The empirical formula of a compound is $C_2H_5O$ and its molecular weight is $90$. The molecular formula of the compound is:

The mass $\%$ of carbon in $C_{57}H_{110}O_6$ is

An organic compound contains $78\%$ (by $wt.$) carbon and the remaining percentage of hydrogen. The correct option for the empirical formula of this compound is: [Atomic $wt.$ of $C$ is $12$,$H$ is $1$]

An organic compound contains $69 \%$ carbon and $4.8 \%$ hydrogen,the remainder being oxygen. Calculate the masses of carbon dioxide and water produced when $0.20 \ g$ of this substance is subjected to complete combustion.

$A$ substance contains $52.2\%$ carbon,$13\%$ hydrogen,and $34.8\%$ oxygen. If the vapor density of the substance is $46$,find its molecular formula.

$0.102 \ g$ 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 $Ba = 137$]