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Related questions

Molar Mass of a Vapor

Unknown liquid number: 1

Mass of flask + cap + rubber band: 74.00 g

Temperature of boiling water: 99.5oC

Barometric pressure: 771 mm Hg

Mass of flask + rubber band + cap + condensed vapor: 74.38 g

Mass of condensed liquid: 0.38 g

Volume of flask: 146 mL

Molar mass of vapor: _____ 

Questions

1. If an insufficient amount of liquid unknown had been used, how would this have affected the value of the experimental molar mass?

2. What are the major sources of error in your determination of the molar mass?

3. If the flask was not thoroughly wiped dry, how would this affect the molar mass?

4. Isobutyl alcohol has a boiling point of 108 oC. How would you modify the procedure used in this experiment to determine its molar mass?

In this experiment, a flask is filled with vapor( fastened by a piece of aluminum foil over the opening), by boiling a volatile unknown liquid in the flask. As it boils away, the vapor of the unknown pushes the aire out of the flask through a tiny pinhole opening, and eventually the flask is filled witha an atmosphere composed exlcusively of the unknown. The P, V, and T of the vapor will be determined and number of moles will be c alculated. When the flask is allowed to cool the vapor condenses and aire again refulls the flask. Re weighing the flask and figure out the the wight of the unknown vapor which filled the flask during the boiling.

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