The osmotic pressure of a decimolar solution of urea at 27$°$ C is

Concentration of solution = C = 0.1 M ( $\therefore$ Decimolar solution)

Temperature = T=27+ 275 -300K

Osmotic pressure = $\mathrm{\pi }=$ CST

$=0.1\times 0.082\times 300\left(\therefore \mathrm{S}=0.0821 \mathrm{lit} \mathrm{atm} {\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}\right)$

$=2.463 \mathrm{atm}$

1atm= 1.013bar

$\mathrm{\pi }=2.463\times 1.013 \mathrm{bar}$

=2.49 bar