A mixture of CH2Cl2(l) and CHCl3(l) had a calculated vapor-pressure of solution to be 478 mmHg at room temperature. Upon conducting an experiment it was observed that this mixture had an actual vapor-pressure of solution to be 590 mmHg. What can be determined by these results?
Cannot relate forces of attraction to vapor-pressure of solution
The forces of attraction of the individual liquids is weaker than the forces of attraction in the mixture
The forces of attraction of the individual liquids is stronger than the forces of attraction in the mixture
The forces of attraction of the solution is weaker then predicted