How many liters of anti-freeze ethylene glycol [Ch2(OH)Ch2(OH)] would you add to a car radiator containing 6.50 L of water if the coldest winter temperature in the area is -20 degree celcius? Calculate the boiling point of of this mixture. The density of th ethylene glycol is 1.11 g/ml. The k (f) of water is 1.86 /m and k(b) of water is 0.52 C/m. Please advise with steps included, thanks.
delta Tf = 0 -(-20) = 20 oC
Kf = 1.86 oC / m
delta Tf = Kf x molality
20 = 1.86 x molality
molality = 10.75 m
molality = moles of solute / mass of solvent
density of water = 1 g / mL
so mass of water = volume of water
10.75 = moles of solute / 6.50
69.89 = moles
mass of glycol = moles x molar mass
= 69.89 x 62
= 4333 g
mass of anti -freeze = 4333 g
delta Tb = Kb x molality
Tb - 100 = 0.52 x 10.75
Tb = 105.6 oC
boiling point = 105.6oC
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