Gas Laws Equipment Set-up and Leveling bulb discussion: A buret will be used to collect our gas product, so we can measure the volume of gas produced accurately. A leveling bulb (a plastic bottle with an opening at its base) is attached to the bottom of the buret with a rubber hose. The opening allows the water in the system to be exposed to the atmospheric pressure in the lab. The leveling bulb is filled with water, and the water moves through the hose to fill the buret. As gas is produced, the water will be pushed out of the buret into the leveling bulb thus preventing excess pressure build up. The reaction chamber is a round-bottomed flask, into which the hydrochloric acid and aluminum metal is placed. There is a second hose that connects the reaction vessel to the top of the buret. When the reaction flask is screwed on, the system is closed. Note that when the reaction flask is removed by unscrewing the screw cap, the water levels in the buret and leveling bulb will be equal (both at atmospheric pressure). Thus, to raise or lower the water level in the buret you simply raise or lower the leveling bulb. Before beginning the reaction with the reaction flask off, adjust the leveling bulb up and down. Verify that as the bulb is raised, the water in the buret rises to match the level of water in the bulb and when the bulb is lowered, the water level in the buret drops to match the level in the bulb, so the water levels remain equal. Figure 1: Experimental Set-up with Leveling Bulb Check for leaks. With the reaction flask screwed on and the rubber septum attached, raise and lower the bulb. The water should not flow as freely as before due to the system being closed, and the water levels should not remain the same. With the reaction flask on (system closed), lower the bulb so the water level in the buret is higher than the water level in the bulb. The level of water in the buret should not continue dropping to the same level as the water level in the bulb. If it does, your system has a leak. Check to make sure the reaction flask is screwed on securely and the septum is attached. If you cannot find the source of the leak, consult your instructor. Once leaks have been eliminated, lower the leveling bulb, so its water level is lower than the level of water in the buret. The pressure inside the buret is now less than atmospheric pressure (the gas in the buret is not pressing down as hard as the atmosphere). Now raise the bulb so that the water level in the buret is lower than the water level in the bulb. The pressure inside the buret is now higher than atmospheric pressure (the gas in the buret is pressing down harder than the atmosphere). Remember, when the water levels are equal, the pressures are equal. You will keep the water levels equal while running the reaction so that the pressure inside the reaction chamber and buret is equal to atmospheric pressure. Water Vapor Pressure: As a gas is collected over water it becomes saturated with water vapor. The total pressure in the system at the end of the reaction is, thus, due to both the gas product’s pressure and the water vapor pressure. So the total pressure is the sum of the pressure of the gas (Pgas) and the pressure of the water vapor ( PH 2 O ). This is a result of Dalton’s Law of Partial Pressures. Ptotal = Pgas + PH 2O Since the water levels were kept equal with the leveling bulb, the total pressure inside the buret is the same as the pressure outside the buret. Thus the total pressure is simply the atmospheric pressure. The pressure of the water vapor depends only on temperature and can be obtained by entering the temperature (in °C) into the Vapor Pressure Calculator Website. Thus, the pressure of the gas alone can be calculated by subtracting the vapor pressure of water from the total atmospheric pressure. In reality, if a reaction is carried out in a closed container to trap any gas product, the pressure inside the container will build up. If too much pressure results, the container could explode. We must avoid building up pressure in the glass buret, and this is accomplished by keeping one end (the leveling bulb end) of the apparatus open to the atmosphere throughout the experiment. Thus, when gas is generated, the gas can push the water through the buret into the leveling bulb. SAFETY PRECAUTIONS: In the presence of a flame, the hydrogen gas given off in this reaction can react explosively with oxygen in the air. No flames are thus allowed in laboratory during this experiment. Hydrochloric acid can cause burns if in comes in contact with skin. If any acid is spilled on your skin, wash immediately with soap and water, tell your instructor, and rinse for 15 minutes. Safety goggles must be worn at all times because contact with HCl(aq) for even a short time can cause permanent eye damage. Procedure: 1. LAB NOTEBOOK: Prepare a data table that contains the following information for 3 trials: Mass of Al, Theoretical Moles of Gas, Theoretical Volume of Gas, Initial Buret Volume, Final Buret Volume, Actual Volume of Gas Produced, Actual Pressure due to Gas in Buret, Actual Moles of Gas Produced, Percent Yield, and Average Percent Yield. Note that the actual pressure due to gas in buret and the average percent yield will be the same for all three trials. Label a place either directly above or below the data table to record the following data: Room Temperature, the Atmospheric Pressure, and Vapor Pressure of Water at this Temperature. 2. Obtain 6 round pieces of an aluminum can by using a hole punch. Obtain three weigh boats, and put two of the aluminum pieces in each. (Each trial will use 2 pieces.) Weigh the aluminum pieces on an analytical balance by taring the empty weigh boat first. Record the exact mass of the aluminum pieces for your three trials in your data table. 3. Now carry out the following theoretical calculations in your LAB NOTEBOOK. (Make sure to label each calculation such that it can be graded): a. Write and balance the equation for the reaction between solid aluminum and hydrochloric acid. b. Use this balanced equation to calculate the number of moles of gas that should be produced from the grams of aluminum. (This is your theoretical number of moles of gas produced.) c. Use the Ideal Gas Law to calculate the volume of gas that should form given the theoretical number of moles of gas calculated. (This is your theoretical volume of gas produced.) Have your instructor confirm your calculations and initial in your lab notebook. d. Do NOT forget to put your results from calculations b. and c. above in your data table. 4. Now you are ready to test your theoretical calculations. Make sure your equipment is set up according to Figure 1, shown on page 3. a. Adjust the leveling bulb and check for leaks as described in the Experimental Set-up section. b. Take your graduated cylinder and obtain about 3.0 mL of 6M hydrochloric acid at the reagent station. Return to your bench and take care not to spill any of the acid. c. Remove the reaction flask, and pour the hydrochloric acid inside.(The flask does not need to be dry – if you are unsure if it is clean rinse with DI water several times.) d. Lift the leveling bulb so that the buret water level is around 15 mL. When everyone is ready in your group, drop the two aluminum pieces for trial one into the flask. Screw the reaction flask back on while holding the leveling bulb steady so that the water levels in the bulb and buret are equal. Record the exact volume in the buret as the initial volume for trial 1 making sure the bulb and buret water levels are still equal. e. While the reaction proceeds, keep the leveling bulb and buret water levels equal. f. When the reaction has stopped, hold the bulb steady with the water levels equal, and record the exact final buret volume. g. Unscrew the reaction flask, empty the contents into your waste beaker, and rinse with DI water twice. 5. Repeat step 3 for the remaining two trials with the other aluminum can pieces. 6. When you are done with all 3 trials, wash the reaction flask using tap water and then rinse the reaction flask with DI water for the next class. Do the same for all your glassware and wipe down your lab bench. 7. LAB NOTEBOOK: Using your results explicitly label and complete the following calculations in your lab notebook. Do not forget to complete your data table. a. Actual moles of gas produced for each trial. b. Pressure due to the gas produced in reaction (See the Water Vapor Pressure section, p. 2). c. Percent Yield for each trial. 8. LAB REPORT: Submit the following for your lab report: Lab Notebook copies and Postlab Questions (pages 5 & 6). _________________________________________________________________ Gas Laws: Lab Report Name: ________________________ Partner(s): _____________________ Section Number: ________________ Post Lab Questions: 1. Using the Activity Series circle the metals that would react with hydrochloric acid to produce hydrogen gas. Cu(s) Ni(s) Au(s) Mg(s) Pb(s) Ag(s) Mn(s) Fe(s) 2. Why was the exact volume of the hydrochloric acid in the flask not recorded? 3. Draw a picture representing 5 molecules of hydrochloric acid in the beaker of water. Hint: Is hydrochloric acid a strong, weak, or non-electrolyte? 4. Would the following 3 hypothetical errors cause a higher or lower percent yield? Explain your answer in each case. High a. A leak in the rubber tubing allows some gas to escape. Low High b. A student forgot to subtract the water vapor pressure from the atmospheric pressure while doing the calculations. Low High c. A student held the leveling bulb way below the buret’s water level while reading the final buret volume. Low 5. The reaction between the hydrochloric acid and the can began slowly. When the reaction began to accelerate, two thin films of plastic came off the metal. These plastic films did not react with the acid. Why did the reaction start slowly and then suddenly accelerate? 6. There is a difference between your theoretical and actual volume of hydrogen gas. Assuming your technique was good and there was no human error, explain the difference. 7. In reality, most of the gas in the buret was actually air from the tubing and reaction flask that was pushed into the buret as hydrogen gas was produced. Does the presence of this air instead of hydrogen gas affect your experiment? Explain your answer.