$A$ solution of sucrose (molar mass $= 342 \ g \ mol^{-1}$) is prepared by dissolving $68.4 \ g$ of it per litre of the solution. What is its osmotic pressure in $atm$ at $273 \ K$? (Given: $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

The osmotic pressure of a solution containing $34.2 \ g$ of cane sugar (molar mass = $342 \ g \ mol^{-1}$) in $1 \ L$ of solution at $20^{\circ} C$ is
(Given,$R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $atm$)

In an osmosis process,the volume of the solution:

Calculate the osmotic pressure of a $0.2 \ M$ aqueous solution of an electrolyte at $300 \ K$. If the van't Hoff factor is $1.6$,find the osmotic pressure. $\left[R=0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}\right]$ (in $atm$)

If a solution has an osmotic pressure of $0.82 \ bar$ at $27 \ ^oC$,find the concentration of such a solution. (in $M$)

$200 \ mL$ of an aqueous solution of a protein contains its $1.26 \ g$. The osmotic pressure of this solution at $300 \ K$ is found to be $2.57 \times 10^{-3} \ bar$. The molar mass of protein will be ......... $g \ mol^{-1}$.
$(R = 0.083 \ L \ bar \ mol^{-1} \ K^{-1})$