At which temperature does a $0.006\% \ w/V$ urea solution have an osmotic pressure of $0.0246 \ atm$ (in $K$)?

Calculate the molar mass of a solute at $300 \ K$ if $400 \ mg$ of it is dissolved in $300 \ mL$ of water to exert an osmotic pressure of $0.2 \ atm$. $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$

Which of the following pairs of solutions is isotonic?

The empirical formula of a non-electrolyte is $CH_{2}O$. $A$ solution containing $6 \ g$ of the compound exerts the same osmotic pressure as that of $0.05 \ M$ glucose solution at the same temperature. The molecular formula of the compound is

Calculate the amount of solute dissolved in $3 \ dm^3$ water having osmotic pressure $0.3 \ atm$ at $300 \ K$. (Molar mass of solute $= 108 \ g \ mol^{-1}, R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}$) (in $g$)

The osmotic pressure of a solution at $327^o C$ and concentration $C$ is $P$. The osmotic pressure of the same solution at $427^o C$ and concentration $C/2$ is $2$ bar. Then $P = ......$ bar.