2. Calculate the average volume of the flask using the data from your three measurements. Use this average value to calculate the molar mass of your volatile liquid for each of your three trials of mass determination. (Don't forget to convert your temperature to the absolute scale.)

2. Calculate the average volume of the flask using the data from your three measurements. Use this average value to calculate the molar mass of your volatile liquid for each of your three trials of mass determination. (Don't forget to convert your temperature to the absolute scale.)

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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Question

Procedure
You are given an UNKNOWN VOLATILE LIQUID. You put 5 mL in a weighed flask tightly capped
with a piece of aluminum foil with a pinhole.
This is heated in a boiling water bath, until the vapors completely displace all the air, and all of the
liquid has evaporated.
The pin is replaced. The flask is then cooled to recondense the vapors and weighed.
The exact volume of the flask is also determined.
Data
Atmospheric pressure 23.94 inch Hg
Trial
Water
Initial mass of
Final mass of
Volume of the
Temperature
(degrees Celsius)
flask, pin and foil
(g)
flask, foil, pin and
recondensed
Erlenmeyer Flask
(mL)
volatile liquid (g)
83.79g
84.23g
84.02g
95 C
83.15g
83.24g
83.3g
1
146mL
2
95 C
148mL
3
95 C
147mL
Avg. 147mL
Questions
2. Calculate the average volume of the flask using the data from your three measurements. Use
this average value to calculate the molar mass of your volatile liquid for each of your three trials
of mass determination. (Don't forget to convert your temperature to the absolute scale.)
3. Calculate the average molar mass from your three trials. Calculate the standard deviation in
your value for molar mass. (See the popcorn experiment for the equation)
4. Explain why the pin must be replaced into the pinhole during cooling of the flask.
5. Due to the fact that the liquid you used was a volatile one, it will not completely recondense.
Some of the liquid remains in the vapor phase, even at room temperature. If you were able
to correct for this by making the vapors recondense completely, would your final molar
mass value be greater than, less than or the same as the value you determined? Explain your
reasoning.

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