2. The mass of an "empty" flask with its rubber stopper (the mass of air has already been subtracted) was 104.6164 g when placed on an analytical balance. A piece of dry ice was placed inside the flask and allowed to sublime. The flask, rubber stopper, and carbon dioxide gas were placed on the same balance and obtained a mass of 104.8959 g. a. What was the mass of the piece of dry ice? b. Convert this mass of dry ice (carbon dioxide) into moles of carbon dioxide. C. The volume of the flask was found to be 0.139 L. Calculate the molar volume using the moles determined in part 2b. (molar volume = L/moles of carbon dioxide)
2. The mass of an "empty" flask with its rubber stopper (the mass of air has already been subtracted) was 104.6164 g when placed on an analytical balance. A piece of dry ice was placed inside the flask and allowed to sublime. The flask, rubber stopper, and carbon dioxide gas were placed on the same balance and obtained a mass of 104.8959 g. a. What was the mass of the piece of dry ice? b. Convert this mass of dry ice (carbon dioxide) into moles of carbon dioxide. C. The volume of the flask was found to be 0.139 L. Calculate the molar volume using the moles determined in part 2b. (molar volume = L/moles of carbon dioxide)
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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Transcribed Image Text:2. The mass of an "empty" flask with its rubber stopper (the mass of air has already
been subtracted) was 104.6164 g when placed on an analytical balance. A piece of dry
ice was placed inside the flask and allowed to sublime. The flask, rubber stopper, and
carbon dioxide gas were placed on the same balance and obtained a mass of
104.8959 g.
a. What was the mass of the piece of dry ice?
b. Convert this mass of dry ice (carbon dioxide) into moles of carbon dioxide.
C. The volume of the flask was found to be 0.139 L. Calculate the molar volume
using the moles determined in part 2b.
(molar volume = L/moles of carbon dioxide)
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