1.2 g of organic compound of Kjeldalization liberates ammonia which consumes  $30c{m}^3$ of 1N  HCl. The percentage of nitrogen in the organic compound is.                         

Given : weight of the organic compound (w) =1.2 g

Amount of ammonia consumed $=30c{m}^3=30ml$

Normality of $HCl=1N$

The percentage of nitrogen evolved can be calculated using the formula :

$\begin{array}{l}\%N=\frac{1.4\times N\times V\left(ml\right)}{w\left(gm\right)}\\ \%N=\frac{1.4\times 1\times 30}{1.2}=35\%\end{array}$