VAPOR PRESSURE AS A FUNCTION OF TEMPERATURE …

1 VAPOR PRESSURE AS A FUNCTION OF TEMPERATURE Objectives: (1) Observe and measure the change in the VAPOR PRESSURE (dependent variable) as a FUNCTION of TEMPERATURE (independent variable). (2) Analyze the experimental data to determine the normal boiling point and the heat of vaporization, Hvap, using the Clausius-Clapeyron equation. This laboratory covers material presented in section of the 9th Ed. of the Chang text. Introduction: The quantity of VAPOR above a liquid in a closed system increases with the TEMPERATURE of the system. The quantity of VAPOR can be measured as the VAPOR PRESSURE of the system. This relationship is pictorially shown in Figure 1.

2 Figure 1. Pictorial representation of the increased quantity of gas above a liquid as the system is heated. The relationship between VAPOR PRESSURE and TEMPERATURE can be understood in terms of molecules in the liquid escaping the attractive forces of the liquid to enter the gas phase. A measure of the liquid s molecular attraction is the heat of vaporization ( Hvap). A large Hvap would indicate strong attractive forces between molecules in the liquid phase. At a low TEMPERATURE few molecules have enough energy to overcome the intermolecular attractions of the liquid. As TEMPERATURE increases, a greater number of molecules have enough energy to escape the intermolecular forces of the liquid.

3 In Figure 2 the kinetic energy distribution for a low TEMPERATURE sample is shown by the blue trace and the blue shaded area indicates the fraction of molecules with enough energy to escape from the liquid. The red kinetic energy distribution is for a warmer sample and the larger red shaded area indicates the number of molecules with enough energy to escape the molecular attractions of the liquid at the higher TEMPERATURE . Figure 2. The plot shows the kinetic energy distribution for molecules at a low TEMPERATURE (blue trace) and at a higher TEMPERATURE (red trace). As TEMPERATURE increases, a greater fraction of the molecules have enough energy to escape the molecular attractions of the liquid.

4 For liquids the VAPOR PRESSURE as a FUNCTION of TEMPERATURE has an exponential behavior as shown in Figure 3. Figure 3. Plot of VAPOR PRESSURE vs. TEMPERATURE of a sample. The exponential behavior of VAPOR PRESSURE (P) as a FUNCTION of TEMPERATURE (T) is given by the exponential FUNCTION : P=Ae HvapRT() (1) A in the expression is an experimental constant that can be related to the normal boiling point, Hvap is the heat of vaporization of the liquid, and R is the gas constant, R = J/(K mol). The author of your text indicates a relationship between PRESSURE and TEMPERATURE that does not contain an exponential term. To remove an exponent from an expression the log FUNCTION (log or ln) can be used.

5 Taking the natural log (ln) of both sides of equation (1) gives: ln(P)=ln(A) HvapRT (2) This can be made to look like a straight-line equation similar to textbook equation by rearranging terms. ln(P)= HvapR1T+ ln(A) y = m x + b The textbook also nicely points out that this is the equation of a straight line if you plot ln(P), y, vs. 1/T, x, and the slope, m, is equivalent to Hvap/R. This equation is the Clausius-Clapeyron equation named after the German physicist Rudolf Clausius (1822 - 1888) and the French engineer Emil Clapeyron (1799 - 1864). This week in lab you will fit a set of VAPOR PRESSURE vs. TEMPERATURE data to the Clausius-Clapeyron equation to determine the heat of vaporization of an unknown liquid, shown in Figure 4.

6 Figure 4. The linear relationship between ln(P) vs 1/T comes from the Clausius-Clapeyron equation. Experimental Procedure: In measuring VAPOR PRESSURE vs. TEMPERATURE you will take advantage of the definition of boiling. Recall that boiling is defined as the TEMPERATURE of liquid at which the VAPOR PRESSURE is equal to the atmospheric PRESSURE . You will reduce the PRESSURE above a liquid using the vacuum system in the hood. By recording the TEMPERATURE and PRESSURE at which the liquid boils for several different external pressures, the plot in Figure 4 will be created for your unknown liquid. You must have on safety glasses for this experiment. Glass under vacuum is potentially hazardous.

7 A small crack in a glass vessel can result in an implosion of the vessel, dispersing small pieces of glass over a large area. Become familiar with the apparatus shown in Figure 5 and assembled in the hood. The fist thing to do is check the apparatus for air leaks. Fixing these leaks can be tedious. Figure 5. A schematic of the vacuum distillation apparatus Turn on the vacuum at the hood by opening the vacuum valve all the way and then close it about half a turn. Open the 3-way valve so that there is a PRESSURE drop in the system. The hood vacuum should pump the system to about 20 inches of Hg (in Hg). Close the 3-way valve so that the system is isolated from the vacuum.

8 This valve placement shown in Figure 5 will isolate the system from the atmosphere as well. Watch the gauge. It should remain stable, losing no more than 1 in Hg in two minutes. If the system is leaking you have some work to do. Finding leaks in vacuum systems is challenging. Obtain some vacuum grease from the TA and apply a small amount to the joints of the still. Reassemble the apparatus and try the vacuum test again. If a leak persists, discuss possible sources with your partners. Take pieces apart and reconstruct the system so that individual elements can be checked. If the system is vacuum tight, practice bleeding air slowly into the system to familiarize yourself with the 3-way stopcock.

9 Figure 6 shows the three operational modes of the stopcock. Work with it until you are able to increase and decrease the PRESSURE in your apparatus by one inch of Hg. It will take a while to master this. Keep practicing and let everyone in the group have a turn. Figure 6. Setting on the 3-way stopcock. Once your group is comfortable with controlling the PRESSURE of your apparatus, vent the system to the atmosphere and disconnect thermometer joint. Use a long-stem funnel to fill the round bottom flask in the heating mantel with 200 ml of the liquid to be studied. Add to the round bottom flask a stir bar. Fill the plastic container around the collection flask 2/3 full with water and ice to make a bath.

10 Gently apply a vacuum to the system with the 3-way stopcock. Eventually open the stopcock to full vacuum. The system should pump to about 20 in Hg on the vacuum gauge. The liquid in the round bottom flask is likely to bubble as the vacuum is initially applied, this is not boiling, but rather the outgassing of air dissolved in the liquid. This is the same phenomenon as the bubbles released in a soda pop when a bottle is first opened. This is Henry s law in action. Even though this looks like boiling, bubbles forming in a liquid, it is important to note the difference. Boiling is the formation of bubbles composed of gas molecules of the liquid (ex. acetone), while degassing consists of gas bubbles composed of N2 or CO2.