Name: ______________________________________________________ Date: _________ Period: ____
Molar Mass of a Volatile Liquid
Background
The molar masses of compounds are used daily in the chemistry
profession. The molar mass is defined as the mass, in grams, of 1 mole of any
element or compound. How is molar mass determined and how is the molar
mass of an unknown found? In this experiment, the molar mass of a volatile
liquid will be determined based on measurements of vapor density.
The ideal gas law relates the four measurable properties of a gas (P, V, n,
T). In this experiment, the ideal gas law will be used to determine the molar
mass of gases and nonvolatile liquids.
PV = nRT
Equation 1
The number of moles (n) of any pure substance is equal to the mass of the
substance divided by the molar mass of the substance.
n = mass/molar mass
Equation 2
Substituting for n in Equation 1 and then rearranging produce the equation for
the molar mass of a gas.
molar mass = mass (g) x RT
PxV
Equation 3
The molar mass of an unknown volatile liquid with a boiling point well below
the boiling point of water will be determined. A small sample of the liquid will
be placed in a tared 125 mL erlynmeyer flask and the flask will be heated in
boiling water to vaporize the liquid. The air and excess vapor escape, leaving
the flask filled only with the volatile liquid vapor at atmospheric pressure and
at the temperature of boiling water. The flask is removed and cooled to
condense the vapor. Once cooled, the flask is weighed. By massing the same
flask filled with distilled water, the volume of the flask is calculated. The molar
mass of the volatile liquid is then determined from Equation 3 using the mass
of the condensed vapor, the volume of the flask, the atmospheric pressure, and
the temperature of the boiling water.
Pre-Lab Questions
Read the entire procedure carefully before beginning the exercise.
1) A determination of the molar mass of methyl alcohol (CH3OH) yielded the
following data:
Temperature of boiling water bath
Barometric pressure
Temperature of room temp. water bath
Density of water at room temp.
Mass of empty flask
Mass of flask and condensed methyl alcohol
Mass of flask and water
Mass of condensed methyl alcohol
Mass of water in filled pipet
Volume of pipet
Molar mass of methyl alcohol (experimental)
Molar mass of methyl alcohol (theoretical)
99.5oC
738 mm Hg
24.0oC
0.9973 g/mL
Trial 1
1.557 g
1.571 g
16.001 g
Using the data, fill in the rest of the table. The volume of the flask is equal to
the volume of water in the flask. Use the relationship of mass and density to
determine this volume. Once the volume of the pipet is determined, equation
3 in the Background section can be used to calculate the molar mass of methyl
alcohol. Compare this value to the actual molar mass of methyl alcohol.
2) In this lab, you will be asked to identify an unknown volatile liquid. The
liquid must be one of the following compounds. Determine the molar mass of
each of the possible unknown liquids.
Compound
acetone
methanol (CH3OH)
ethanol (C2H5OH)
isopropanol (C3H7OH)
Molar Mass (g/mol)
Materials
Chemicals:
Unknown volatile liquid
Deionized water
Equipment
125 mL erlynmeyer flask
Rubber stopper to fit flask
Eyedropper or glass tubing to fit in rubber stopper
Thermometer
Milligram balance
Barometer
Boiling chips
1 L beaker
Hot plate
Ring stand
Clamp
Procedure
1) Place a 1 L beaker on the hot plate and add about 500 mL water to the
beaker, along with several boiling chips. Turn on the hot plate to boil the
water.
2) Obtain a 125 mL erlynmeyer flask and rubber stopper with glass tubing.
Mass the flask and stopper apparatus to the nearest 0.001 g. Record the
mass in Data Table 1.
3) Place 5.00 mL of an unknown volatile liquid in the bottom of the erlynmeyer
flask.
4) Place the rubber stopper in the erlynmeyer flask and mark the bottom of the
stopper.
5) Clamp the flask as high up on the neck as possible and slowly lower the
flask into the boiling water. Lower the clamp until it touches the lip of the
beaker. Clamp in place. (Do not inhale the vapor from the flask.)
6)
Continue heating about two minutes after all the liquid in the flask has
evaporated. The vapor will force the air from the flask, which will finally
contain only the vapor.
7) During this period, take the temperature of the water, placing the bulb of
the thermometer on a level with the middle of the flask.
8) Take the flask out of the water and, while it is still warm, wipe it and the
outside surface of the foil dry. Allow the flask to cool for 10 minutes with
the rubber stopper still in place.
9) Weigh the assembly and its contents.
10) Record the atmospheric pressure. The total pressure of the gases in the
flask is equal to this.
11) Remove the rubber stopper and fill the flask to the line where you marked
the bottom of the stopper with water, making certain there are no bubbles of
air trapped in it.
12) Dry the outside of the flask and then mass the flask and water. Record the
mass in the data table.
13) If time permits, repeat the experiment.
Data Analysis
1) Determine the mass of condensed, volatile vapor. Enter this value in the
data table.
2) Using the information provided, determine the density of water placed in the
flask. Use this value and the mass of water in the flask to calculate the
volume of the flask.
3) Determine the mass of the condensed volatile liquid.
4) Identify the unknown volatile liquid.
5) Calculate the percent error of your calculated molar mass.
Conclusion
1) Volatile liquids with lower boiling points often give better results than those
with higher boiling points. Suggest a reason for this.
2) What effect would vapor condensing in the neck of the flask have on the
reported molar mass? How large an error might this introduce?
3) Did all of the vapor condense into the liquid? If not, how would this affect
the calculated molar mass?
4) Why is not necessary to be precise when the liquid is measured out into the
test tube?
Data Tables
Table 1.
Temperature of boiling water
Barometric pressure
Temperature of water in flask when measuring volume
Density of water in the flask
Mass of empty flask with rubber stopper
Mass of flask and water
Mass of water in flask
Volume of flask
Table 2.
Mass of flask and condensed liquid
Mass of condensed liquid
Molar mass of unknown liquid
Density of Water
Vapor Pressure of Water
Temperature Density
Vapor
Pressure
oC
g/mL
torr
15
0.9991026
12.79
16
0.9989460
13.64
17
0.9987779
14.54
18
0.9985986
15.49
19
0.9984082
16.49
20
0.9982071
17.55
21
0.9979955
18.66
22
0.9977735
19.84
23
0.9975415
21.09
24
0.9972995
22.40
25
0.9970479
23.78
26
0.9967867
25.24
27
0.9965162
26.77
28
0.9962365
28.38
29
0.9959478
30.08
30
0.9956502
31.86