oxygen is released. The oxygen will force an equal volume of H20 out of the flask into Gently heat the flask with the Bunsen burner. As the KCIO4 begins to decompose, pure the beaker. The amount of oxygen released will depend on you. Try to get between 150 and 300 mL of H2O collected in the beaker. If you heat the flask too much, the water level will drop below the bottom of the longer tube and you will have to start over. 7. When enough H20 has been collected, allow the system to cool for 15 minutes. Hold the beaker so the level of H20 in the beaker and Florence flask are equal then remove the filler tube. This will equalize the pressure inside the flask so it will be equal to atmospheric pressure. 8. Record the temperature of the collected H20 to the nearest 0.1°C. This will be the approximate temperature of the gas within the Florence flask. 9. Use a large graduated cylinder available in the lab to measure the volume of the H20 displaced by the O2 gas to the nearest mL, (record on the data sheet). 10. When the Erlenmeyer flask has cooled to room temperature, weigh it again to obtain the mass lost due to O2 generation (record). [Dispose of the leftover KCIO4 + MnO2 mixture in the designated waste container in the lab.] Remember to put away your glassware, wash bottles and any other equipment you removed from your drawer. Both you and your lab partner should check to make sure that the equipment you used during the lab is cleaned and replaced. Data and Observations: (Summarize the data below in table format with an appropriate title.) 1. Mass of flask + KCIO4 + MnO2 (initially) 81.80239 2. Mass of flask after heating 81.62oog 3. Volume of O2 gas (H20 displaced) 151 m2 4. Temperature of O2 gas (temp. H2O) 20,2 co 5. Atmospheric pressure (mm Hg) 6.22.2mm Hg 2.3288 pk a 6. Pressure H2O vapor (pka) (see chart on wall) riculations and Results: 1. Mass O2 generated summarize the results below in table format with an appropriate title.) 2. Volume O2 in liters 3. Temperature of O2 in K 4. Pressure O2 gas in mmHg. 5. Pressure O2 gas in atm. 6. Molar mass of O2 gas calculated 7. % Error = (Your MM-actual MM) x 100% actual MM 8. List at least two possible sources of error which could have lead to an incorrect determination of molar mass. Additional Questions: 1. A gaseous compound is composed of 85.7% of carbon and 14.3% of hydrogen. Its density is 2.28 g/L at 300K and 1.00 atm pressure. Determine the molecular formula of the compound. 2. A 1.525 g mass of a volatile liquid is vaporized, giving 500.0 mL of vapor when measured over water at 30°C and 770 torr. The vapor pressure of water at 30°C is 32 torr. What is the molar mass of the substance? 3. A mixture containing 0.226 mol He, 0.342 mol Ne, and 0.128 mol Ar is confined in a 4.00 L vessel at 25°C. What is the total pressure of the gas?
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