$18 \ g$ glucose (Molar mass $= 180 \ g/mol$) is dissolved in $100 \ mL$ of water at $300 \ K$. If $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$,what is the osmotic pressure of the solution (in $atm$)?

At a constant temperature,the osmotic pressure of a solution is.....

What is the concentration (in $g/L$) of a sugar solution $(mol. wt. = 342 \, g/mol)$ that is isotonic with a $6 \, g/L$ urea solution $(mol. wt. = 60 \, g/mol)$?

$A$ 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 $atm$)

At $300 \ K$,the osmotic pressure of a solution containing $36 \ g$ of glucose per liter is $4.98 \ bar$. If the osmotic pressure of the solution is $1.52 \ bar$ at the same temperature,what will be its concentration (in $M$)?

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 ......... $atm$.