`620g` ethylene glycol is added to `4kg` water in the radiator of a car.The amount (in `gm` ) of ice will separate out at `-6^(@)C` is `x times100` `(K_(f)=1.86Kkgmol^(-1))`.Find `x`

The boiling point elevation and freezing point depression of solutions have a number of partical applications. Ethylene glycol (CH_(2)OH-CH_(2)OH) is used in automobile radiatiors as an antifreeze because it lowers the freezing point of the coolant. The same substance also helps to prevent the radiator coolant from boiling away by elevating the boiling point. Ethylene glycol has low vapour pressure. We can also use glycerol as an antifreeze. In order for the boiling point elevation to occur, the solute must be non-volatile, but no such restriction applies to freezing point depression. For example, methanol (CH_(3)OH) , a fairly volatile liquid that boils only at 65^(@)C , is sometimes used as an antifreeze in automobile radiators. 620 g glycol is added to 4 kg water in the radiator of car. What amount of ice will separate out at -6^(@)C ?

75 g ethylene glycol is dissolved in 500 gram water. The solution is placed in a refrigerator maintained at a temperature of 263.7 K. What amount of ice will separate out at this temperature ? ( K_(f)" water"=1.86 K "mollality"^(-1) )

Calculate the mole fraction of solute in a dilute aqueous solution from which ice begins to separate out at -46^(@)C . ( K_(f) of H_(2)O = 1.86 K m^(-1) )

A 10 m solution of urea is cooled to -13.02^(@)C . What amount of urea will separate out if the mass of solution taken is 100 g ? [K_(f)("water") =1.86 Kkg mol^(-1)]

Find the freezing point of a glucose solution whose osmotic pressure at 25^(@)C is found to be 30 atm. K_(f) (water) = 1.86 kg mol^(-1)K .

45 g of ethylene glycol C_(2)H_(6)O_(2) is mixed with 600 g of water. Calculate (a) the freezing point depression and (b) the freezing point of solution. Given K_(f)=1.86 K kg mol^(-1) .

45 g of ethylene glycol C_(2)H_(4)O_(2) is mixed with 600 g of water. Calculate (a) the freezing point depression and (b) the freezing point of solution. Given K_(f)=1.86 K kg mol^(-1) .

1000 g of 1 molal aqueous solution of sucrose is cooled and maintained at -3.534^(@)C . Find out how much ice will separate out at this temperature. (K_(f) for water =1.86 k m^(-1) )

Some ethylene glycol HOCH_(2)CH_(2)OH is added to your car cooling system along with 5 kg of water .If the freezing point of water glycol solution is -15.0^(@)C what is the boiling point of the solution ? (k_(b)=0.52 kg mol^(-1) and k_(f)=1.86 kg mol^(-1) for water)

How much ethyl alcohol must be added to 1.00 L of water so that the solution will not freeze at -4^(@)F ? K_f of water = 1.86 ^(@)C/m