When $10 \ g$ of glucose (osmotic pressure $P_1$),$10 \ g$ of urea (osmotic pressure $P_2$),and $10 \ g$ of sucrose (osmotic pressure $P_3$) are dissolved in $250 \ mL$ of water,the correct relationship between the osmotic pressures of these solutions is:

Which particles can pass through a semipermeable membrane?

At $27\,^oC$,the osmotic pressure of a solution containing $36\,g$ of glucose per liter is $4.92\,atm$. If the osmotic pressure of the solution is adjusted to $1.5\,atm$ at the same temperature,what will be its concentration?

At $300 \ K$, a one litre solution of sucrose (molecular weight: $342$) was prepared by dissolving $40 \ g$ of sucrose. What is the approximate osmotic pressure (in $kPa$) of the solution at the same temperature? $(R = 8.314 \times 10^6 \ cm^3 \ Pa \ K^{-1} \ mol^{-1})$

Pure water can be obtained from sea water by

Solution $A$ is prepared by dissolving $1 \text{ g}$ of a protein (molar mass = $50000 \text{ g mol}^{-1}$) in $0.5 \text{ L}$ of water at $300 \text{ K}$. Its osmotic pressure is $x \text{ bar}$. Solution $B$ is made by dissolving $2 \text{ g}$ of the same protein in $1 \text{ L}$ of water at $300 \text{ K}$. The osmotic pressure of solution $B$ is $y \text{ bar}$. The entire solution of $A$ is mixed with the entire solution of $B$ at the same temperature. The osmotic pressure of the resultant solution is $z \text{ bar}$. $x, y$ and $z$ respectively are: $(R = 0.083 \text{ L bar mol}^{-1} \text{ K}^{-1})$