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:

An organic compound having molecular mass 60 u is found to contain $\text{C }=\text{ 2}0\%,\text{ H }=\text{ 6}.\text{67}\%\text{ and N }=\text{ 46}.\text{67}\%$ rest being oxygen. On heating, it gives ${\text{NH}}_{\text{3}}$along with solid residue. The solid residue gives violet colour with alkaline copper sulphate solution. The compound is

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.

To check the principle of multiple proportions, a series of pure binary compounds $\left({\mathrm{P}}_{\mathrm{m}}{\mathrm{Q}}_{\mathrm{n}}\right)$ were analysed and their composition is tabulated below. The correct option(s) is(are)

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?

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:

A compound contains $1.2\times {10}^{25}$ atoms of $\mathrm{A}$, $4.8\times {10}^{25}$ atoms of $\mathrm{B}$ and $2.4\times {10}^{25}$ atoms of $\mathrm{C}$.  Find the empirical formula of compound:

Determine the simplest formula of a compound containing $50\%$ of element$\mathrm{X}$ (atomic mass$=10$ ) and $50\%$ of the element $\mathrm{Y}$(atomic mass $=20$ ) by weight.

The empirical formula as well as molecular formula of water is ${\mathrm{H}}_2\mathrm{O}$.