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An ideal solution was prepared by dissol...

An ideal solution was prepared by dissolving some amount of cane sugar (non-volatile) in `0.9` moles of water. The solution was then cooled just below its freezing temperature `(271K)`, where some ice get separated out. The remaining aqueous solution registered a vapour pressure of 700 torr at `373 K`. Calculate the mass of ice separated out, if the molar heat of fusion of water is `96 kJ`.

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An ideal solution was prepared by dissolving some amount of can sugar (non-volatile) in 0.9 moles of water.The solution was then cooled just below its freezing temperature (271 K) where some ice get separated out.The remaining aqueous solution registered a vapour pressure of 700 torr at 373K.Calculate the mass of ice separated out, if the molar heat of fusion of water is 6 kJ.

Assertion:When a solution of non-volatile solute in water is cooled slightly below its freezing temperature, some ice separates out and then freezing stops. Reason: Separation of ice increases the molality of the left over solution.

The vapour pressure of a 5% aqueous solution of a non-volatile organic substances at 373K is 745 mm. calculate the molar mass of the solute. (Vapour pressure of water at 373K=760mm Hg).

A solution is prepared by dissolving 10g of non-volatile solute in 200g of water. It has a vapour pressure of 31.84 mm Hg at 308 K. Calculate the molar mass of the solute. (Vapour pressure of pure water at 308K =32 mm Hg)

A solution is prepared by dissolving 10g of non-volatile solute in 200g of water. It has a vapour pressure of 31.84 mm Hg at 308 K. Calculate the molar mass of the solute. (Vapour pressure of pure water at 308K =32 mm Hg)

A solution is prepared by dissolving 9.25 g of non volatile solute in 450 ml of water. It has an osmotic pressure of 350 mm of Hg at 27^(@)C . Assuming the solute is non-electrolyte, determine its molecular mass. (R = 0.0821 lit atm K^(-1)mol^(-1) )