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(C) The formula for osmotic pressure $(\pi)$ is $\pi = CRT$,where $C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature in

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$249$

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(C) The formula for osmotic pressure $(\pi)$ is $\pi = CRT$,where $C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature in Kelvin.Given: $\pi = 0.4 \ bar$,$w = 4 \ g$,$V = 1.0 \ L$,$R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$,$T = 27 + 273 = 300 \ K$.The molar concentration $C = \frac{n}{V} = \frac{w}{M 	imes V}$,where $M$ is the molar mass.Substituting the values: $0.4 = \frac{4}{M 	imes 1.0} 	imes 0.083 	imes 300$.$0.4 = \frac{4 	imes 0.083 	imes 300}{M}$.$M = \frac{4 	imes 0.083 	imes 300}{0.4} = \frac{99.6}{0.4} = 249 \ g \ mol^{-1}$.

At $27^{\circ} C$,the osmotic pressure of a solution containing $4 \ g$ of a non-electrolyte solute in $1.0 \ L$ of solution is $0.4 \ bar$. The molar mass of the solute in $g \ mol^{-1}$ is :
$(R=0.083 \ L \ bar \ K^{-1} \ mol^{-1})$

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At $27^{\circ} C$,the osmotic pressure of a solution containing $4 \ g$ of a non-electrolyte solute in $1.0 \ L$ of solution is $0.4 \ bar$. The molar mass of the solute in $g \ mol^{-1}$ is :$(R=0.083 \ L \ bar \ K^{-1} \ mol^{-1})$