula of the compound is:

The empirical formula of a carbohydrate is $CH_2O$. If $0.1 \, \text{mol}$ of this carbohydrate contains $1 \, g$ of hydrogen,what is its molecular formula?

Compound $A$ contains $8.7\,\%$ Hydrogen,$74\,\%$ Carbon and $17.3\,\%$ Nitrogen. The molecular formula of the compound is ....
Given : Atomic masses of $C$,$H$ and $N$ are $12$,$1$ and $14\, amu$ respectively.
The molar mass of the compound $A$ is $162\, g\, mol^{-1}$.