Empirical and Molecular Formulae

An organic compound A contains $69.77\%$ carbon, $11.63\%$ hydrogen and the rest is oxygen. The molecular mass of the compound is $86$. It does not reduce Tollen’s reagent but forms an addition product with sodium hydrogen sulphite and gives positive iodoform test. On vigorous oxidation it gives ethanoic and propanoic acids. The compound A is:

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

A certain hydrocarbon $\mathrm{A}$was found to contain $85.7$ percent carbon and $14.3$ percent hydrogen. This compound consumes $1 \mathrm{molar}$ equivalent of hydrogen to give a saturated hydrocarbon $\mathrm{B}$. $1.00 \mathrm{g}$ of hydrocarbon $\mathrm{A}$just decolourised $38.05 \mathrm{g}$ of a $5$ percent solution (by weight) of ${\mathrm{Br}}_2\mathrm{in}\mathrm{CC}{\mathrm{l}}_4.$ Compound $\mathrm{A}$, on oxidation with concentrated ${\mathrm{KMnO}}_4,$ gave compound $\mathrm{C}$(molecular formula, ${\mathrm{C}}_4{\mathrm{H}}_8\mathrm{O}$ ) and acetic acid. The compound $\mathrm{C}$could easily be prepared by the action of acidic aqueous mercuric sulphate on $2-$butyne. The molecular formula of $\mathrm{A}, \mathrm{B} \mathrm{and} \mathrm{C}$ are.

$9$ volumes of gaseous mixture consisting of gaseous organic compound A and just sufficient amount of ${\mathrm{O}}_2$ required for complete combustion yielded on burning $4$ volumes of ${\mathrm{CO}}_2$, $6$ volumes of water vapour and $2$ volumes of ${\mathrm{N}}_2$. All volumes measured at the same temperature and pressure. If the compound $\mathrm{A}$ contained only $\mathrm{C}, \mathrm{H} \text{and} \mathrm{N}$. What is the molecular formula of the compound $\mathrm{A}$? 

The silver salt of a certain organic acid with the atomic ratio $\mathrm{C}:\mathrm{H}:\mathrm{O}$ as $2:3:2$ contains $65.06\%$ of silver. If acid is dibasic, the formula of the acid is:

An organic compound on analysis gave the following results: $\mathrm{C}=54.5\%$, $\mathrm{O}=36.4\%$, $\mathrm{H}=9.1\%$. The Empirical formula of the compound is:

The pair of species having same percentage of carbon is -

A compound contains $4.07\%$ hydrogen, $24.25\%$ carbon and $71.75\%$ chlorine. What is its empirical formula?

What is the empirical formula of the salt? 

In an ionic compound moles ratio of cation to anion is $1:2$. If atomic masses of metal and non-metal respectively are $138$ and $19$, then correct statement is:

Which of the following is true about empirical formula and molecular formula?

Elements $\mathrm{X}$ and $\mathrm{Y}$ can combine to form two different compounds. If $1.6 \mathrm{g}$ of $\mathrm{X}$ reacts with exactly $1.6 \mathrm{g}$ of $\mathrm{Y}$, the compound produced has formula ${\mathrm{XY}}_2$. However under different condition, $2.4 \mathrm{g}$ of $\mathrm{X}$ will react with $1.6 \mathrm{g}$ of $\mathrm{Y}$ to form a second compound, whose empirical formula is-

For fixed mass of nitrogen in its two oxides $\mathrm{A}$ and $\mathrm{B}$ mass ratio of oxygen is $1 : 3$. If in $\mathrm{A}, 7 \mathrm{g}$ of $\mathrm{N}$ combines with $4 \mathrm{g}$ of oxygen, then empirical formula of $\mathrm{B}$ will be: