Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.Use 100°C as the boiling point of water. A) 108°C B) 92°C C) 130°C D) 70°C E) 8.3°C

Question

Quizplus · Accepted Answer

First, we need to calculate the molality of the solution:

molality = moles of solute / mass of solvent (in kg)

We know that the mass of water is 500.0 g, which is 0.5 kg. To calculate the moles of solute, we need to convert the grams of ethylene glycol to moles:

moles of ethylene glycol = 500.0 g / 62.07 g/mol = 8.05 mol

Now we can calculate the molality:

molality = 8.05 mol / 0.5 kg = 16.1 mol/kg

Next, we can use the equation:

ΔTb = Kb * molality

where ΔTb is the boiling point elevation, and Kb is the boiling point elevation constant for water (which is 0.512°C/m for water). We can solve for ΔTb:

ΔTb = 0.512°C/m * 16.1 mol/kg = 8.24°C

This tells us that the boiling point of the solution will be 8.24°C above 100°C, the boiling point of pure water. Therefore, the boiling point of the solution is:

boiling point = 100°C + 8.24°C = 108.24°C

However, the answer choices are given in whole degrees, so we must round down to the nearest degree. Thus, the answer is:

Answer: A (108°C)

Calculate the Boiling Point of a Solution of 500