The relationship between osmotic pressure at 273 K when 10 g glucose (P₁), 10 g urea (P₂), and 10 g sucrose (P3) is dissolved in 250 ml of water is 

We know that the osmotic pressure is given by Π=iMRT

where i is the Van't Hoff factor

           M is the molarity

           R=0.08206 $\mathrm{L}\text{-atm }{\mathrm{mol}}^{-1}{ \mathrm{K}}^{-1}$ is the gas constant

           T is the absolute temperature

Π∝M

We also know that Molarity is inversely proportional to molecular weight.

Molecular weight of glucose=180, urea=60, sucrose=342.

And Osmotic pressure is also inversely proportional to molecular weight.

P1=Osmotic pressure of glucose (10 g)

P2=Osmotic pressure of urea (10 g)

P3=Osmotic pressure of sucrose (10 g)

So, P2>P1>P3

Therefore, option C is the correct answer