Suppose we prepare an aqueous solution by dissolving different amounts of a particular solute in a solvent, then measure the vapor pressure of the solvent above the solution. The table below summarizes the data collected, at 25 degrees Celsius, in the experiment.

Mole Fraction (solvent)

Vapor Pressure (mm Hg)

1.0

23.600

.9

21.240

.8

18.880

.7

16.520

.6

14.160

.5

11.800

.4

9.440

.3

7.080

.2

4.720

.1

2.360

0

0

 

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Give me some responses to the questions below and I'll give you some extra credit.

SID#:

Laboratory Section:

1. What does it mean mol fraction of solvent is 1.0 in the table above?

2. What does it mean mol fraction of solvent is 0.8?

3. What happens to the vapor pressure of water above the solution as the mol fraction of solvent decreases?

4. Here is a plot of the data from the table above;

What kind of relationship exists between the vapor pressure above the solution and the mol fraction of solvent?

5. Why does the vapor pressure of water above the solution decrease as the mol fraction of solvent decreases?

6. Is there anything about the table that you feel you do not understand? List your concerns/questions.