The mole fraction of urea in an aqueous urea solution containing 900 g of water is 0.05. If the density of the solution is 1.2 g/cm^3, the molarity of urea solution is ______.

Correct option is A. 2.98
Mole fraction of urea in aqueous solution =0.05
0.05 = Moles of urea/(Moles of urea + 900/18)
0.05(Moles of urea) + 2.5 = Moles of urea
Moles of Urea = 2.63 moles
Mass of urea = 2.63 × 60 = 158 gm
Mass of solution = 158 + 900 = 1058 gm
Density = 1.2 g cm^3
Volume of solution = 1058/1.2= 881.67 ml
Molarity=n_solute/V_solution (in mL) × 1000
=2.63/881.67 × 1000
= 2.98 ≈ 3 M