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 $g$)

At a certain temperature,a $1.6 \%$ solution of an unknown substance is isotonic with a $2.4 \%$ solution of Urea. If both solutions have the same solvent and the same density of $1 \ g/cm^3$,what is the molecular mass of the unknown substance in $g/mol$? [Molecular mass of urea $= 60 \ g/mol$]

Which of the following has the highest osmotic pressure at $300 \, K$?

One mole each of urea,glucose,and sodium chloride were dissolved in one litre of water. Equal osmotic pressure will be produced by solutions of

The following solutions were prepared by dissolving $10 \ g$ of glucose $(C_{6}H_{12}O_{6})$ in $250 \ mL$ of water $(P_{1})$,$10 \ g$ of urea $(CH_{4}N_{2}O)$ in $250 \ mL$ of water $(P_{2})$,and $10 \ g$ of sucrose $(C_{12}H_{22}O_{11})$ in $250 \ mL$ of water $(P_{3})$. The right option for the decreasing order of osmotic pressure of these solutions is:

The osmotic pressure of $0.4\%$ urea solution is $1.66\ atm$ and that of a solution of sugar of $3.42\%$ is $2.46\ atm$. When both the solutions are mixed in equal volumes,then the osmotic pressure of the resultant solution will be ......... $atm$.