In case of osmosis,solvent molecules move from:

Calculate the molar mass of a non-electrolyte solute when $6 \text{ g}$ of it is dissolved in $1 \text{ dm}^3$ of water, having an osmotic pressure of $2.4 \text{ atm}$ at $300 \text{ K}$ $(R = 0.0821 \text{ atm dm}^3 \text{ K}^{-1} \text{ mol}^{-1})$.

One mole each of urea,glucose,and sodium chloride were dissolved in one litre of water. Equal osmotic pressure will be produced by solutions of

Explain: What is osmosis? Give examples.

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: $(R = 0.083 \text{ L bar mol}^{-1} \text{ K}^{-1})$

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 $\text{ g}$)