Discussion
The osmotic pressure of 0.01 M aqueous solution of urea at 300 K is (R = 0.082 lit atm mol-1)
Answer: E
The osmotic pressure is 0.246 atm.
Urea does not ionise, so van 't Hoff's equation applies directly, \(\pi = CRT\), with R in L atm K-1 mol-1:
\[ \pi = 0.01 \times 0.082 \times 300 = 0.246\ \text{atm} \]
The value of R is printed with its kelvin unit missing, but 0.082 L atm K-1 mol-1 is the standard value. 2.46 and 24.6 atm are ten and a hundred times too large, as if the solution were 0.1 M or 1 M, and 0.0082 and 0.082 atm do not include the factor of 300 K.
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