When 0.01 mol of an organic compound containing 60% carbon was burnt completely, 4.4g of $C{O}_2$ was produced. The molar mass of compound is $gmo{l}^{-1}$  (Nearest integer)

Let M is the molar mass of the compound (g/mol) 
mass of compound = 0.01M gm.  
Mass of carbon  = 0.01M  $\times \frac{60}{100}$
Moles of $C{O}_2$ from combustion $=\frac{4.4}{44}=molesof$ carbon
 $\frac{0.01M}{12}\times \frac{60}{100}=\frac{4.4}{44}$
 $M=\frac{4.4}{44}\times \frac{100}{60}\times \frac{12}{0.01}=200gm/mol$