To determine the osmotic pressure of the solution, we use the formula for osmotic pressure
(Ï€) given by:
Ï€=iâ‹…Câ‹…Râ‹…TWhere:
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∕molFor urea
(NH2CONH2) :
‌ Molar mass ‌‌=2(14‌ for ‌N+1‌ for ‌H)+12‌ for ‌C+16‌ for ‌O
‌=2(15)+12+16‌=30+28‌=60g∕mol Now, calculate the number of moles of each solute:
For glucose:
‌ moles of glucose ‌=‌=0.02‌molFor urea:
‌ moles of urea ‌=‌=0.02‌molThe 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:
π=1⋅0.2‌mol∕L⋅0.082L‌atm‌K−1‌mol−1⋅300K=4.92‌atm
Thus, the osmotic pressure of the solution is 4.92 atm . The correct answer is:
Option D: 4.92