Question

Find the osmotic pressure of $0.1M$ solution of urea at ${127}^{\circ }C$
$\text{Molecular formula of urea is}\left(C{H}_4{N}_{2}O\right)$

• A. $2.78atm$
• B. $5.56atm$
• C. $1.57atm$
• D. $3.28atm$

Answer 1

The correct option is D $3.28atm$

Osmotic pressure:

$\pi =C\times R\times T$

Here
$C\text{is concentration (Molarity)}\left(mol{L}^{-1}\right)R\text{is ideal gas constant}\left(Latmmo{l}^{-1}{K}^{-1}\right)T\text{is temperature (K)}$


$C=0.1mol{L}^{-1}R=0.0821Latmmo{l}^{-1}{K}^{-1}T={127}^{\circ }C=400K$

$\pi =(0.1\times 0.0821\times 400)atm\pi =3.284atm$