Ethylene glycol (molar mass = 62 g mol ^(-1)) is a common automobile antifreeze. Calculate the freezing point of a solution containing 12.4 of this substance in 100 g of water. Would it be advisable to keep this substance in the car radiator during summer? (K_(f) for water= 1.86 k kg//mol) (K_(b) for water = 0.512 K kg//mol.)

Ethylene glycol (molar mass = 62 g mol ^(-1)) is a common automobile a

1.	Ethylene glycol (molar mass = 62 g mol ^(-1)) is a common automobile antifreeze. Calculate the freezing point of a solution containing 12.4 of this substance in 100 g of water. Would it be advisable to keep this substance in the car radiator during summer? (K_(f) for water= 1.86 k kg//mol) (K_(b) for water = 0.512 K kg//mol.)
Answer» SOLUTION :`Delta T_(b) = K _(b) xx (W_(B))/(M _(B)) xx ( 1000 )/( W _(A)) = 0.512 xx (12.4)/(62) xx (100)/(100) = 1. 024 K` Since WATER boils at `100^(@)C,` so a solution CONTAINING ethylene glycol will boil at `101.024 ^(@)C,` so it is advisable to keep this substance in car RADIATOR during summer.