$0.0833 \, mol$ of a carbohydrate with the empirical formula $CH_2O$ contains $1 \, g$ of hydrogen. What is the molecular formula of the carbohydrate?

On complete combustion,$1.0 \ g$ of an organic compound $(X)$ gave $1.46 \ g$ of $CO_2$ and $0.567 \ g$ of $H_2O$. The empirical formula mass of compound $(X)$ is $.......... \ g \ mol^{-1}$. (Given molar mass in $g \ mol^{-1}: C: 12, H: 1, O: 16$)

Two oxides of a metal $X$ contain $50 \%$ and $40 \%$ of oxygen respectively. If the formula of the first oxide is $XO_2$,then the formula of the second oxide is:

Complete combustion of $1.80 \, g$ of an oxygen-containing compound $(C_xH_yO_z)$ gave $2.64 \, g$ of $CO_2$ and $1.08 \, g$ of $H_2O$. The percentage of oxygen in the organic compound is

An organic compound containing $C$, $H$, and $O$ has $13.13 \% H$, $52.14 \% C$, and $34.73 \% O$. Its molar mass is $46.068 \ g/mol$. What are its empirical and molecular formulae?

The complete combustion of $0.492 \, g$ of an organic compound containing $'C'$,$'H'$,and $'O'$ gives $0.793 \, g$ of $CO_{2}$ and $0.442 \, g$ of $H_{2}O$. The percentage of oxygen composition in the organic compound is .... (nearest integer)