1. If grams of the vapor of a volatile liquid can fill a 498 ml flask at o C and 775 mm Hg, what is the molecular mass of the gas?

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1 MOLECULAR MASS OFA VOLATILE LIQUID A lab to study the ideal gas law Introduction The ideal gas law indicates that the observed properties of a gas sample are directly related to the number of moles of gas sample in the container. For a given pressure, volume and temperature there is a set number of moles that will be present. If we can measure the number of grams of gas present in a container and calculate the number of moles present, the molecular mass of the gas can be determined. In this lab, we will use a highly volatile liquid and study its properties as a gas. A small amount of liquid will be placed in a flask and heated until it completely evaporates. Once it fills the flask, we can measure its temperature (it will be immersed in boiling water), pressure (same as the pressure in the lab at that time), and volume (by filling the flask). Once the sample is allowed to cool, the gas will recondense and the mass of the sample needed to fill the flask can be found. Using the ideal gas law, PV=nRT, and the data recorded, the molecular mass of the volatile liquid can be determined. Prelab questions: 1. If grams of the vapor of a volatile liquid can fill a 498 ml flask at o C and 775 mm Hg, what is the molecular mass of the gas? 2. What is the density of the gas at the time of collection?

2 Set-up an adapted Dumas method: Ring Thermometer And Test Tube Clamp Al foil cap with SMALL pinholesecured with a rubber band 125 ml Erlenmeyer flask Volatile Liquidenough to cover the bottom of flask 600 ml beaker Hot Plate MOLECULAR MASS OFA VOLATILE LIQUID 1. Place a small pinhole in the Al foil square. 2. Assemble the pictured apparatus a clean, dry 125 ml Erlenmeyer flask, fitted with the Al foil square containing the pinhole. Carefully secure it over the mouth of the Erlenmeyer flask with the rubber band. 3. On an analytical balance, weigh (_.xxxx g) the apparatus assembled in step 2.

3 4. Partially fill (about 3 4) a clean 600 ml beaker with water (tap water is fine) and place it on a hot plate. Bring the water just to boiling. 5. Meanwhile, remove the rubber band and foil cap from the Erlenmeyer flask, and place 4-5 ml of the volatile liquid in the Erlenmeyer flask - the exact amount is not important as long it completely covers the bottom of the flask. Then replace the foil cap and rubber band. 6. Once the water in the beaker is brought to boiling, remove the Bunsen burner and clamp the assembled apparatus to the ring stand by its neck with the test tube clamp. [The amount of water in the beaker can be adjusted such that when the final set-up is fully assembled, the Erlenmeyer flask is submerged up to its neck just an inch or so below the top - in the water bath in the beaker.] 7. Using a second test tube clamp, secure a thermometer and position it in the water bath in the beaker such that it can monitor the water bath temperature without touching either the sides of the beaker nor the Erlenmeyer flask. 8. Return the hot plate beneath the set-up and gently maintain such that the thermometer registers a steady temperature somewhere between 85 o C and 95 o C. It should not be boiling. Be sure that the Erlenmeyer flask is submerged up to its neck. 10. The volatile liquid should steadily begin to vaporize. You can monitor the escaping excess vapor by looking at its vapor trail as it exits the pinhole. [Another way to monitor the escaping vapor is to place the blade of the spatula over the pinhole and notice the condensation like your breath on a mirror.] 11. When you notice the vapor trail has ceased to escape from the pinhole, remove the Bunsen burner and immediately record the temperature on the thermometer to the tenth s place (_.x o C). 12. Allow the system to cool to room temperature. Then carefully unclamp the the Erlenmeyer flask still covered with the foil cap and rubber band from the water bath. If it is still warm to the touch, you may set it on the bench top on the wire gauze. 13. Once cooled, completely dry the outside of the covered Erlenmeyer flask and

4 weigh it on the same analytical balance (_.xxxx g). [By the way, when the system is cooled, you should notice that there is some liquid on the bottom of the Erlenmeyer flask but less than the initial amount. Why is this?] 14. Once you have completed step 13 remove the foil cap and rubber band from the Erlenmeyer flask and properly dispose of any remaining volatile liquid. 15. Rinse out the Erlenmeyer flask be sure that it is dry. 16. Weigh the clean, dry Erlenmeyer flask on a balance and record its mass 17. Now fill the Erlenmeyer flask with water (tap is fine) to the brim using a buret to measure the volume. Dry the outside if it is wet. Weigh the water-filled Erlenmeyer flask on the same balance and record its mass Also, record the temperature of the water in the filled Erlenmeyer flask on the thermometer to the tenth s place (_.x o C). 19. Clean Up Discard the liquid in the appropriate container, clean and return glassware to appropriate location. 20. Be sure to obtain and record the barometric pressure before you leave the lab. Calculations 1. Summarize data collected in a table. 2. Calculate the molecular mass of the volatile liquid studied. Show all conversions and calculations with units. 3. Calculate the percent error of your determination, the class average, and the class percent error. 4. Discuss the effect of each of the following possible errors on the results of this lab, including an EXPLANATION of how the error will affect the calculated molecular mass. a. Removing the flask from the hot water bath prematurely, leaving some of the unknown in the liquid phase. b. Not completely drying off the flask and foil before massing it. c. Loosening the aluminum foil before massing the flask, or having the rubber band break, with the same effect. d. Removing the flask from the hot water bath before the temperature of the flask reaches the temperature of the hot water bath. e. Heating the flask for too long after the volatile liquid has evaporated

5 5. Represent, in diagram #1, the flask with the original liquid in it. The liquid should be represented as molecules. Label. Represent, in diagram #2, the flask immediately after heating has been completed, including any molecules that may have escaped the flask. Represent all molecules used in diagram #1. Conclusion with support from data Validity Address, in detail, the techniques and procedures that contributed to the validity of your lab results. You may refer to your percent error in your discussion. Also, refer to the class results, since these represent more trials of the same procedure. Is the validity of your lab supported or not supported? DISCUSS possible sources of error and their EFFECTS upon results. Then address each source of error in your improvements. The improvement must be directly correlated with experimental procedure. There are numerous sources of error in this lab, but only address those that could reasonably happen.

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