How to Calculate the Normal Boiling Point of Ethylene Glycol Solution?
What is the normal boiling point of ethylene glycol (C2H602) for the 34% solution and Kf = 1.86 (°C/m)?
Choose one:
- Tb=48.10
- Tb=77.50
- Tb=84.5C DOES NOT EXIST
- Tb=72.50
- Tb=88.6C
- Tb=64.30
- Tb=79.50
Answer:
The correct answer is Tb = 110.15 °C. The normal boiling point of a 34% solution of ethylene glycol (C2H6O2) can be calculated using the boiling point elevation equation.
The normal boiling point of ethylene glycol solution can be determined by calculating the boiling point elevation caused by the presence of the solute in the solution. In this case, a 34% solution of ethylene glycol is considered.
The normal boiling point of a solution is affected by the presence of solute particles. By using the boiling point elevation equation and the molal boiling point elevation constant (Kf = 1.86 °C/m), the normal boiling point can be determined.
To calculate the boiling point elevation, we need to find the molality of the solution, which involves determining the moles of the solute and the mass of the solvent. By using the moles of ethylene glycol and the mass of water, we can calculate the molality.
After finding the molality, we can use the boiling point elevation equation to calculate the boiling point elevation. The normal boiling point of a 34% solution of ethylene glycol can then be obtained by adding the calculated boiling point elevation to the normal boiling point of water.
Therefore, the correct answer to the normal boiling point of ethylene glycol (C2H602) for the 34% solution and Kf = 1.86 (°C/m) is Tb = 110.15 °C.