When 0 . 01 mol of an organic compound containing 60 % carbon was burnt completely, 4 . 4   g of CO 2…

Let $\mathrm{M}$ is the molar mass of the compound $\left(\mathrm{g}/\mathrm{mol}\right)$
mass of compound $=\mathrm{mole} \times \mathrm{molecular} \mathrm{mass} = 0.01\mathrm{M} \mathrm{g}$

mass of carbon $=0.01\mathrm{M}\times \frac{60}{100}$ ....(i)

moles of carbon $=\frac{\mathrm{mass} \mathrm{of} \mathrm{compound}}{\mathrm{molecular} \mathrm{mass} \mathrm{of} \mathrm{carbon}} = \frac{0.01\mathrm{M}}{12}\times \frac{60}{100}$  ....(ii)

Thus, moles of ${\mathrm{CO}}_2$ from combustion $=\frac{4.4}{44}=$0.1 moles of carbon dioxide

Using POAC,
Thus, from (i) and (ii),
$\Rightarrow \frac{0.01\mathrm{M}}{12}\times \frac{60}{100}=\frac{4.4}{44}$

$\Rightarrow \mathrm{M}=\frac{4.4}{44}\times \frac{100}{60}\times \frac{12}{0.01}=200 \mathrm{g}/\mathrm{mol}$