A solution contains 15 g non-volatile non-electrolyte solute C6H14O6 dissolved in 500 g of water at 40 c.

Calculate
(A)Vapor pressure of the solution.
(B)Boiling point of the solution.
(C)Freezing point of the solution.

b. mols C6H14O6 = grams/molar mass.

Substitute mols into
molality = mols/kg solvent and solve for m, then substitute m into
delta T = Kb*m, solve for delta T and add to the normal boiling point for H2O.

c. Use calculation for mols and molality from above and substitute into
delta T = Kf*m and solve for delta T and subtract from normal freezing point of H2O.

a. Psoln = XH2O*PoH2O
where XH2O = mols H2O/total mols.

To calculate the vapor pressure, boiling point, and freezing point of the solution, we need to use colligative properties. Colligative properties are the properties of a solution that depend solely on the number of solute particles, not on their identity. The three colligative properties that we are interested in for this question are vapor pressure lowering, boiling point elevation, and freezing point depression.

Before we can calculate these properties, we need to find the mole fraction of the solute in the solution. The mole fraction, denoted by "X," is the ratio of the number of moles of solute to the total number of moles in the solution.

Step 1: Calculate the number of moles of solute (C6H14O6).
Given mass of solute = 15 g
Molar mass of C6H14O6 = 6(12.01 g/mol) + 14(1.01 g/mol) + 6(16.00 g/mol) = 180.22 g/mol
Number of moles of solute = mass of solute / molar mass of solute
= 15 g / 180.22 g/mol

Step 2: Calculate the number of moles of solvent (water).
Given mass of solvent = 500 g
Molar mass of H2O = 2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol
Number of moles of solvent = mass of solvent / molar mass of solvent
= 500 g / 18.02 g/mol

Step 3: Calculate the mole fraction of the solute.
Mole fraction of solute (X) = moles of solute / (moles of solute + moles of solvent)

Now, let's use the mole fraction to calculate the colligative properties.

(A) Vapor Pressure of the Solution:
The vapor pressure of a solution can be calculated using Raoult's Law. According to Raoult's Law, the vapor pressure of the solution is equal to the mole fraction of the solvent multiplied by the vapor pressure of the pure solvent.

Vapor pressure of pure water at 40°C = Known value (let's assume it to be P°)
Vapor pressure of the solution = X(solvent) * P°

(B) Boiling Point of the Solution:
The boiling point elevation can be calculated using the equation:

∆Tb = Kb * m

Where ∆Tb is the boiling point elevation, Kb is the molal boiling point constant for the solvent, and m is the molality of the solution.
Molality (m) = (moles of solute) / (mass of solvent in kg)

Boiling point of the solution = Boiling point of pure solvent + ∆Tb

(C) Freezing Point of the Solution:
The freezing point depression can be calculated using the equation:

∆Tf = Kf * m

Where ∆Tf is the freezing point depression, Kf is the molal freezing point constant for the solvent, and m is the molality of the solution.
Molality (m) = (moles of solute) / (mass of solvent in kg)

Freezing point of the solution = Freezing point of pure solvent - ∆Tf

To obtain the specific values for Kb and Kf, you may need to refer to a reference book or look them up online based on the solvent you are using.

Remember to convert the temperature from degrees Celsius to Kelvin when calculating the colligative properties.

Overall, these calculations will allow you to determine the vapor pressure, boiling point, and freezing point of the solution.