What is the osmotic pressure (in $atm$) of $0.02 \ M$ aqueous glucose solution at $300 \ K$?
$(R=0.082 \ L \ atm \ mol^{-1} \ K^{-1})$

The relationship between osmotic pressure at $273 \ K$ when $10 \ g$ glucose $(P_1)$,$10 \ g$ urea $(P_2)$,and $10 \ g$ sucrose $(P_3)$ are dissolved in $250 \ mL$ of water is:

$A$ solution is prepared by dissolving $0.3 \ g$ of a non-volatile non-electrolyte solute '$A$' of molar mass $60 \ g \ mol^{-1}$ and $0.9 \ g$ of a non-volatile non-electrolyte solute '$B$' of molar mass $180 \ g \ mol^{-1}$ in $100 \ mL$ $H_2O$ at $27^{\circ}C$. Osmotic pressure of the solution will be
[Given: $R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$] (in $atm$)

What is the osmotic pressure of a solution prepared by dissolving $3 \ g$ of solute in $2 \ dm^3$ of water at $300 \ K$ (in $atm$)? (Molar mass of solute $= 60 \ g \ mol^{-1}$,$R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}$)

$15 \%$ aqueous solution of glucose (molecular weight $= 180 \ g/mol$) is isotonic with $8 \%$ aqueous solution containing an unknown non-dissociable solute. What is the molecular weight of the unknown solute?

When $10 \ g$ of glucose $(P_1)$,$10 \ g$ of urea $(P_2)$,and $10 \ g$ of sucrose $(P_3)$ are dissolved in $250 \ mL$ of water,what is the relationship between their osmotic pressures at $273 \ K$?