$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right)+400\mathrm{kJ}$
$\mathrm{C}\left(\mathrm{s}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to \mathrm{CO}\left(\mathrm{g}\right)+100\mathrm{kJ}$
When coal of purity 60% is allowed to burn in presence of insufficient oxygen, 60% of carbonis converted into 'CO' and the remaining is converted into 'CO'.
The heat generated when 0.6 kg of coal is burnt is ______.

$\begin{array}{l}\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right)+400\mathrm{kJ}\\ 1\mathrm{g}\text{ mole }\\ \mathrm{C}\left(\mathrm{s}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to \mathrm{CO}\left(\mathrm{g}\right)+100\mathrm{kJ}\\ 0.6\times 1000\\ =600\mathrm{gm}\\ 600\times \frac{60}{100}\text{ (Pure Carbon) }\\ =360\mathrm{gm}=\frac{360}{12}=30\text{ mole (Pure Carbon) }\end{array}$
Carbon converted into ${\mathrm{CO}}_2=\left(30-30\times \frac{60}{100}\right)$
= 12 mole
and carbon converted in CO $=30\times \frac{60}{100}=18\text{ mole }$
Energy generated during II equation
$\begin{array}{r}=18\times 100\\ =1800\mathrm{kJ}\end{array}$
Energy generated During 1st reaction
$\begin{array}{l}=12\times 400\\ =4800\\ \text{ Total }=1800+4800=6600\mathrm{kJ}\end{array}$