Answer:
-96.6°C
Explanation:
Given:
mass CCl4 = 530.0 g * (1 kg / 1000)
mass CCl4 = 0.5300 kg
First calculate the molality (m) of the solute, which is the moles of solute divided by the kg of solvent ([tex]\frac{moles}{kg}[/tex]):
molality CHCl3 = (mass moles CHCl3) / (mass CCl4 in kg)
molality CHCl3 = (1.31 mol) / (0.5300 kg)
molality CHCl3 = 2.471698m
Decrease in freezing point of solvent = (Kf) * (molality of solute)
Decrease in freezing point of CCl4 = (Kf) * (molality CHCl3)
Decrease in freezing point of CCl4 = (29.8°C/m) * (2.47m)
Decrease in freezing point of CCl4 = 73.6566°C
Then use the molality of the solute to calculate the change in freezing point and subtract the change from the original freezing point.
Freezing point of solution =
(freezing point of pure solvent) - (Decrease in freezing point)
Freezing point of solution = (-22.9°C) - (73.66°C)
Freezing point of solution = -96.6°C
Learn more about freezing point here: brainly.com/question/22888016
