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 $atm$)

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:

The osmotic pressure of equimolar solutions of $BaCl_2$,$NaCl$,and glucose follows the order:

What is the molar mass of a solute if a solution is prepared by dissolving $4.5 \ g$ of solute in $3 \ dm^3$ of water having an osmotic pressure of $0.25 \ atm$ at $300 \ K$? $(R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1})$

Find the amount of solute in a solution obtained by dissolving it in $2.5 \ dm^3$ of water that generates an osmotic pressure of $0.245 \ atm$ at $300 \ K$. (Molar mass of solute $= 58 \ g \ mol^{-1}$,$R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}$) (in $g$)

$1.46 \, g$ of a biopolymer dissolved in a $100 \, mL$ water at $300 \, K$ exerted an osmotic pressure of $2.42 \times 10^{-3} \, bar$.
The molar mass of the biopolymer is $..... \times 10^{4} \, g \, mol^{-1}$. (Round off to the Nearest Integer)
[Use : $R = 0.083 \, L \, bar \, mol^{-1} \, K^{-1}$ ]