$A$ compound contains $69.5\%$ oxygen and $30.5\%$ nitrogen and its molecular weight is $92$. The molecular formula of the compound is

An organic compound contains $60\ \%\ C$, $4.48\ \%\ H$, and $35.5\ \%\ O$. Its empirical formula is:

$A$ compound gave $80\%$ carbon and $20\%$ hydrogen on analysis. The compound is possibly

$0.5 \ g$ of an organic compound $(X)$ with $60 \%$ carbon will produce $........ \times 10^{-1} \ g$ of $CO_2$ on complete combustion.

$0.102 \ g$ of an organic compound $X$ was oxidised with fuming nitric acid. The resulting solution,after reaction with excess of aqueous $BaCl_2$,produced $0.233 \ g$ of $BaSO_4$ as a precipitate. Compound $X$ is likely to be: [Given: Atomic wt. of $Ba = 137$]

The empirical formula of a compound is $CH_2O$. If its molecular weight is $180$,what is the molecular formula of the compound?