Molecular Weight of a Condesable Vapor

AP Chemistry Period 1 Molecular load of a Condensable Vapor Lab Purpose The purpose and objective of this laboratory was to find the molecular heaviness of a condensed vapor. Materials and Equipment Aluminum foil even up (around 6cm on a side) 125 mL flaskful Barometer 3 mL of unknown liquid 200 mL graduated cylinder 600 mL beaker Pin Balance (0. 002g) Bunsen Burner setup Rubber band Thermometer ceramic sharpen wire gauze Procedure 1. A 125 mL flask was obtained. The square of aluminum was fashioned all over the flask by laying the foil over the mouth and folding the sides down.A pin was indeed obtained and was used to poke a tiny hole in the center of the aluminum cap. 2. Next, the atomic reactor was determined of the clean, dry flask with the cap to 0. 001 g. 3. 3 mL of the unknown liquid was obtained and was poured into the flask. Afterwards the flask cap was replaced securely. 4. Then, a 600 mL beaker was then filled nearly large of water. The beaker was then modify to a boil over the Bunsen burner setup. 5. erstwhile the water reached a boil, the temperature was then recorded and the barometric pressure.Then the flask was clamped at the very outmatch and was suspended to the beaker. 6. The flask from the beaker was not removed and the flask was examined for excess vapor coming out through the pin hole to see a refraction effect. 7. When all of the liquid evaporated, the flask was removed by belongings the clamp and set aside to cool. 8. Next, the flask was wiped down until it was solely dry. 9. Then, the mass of flask, cap, and unknown condensed liquid was found. 10. The flask was filled on the whole full with water.The flask was then poured into a graduated cylinder and measured the volume. 11. Next, all the materials and chemicals were cleaned up. 12. Once the area was clean, the calculations could be completed. Observations The flask in spite of appearance the beaker full of water was being examined. As the water surrounding the fla sk began to boil, droplets started to form on the inside of the flask. After a while, nothing could be seen forming in the flask. When this happened, the droplets evaporated and inside the flask was the condensed vapor. Calculations 1. Questions 2.What does the flask contain? a. The flask contains air before adding the volatile liquid. b. The flask contains all vapor at the point when the volatile liquid has completely vaporized. c. The flask contains condensed vapor and air at the end of the try and at the final weighing. 3. Why is the temperature of boiling water used for measuring the volume of the vapor instead of the temperature of the liquid after it has cooled to room temperature? Instead of pickings the temperature of the gas, the temperature of the boiling water was taken and was transferred. . When vaporized, the volatile liquids used in this experiment do not behave exactly as ideal gases. How would this list to affect your calculated molecular weight? The molecular we ight was littler than expected. This happened because the density was smaller due to the mass being smaller and this meant in addition much vapor fly the flask. Conclusion In this experiment, the molecular weight of a condensed vapor was found through a procedure exploitation an unknown liquid. The flask before adding the unknown liquid in was full of air.After the beaker full of water started to boil the flask was examined until the unknown liquid was completely vaporized. At that exact point the flask contained all vapor. At the final weighing the flask contained condensed vapor and air. There is always a come up for error. Some sources of error could have come with completing this lab over an open water bath and some water vapor whitethorn have been in place. Also, too much vapor could have escaped and the experiment might not have been stopped quick enough.