Question

What is the change in the freezing point of a solution made by dissolving 14.7 g of C₆H₁₂O₆ into 150.0 ml of water? the density of water is 1.00 g/ml and k f

It seems like the question got cut off. I'll provide a general multiple-choice format, and you can fill in the blanks with the appropriate options:
a) ΔTf = -1.86°C
b) ΔTf = +1.86°C
c) ΔTf = -0.465°C
d) ΔTf = +0.465°C

Answer 1

To calculate the change in freezing point of a solution upon dissolving glucose, the molality of the solution is needed, which is determined from the mass of glucose and the mass of the water solvent. The freezing point depression constant (Kf) and the formula ΔTf = Kf x m are then used to find the change. However, the exact value of Kf is missing in the question, so the final freezing point cannot be determined without additional information.

option a is the correct

Step-by-step explanation:

The question is asking for the change in freezing point resulting from dissolving a nonvolatile solute, specifically glucose (C6H12O6), in water. Using the formula ΔTf = Kf x m, where ΔTf is the change in freezing point, Kf is the freezing point depression constant (-1.86°C/m for water), and m is the molality of the solution, we can calculate the change in freezing point for the dissolution of 14.7 g of glucose into 150.0 ml of water. To determine the molality, we must first calculate the number of moles of glucose and then the mass of the solvent in kilograms.

Here are the steps to answer the question:

1. Find the molar mass of glucose (C6H12O6) to convert grams to moles.
2. Calculate the number of moles of glucose using its molar mass.
3. Since the density of water is 1.00 g/ml, convert 150 ml of water to its mass in kilograms.
4. Calculate molality (moles of solute per kilogram of solvent).
5. Use the equation ΔTf = Kf x m to calculate the change in freezing point.
6. Subtract the freezing point change from the freezing point of pure water which is 0.0°C to get the new freezing point of the solution.

Without the exact value of the freezing point depression constant (Kf) provided in the original question, we cannot proceed to obtain a numerical answer. Hence, the multiple-choice answers and further calculation steps provided in the question prompt cannot be completed accurately.

Typically, for such types of calculations, the assumption is that the solute doesn't dissociate and that the solvent's properties are not significantly altered by the addition of the solute, meaning the solution behaves ideally.