The approximate molar mass of a volatile liquid can be determined by:1. Heating a sample of the liquid in a flask with a tiny hole at the top, which converts the liquid into gas that may escape through the hole2. Removing the flask from heat at the instant when the last bit of liquid becomes gas, at which time the flask will be filled with only gaseous sample at ambient pressure3. Sealing the flask and permitting the gaseous sample to condense to liquid, and then weighing the flask to determine the sample’s mass as shown. 895 16.895 12Figure 9.19 When the volatile liquid in the flask is heated past its boiling point, it becomes gas and drivesair out of the flask. At t1– g the flask is filled with volatile liquid gas at the same pressure as theatmosphere. If the flask is then cooled to room temperature, the gas condenses and the mass of the gasthat filled the flask, and is now liquid, can be measured. (credit: modification of work by Mark Ott)Using this procedure, a sample of chloroform gas weighing 0.494 g is collected in a flask with a volume of129 cm at 99.6 °C when the atmospheric pressure is 742.1 mm Hg. What is the approximate molar mass ofchloroform?

The variables of a gas are related by Ideal gas equation,PV=nRTP is pressureV is volumeR is gas…

Answered: 895 16. 895 12 Figure 9.19 When the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The approximate molar mass of a volatile liquid can be determined by:
1. Heating a sample of the liquid in a flask with a tiny hole at the top, which converts the liquid into gas that may escape through the hole
2. Removing the flask from heat at the instant when the last bit of liquid becomes gas, at which time the flask will be filled with only gaseous sample at ambient pressure
3. Sealing the flask and permitting the gaseous sample to condense to liquid, and then weighing the flask to determine the sample’s mass as shown.

895 16.
895 12
Figure 9.19 When the volatile liquid in the flask is heated past its boiling point, it becomes gas and drives
air out of the flask. At t1– g the flask is filled with volatile liquid gas at the same pressure as the
atmosphere. If the flask is then cooled to room temperature, the gas condenses and the mass of the gas
that filled the flask, and is now liquid, can be measured. (credit: modification of work by Mark Ott)
Using this procedure, a sample of chloroform gas weighing 0.494 g is collected in a flask with a volume of
129 cm at 99.6 °C when the atmospheric pressure is 742.1 mm Hg. What is the approximate molar mass of
chloroform?

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