following tables. Write the chemical reactions for both
procedures. Show work on all calculations.
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Molar Volume of Hydrogen Data Mass of magnesium Moles of hydrogen Average temperature of gas (absolute, K) Pressure of hydrogen, PH2 Volume of H₂ at STP Molar volume of O₂ at STP (L/mol) Calculations
PROCEDURE Part 1. Production of Oxygen Gas 1. Assemble the apparatus as shown in Figure 1. Clean the glassware with soap and water, use deionized water (DI water) as the final rinse. For flask B use a 500-mL Erlenmeyer flask or a 500-ml filter flask. You may have one in your drawer. If not, borrow one from the stock room. Remove the yellow side arm from the filter flask and put a cork in the hole on the side of the flask. Corks are provided in a bin along with the rubber stoppers and hoses. 2. Obtain a small test tube (10 x 75 mm provided for this experiment). Test to make sure the small test tube remains standing at an angle in the 250-mL flask. If it drops completely horizontal inside the flask, obtain another flask. Rubber Tube AB Rubber Tube BC Connection A 500 mL 600-ml. 250-mL Erlenmeyer Flask A Flask B Beaker C Figure 1. Note the position of the clamp, it is near the top of flask B. 3. Measure 20 mL of 3% H₂O₂ solution in a graduated cylinder and pour it into a 250-mL Er- lenmeyer flask (flask A in the Figure). Measure and pour approximately 4.5 mL of 3M FeCl, into a 10 x 75 mm test tube (a very small test tube provided for this experiment). Holding flask A at an angle, carefully slide the test tube into the flask or lower the test tube with a pair of tongs.
5. Fill the 500-mL Erlenmeyer flask B to the neck with tap water. Fill the 600-ml beaker C about one-third full with tap water. Disconnect the rubber stopper at point A and attach a pipette bulb. With the pinch clamp open, force air into rubber tube AB by squeezing the pipette bulb, forcing water from flask B into the beaker C. Raise and lower beaker C to move water back and forth through rubber tube BC to remove all air bubbles. With water halfway up the neck of flask B, reconnect the stopper at point A. 6. With the pinch clamp open, test the apparatus for leaks, as follows. Raise beaker C as high as possible without removing tubing from the beaker. The water level in flask B should move a little and then remain fixed. If the water level continues to change, a leak is present. Do not proceed until the leak is fixed. 7. Equalize the pressures inside and outside flask B by raising the beaker until the water level in the beaker and in flask B are the same. While one student holds the beaker to keep the water levels the same, another student closes the pinch clamp, positioned near the stopper on flask B. Pour out all the water in beaker C. Replace the tube in the beaker and open the pinch clamp. A little water will flow out and should be retained in the beaker. 8. Fill a trough half full with water.
9. Tip flask A carefully so that the FeCl, catalyst spills out of the test tube into the hydrogen peroxide solution (avoid getting the solution on the stopper). Place the flask in the water trough. Swirl the flask to mix the reactants. Note and record any changes that you see. As the oxygen is released, water is forced from flask B into beaker C. Feel the bottom of flask A. Is heat released or absorbed in the reaction? Note the level of the water in beaker C. Swirl the flask some more. When the reaction stops, and the water level remains constant, you can assume the decomposition of the hydrogen peroxide is complete. 10. Let the solution sit for 15 minutes to allow the temperature of the solutions in flasks A and B to equilibrate to room temperature. 11. Raise beaker C until the water levels in flask B and beaker C are equal, at which point an- other student closes the pinch clamp on tube BC. Measure the volume of oxygen produced by carefully pouring the water in beaker C into a graduated cylinder. Record the volume of water displaced by the oxygen gas. 12. To measure the temperature of the gas produced in the reaction, loosen the stopper on flask A and insert a thermometer into the solution. Measure and record the temperature of the solution in flask A. Similarly, measure and record the temperature of the solution in flask B. The average of these two temperatures represents the temperature of the oxygen gas. 13. Disconnect flask A at point A and weigh and record the flask and its contents.
1. Set up the apparatus as in part 1. Clean the glassware with soap and water, use DI water as the final rinse. 2. Weigh an 8-cm piece of magnesium and place it into a 250-mL Erlenmeyer flask. Pour 4.5 mL of 3 M HCl into a small, 10 x 75 mm, test tube. Holding flask A at an angle, carefully slide the test tube into the flask or lower it using a pair of tongs without spilling any of the contents.
Repeat steps 4-12 of Part 1. Note in step 7, when flask A is tipped the HCI spills out of the test tube into the flask containing the Mg (s). The reaction is complete when all the magnesium disappears. The reaction produces hydrogen gas. When the temperature of the gas in flask A is measured, tip the flask to submerge the tip of the thermometer in the HCl solution.