How many grams of glucose must be added to $0.5 \ L$ of a solution so that its osmotic pressure is same as that of a solution of $9.2 \ g$ of glucose dissolved in a liter?

Calculate the mass of a non-volatile solute dissolved in $0.3 \text{ dm}^3$ of water, which has an osmotic pressure of $0.1 \text{ atm}$ at $300 \text{ K}$. [Molar mass of solute = $328 \text{ g mol}^{-1}$, $R = 0.082 \text{ dm}^3 \text{atm K}^{-1} \text{mol}^{-1}$] (in $\text{ g}$)

Calculate the osmotic pressure exerted by a solution containing $0.822 \ g$ of solute in $300 \ mL$ of water at $300 \ K$. (Molar mass of solute $= 340 \ g \ mol^{-1}, R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1}$) (in $atm$)

Which of the following solutions has the maximum osmotic pressure?

At $27^{\circ}C$,a solution containing $2.5 \ g$ of solute in $250.0 \ mL$ of solution exerts an osmotic pressure of $400 \ Pa$. The molar mass of the solute is $.............. \ g \ mol^{-1}$ (Nearest integer) (Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

At $17^\circ C$,the osmotic pressure of an aqueous solution of sucrose $(C_{12}H_{22}O_{11})$ containing $34.2 \ g/L$ is $P$. What concentration of glucose $(C_6H_{12}O_6)$ in $g/L$ would be isotonic with this solution?