To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent antifreeze) (density 1.11 g/mL) and water were mixed. Assume that ethylene glycol does not dissociate and has a formula, C2H6O2.
Assume 2 L of solution
Volume of ethylene glycol = 1 L
Mass of ethylene glycol = volume x density
= 1000 mL x 1.11 g/mL = 1110 g = 1.11 kg
Moles of ethylene glycol = mass/molecular weight
= 1110g / 62g/mol = 17.9 mol
Mass of water = 1000 mL x 1g/ml = 1000g = 1 kg
Freezing point depression
ΔT = i Kf m
i = the number of dissolved particles (Van't Hoff Factor)= 1
Kf = molal freezing point depression constant of the solvent = 1.86 °C/m for water
m = molality = moles of solute / kg of solvent
= 17.9/1 = 17.9 moles /kg
ΔT = 1 x 1.86 x 17.9 = 33.3 °C
Tf° - Tf = 33.3 °C
Tf° = freezing point of pure solvent = 0°C
Tf = freezing point of solution
Tf = - 33.3°C
Below this temperature the solution in the radiator will freeze.
This is the minimum temperature would a radiator be protected.
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