Question

A gaseous hydrocarbon requires $6$ times its own volume of $O_2$ for complete oxidation and produces $4$ times its volume of $C{O}_2$ at same pressure and temperature. The formula of gas is :

• A. $C_4{H}_{10}$
• B. $C_4{H}_8$
• C. $C_4{H}_6$
• D. $C_8{H}_{16}$

Answer 1

The correct option is B $C_4{H}_8$

The balanced reaction is as follows:
$C_X{H}_Y+[X+\frac{Y}{4}]O_2\to XC{O}_2+\frac{Y}{2}{H}_{2}O$
Let, $a$ litres of $C_X{H}_Y$ be used.
$a[X+\frac{Y}{4}]=6a$
and given, $aX=4a$
Therefore, $X=4$ and $Y=8$
Hence, the gas is $C_4{H}_8$.