200 ml of an aqueous solution contains 3.6 ~g of Glucose and 1.2 ~g of Urea maintained at a temperature equal to 27^ C . What is the Osmotic pressure of the solution in atmosphere units? R =0.082 ~L ~atm ~K ⁻¹ ~mol ⁻¹ : Molecular Formula: Glucose is C ₆ H ₁₂ O ₆ and of Urea is NH ₂ CONH ₂

Step-by-step solution

The molar mass of Glucose ( C₆H₁₂O₆ ) is 6 12 + 12 1 + 6 16 = 180 g/mol . The molar mass of Urea ( NH₂CONH₂ ) is 14 + 2 + 12 + 16 + 14 + 2 = 60 g/mol . The number of moles of Glucose is n₁ = 3.6 180 = 0.02 mol . The number of moles of Urea is n₂ = 1.2 60 = 0.02 mol . The total number of moles of solute is n = n₁ + n₂ = 0.02 + 0.02 = 0.04 mol . The volume of the solution is V = 200 ml = 0.2 L . The temperature is T = 27^ C = 27 + 273 = 300 K . Using the osmotic pressure formula = CRT = n V RT , we have: = 0.04 0.2 0