Coolent used in car radiator is aqueous solution of ethylene glycol. In order to prevent the solution from freezing at `-0.3^(@)C`. How much ethylene glycol must be added to `5kg` of water? `(k_(f)=1.86Kkgmol^(-1))`

Water is used in car radiators. In winter season, ethylene glycol is added to water so that water may not freeze. Assuming ethylene glycol to be non-volatile, calculate minimum amount of ethylene glycol that must be added to 6.0 kg of water to prevent it from freezing at -0.3^(@)C . The molal depression constant of water is 1.86^(@) .

In a cold climate water gets frozen causing damage to radiator of a car. Ethylene glycol is used as an anifreezing agent. Calculate the amount of ethylene glycol to be added to 4 kg of water to prevent it from freezing at -6^(@) . ( K_(f) for water = 1.85 kg mol^(-1) )

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution , the change in freezing point of water (DeltaT_(f)) when 0.01 mole of sodium sulphate is dissociated in 1 kg of water is : ( K_(f) = 1.86 K kg mol^(-1) )

Calculate the freezing point depression expected for 0.0711 m aqueous solution of Na_(2)SO_(4) . If this solution actually freezes at -0.320 ^(@)C , what would be the value of Van't Hoff factor ? ( K_(f) for water is 1.86 ^(@)C mol^(-1) ) .

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 freezing point of a solution containing 50 cm^(3) of ethylene glycol in 50 g of water is found to be -34^(@)C . Assuming ideal behaviour, Calculate the density of ethylene glycol (K_(f) for water = 1.86 K kg mol^(-1) ).

When 36.0 g of a solute having the empirical formula CH_(2)O is dissovled in 1.20 kg of water, the solution freezes at -0.93^(@)C . What is the moleculer formula of the solute ? ( K_(f) = 1.86^(@)C kg mol^(-1) )

Ethylene glycol is used as an antifreeze agent. Calculate the amount of ethylene glycol to be added to 4 kg of water to prevent it from freezing at -6^(@)C.(K_(f)" for "HH_(2)O=1.85" K mol"^(-1)"kg")

Calculate the amount of ice that will separate out on cooling containing 50 g of ethylene glycol in 200 g of water to -9.3^(@)C (K_(f) for water = 1.86 K mol^(-1) kg )