COMEDK 2024 Shift 2 Paper

To determine the osmotic pressure of the solution, we use the formula for osmotic pressure (π) given by:
π=i⋅C⋅R⋅T
Where:
i is the van 't Hoff factor (for non-electrolytes like glucose and urea, i=1 ).
C is the total molar concentration of the solute (in mol∕L ).
R is the gas constant (0.082L‌atm‌K‌‌−1‌mol−1).
T is the absolute temperature in Kelvin (K).
First, convert the given temperature to Kelvin:
T=27∘C+273=300K
Next, we need the molar concentration of each solute. Calculate the molar mass of glucose and urea:
For glucose (C6H12O6) :
‌ Molar mass ‌‌=6(12)+12(1)+6(16)
‌=72+12+96
‌=180g∕mol
For urea (NH2CONH2) :
‌=2(15)+12+16
‌=30+28
‌=60g∕mol
Now, calculate the number of moles of each solute:
For glucose:
‌ moles of glucose ‌=‌

3.6g

180g∕mol

=0.02‌mol
For urea:
‌ moles of urea ‌=‌

1.2g

60g∕mol

=0.02‌mol
The total volume of the solution is 200 ml or 0.2 L . So, the total molar concentration C of the solution is:
Finally, use the osmotic pressure formula:
Thus, the osmotic pressure of the solution is 4.92 atm . The correct answer is:
Option D: 4.92