$$200 \mathrm{ml}$$ of an aqueous solution contains $$3.6 \mathrm{~g}$$ of Glucose and $$1.2 \mathrm{~g}$$ of Urea maintained at a temperature equal to $$27^{\circ} \mathrm{C}$$. What is the Osmotic pressure of the solution in atmosphere units?

$$\mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}{ }^{-1} \mathrm{~mol}^{-1}$$ : Molecular Formula: Glucose is $$\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6$$ and of Urea is $$\mathrm{NH}_2 \mathrm{CONH}_2$$

$$\mathrm{K}_{\mathrm{H}}$$ for $$\mathrm{O}_2$$ at $$293 \mathrm{~K}$$ is $$34.86 \mathrm{~kbar}$$. What should be the partial pressure of $$\mathrm{O}_2$$ gas so that it has a solubility of $$0.08 \mathrm{~g} / \mathrm{L}$$ in water at $$293 \mathrm{~K}$$ ? (Density of solution $$=1 \mathrm{~g} / \mathrm{ml}$$)

What is the amount of ice that separates out on cooling a solution containing $$60 \mathrm{~g}$$ of Ethylene glycol in $$250 \mathrm{~g}$$ of water to $$-9.3^{\circ} \mathrm{C}$$ ? $$\mathrm{K}_{\mathrm{f}}$$ of $$\mathrm{H}_2 \mathrm{O}=1.86 \mathrm{~K} / \mathrm{m} ;$$ MM of ethylene glycol= $$62 \mathrm{~amu}$$

$$\text { If a compound } \mathrm{X}_3 \mathrm{Y} \text { is } 60 \% \text { ionised in aqueous medium, what is its van't Hoff factor value? }$$