Question

An organic compound containing carbon, hydrogen and oxygen contains $52.20$% carbon and $13.04$% hydrogen. Vapour density of the compound is $23$. Its molecular formula will be:

• A. $C_2{H}_{6}O$
• B. $C_3{H}_{8}O$
• C. $C_4{H}_{8}O$
• D. $C_5{H}_{10}O$

Answer 1

Answer: (A)

$C_2{H}_{6}O$

Percentage of $O$ is $34.76$.

$\therefore C:H:O=\frac{52.20}{12}:\frac{13.04}{1}:\frac{34.76}{16}=4.33:13:2.15=2:6:1$

Equivalent weight $=$ $46$

Molecular weight $=2\times 23=46$.

$x=\frac{46}{46}=1$

$\text{Molecular formula}=(\text{Empirical formula}{)}_x$

$\text{Molecular formula}=C_2{H}_{6}O$

So, the correct option is $A$