Question

Suppose you have a liquid solution containing two components, acetone and nonane. The boiling point of pure acetone is 56 C and the boiling point of pure nonane is 151 C. Your solution has a mole fraction of component acetone equal to 0.1, and the solution behaves as an ideal solution. What is the boiling point of this solution?

Answer 1

The boiling point is somewhere between 56 and 151 °C

Step-by-step explanation:

Hello,

In this case, it is possible to compute it via rigorous methods in phase equilibrium by using for example a cubic equation of state to model the vapor phase and a suitable excess Gibbs free energy model for the liquid phase, nonetheless, it is an arduous task. In such a way, since the information about both acetone's and nonane's pure boiling points is given as well as acetone's mole fraction, which points out it is about a binary liquid solution, one could make up the boiling point is somewhere between 56 and 151 °C precising that it should be closer to 151 °C as the mixture is 90% nonane and 10% acetone.

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