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Experiment 19 Gas Stoichiometry and the Gas Laws The relationship between the physical properties of a gas, and the moles, is given by the “Ideal Gas Law:" PV=nRT where n-number of moles R=the ideal gas constant: 0.0821 atm L mole 'Kor 62.4 L torr molek In this experiment, the theoretical yield of gas, will be compared to the experimental yield. The reaction of aluminum with hydrochloric acid produces hydrogen according to the balanced equation below. 2 Al(s) + 6 HCl(aq) → 3 Hz(g) +2 AlCl3(aq) The number of moles of hydrogen will theoretically be equal to 3/2 times the moles of Al used. In this lab, approximately 0.0067 moles of Al will be used such that about 0.01 mole of hydrogen may be produced. The actual yield of hydrogen can be plugged into the Ideal Gas Law, and the moles calculated. A pressure correction also needs to be made, to correct for the vapor pressure of water, the amount of water vapor in the gas. Materials: Equipment 250 and 500 mL Florence flasks 150 and 400 mL beakers rubber tube/stopper assembly rubber bulb Chemical aluminum wire 6M HCI deionized water Procedure: Connect a 500 mL Florence flask (the large flask) with a 250 mL Florence flask (the reaction flask) with the first tubing as shown in the diagram below, and fill the large flask with 500 mL of distilled water. Use a ring stand and clamp both flasks down for stability. The second tubing is placed in a 150 ml beaker that contains a bit of water. Remove the first tube from the reaction flask, use a bulb and blow in air so that the second tube is filled with water. The second tube should not have any air bubbles. Having water in the 150 mL beaker should prevent air bubbles from coming back into the tube. Close your system by bending the first tube and pinch the tube using the pinch clamo Hold the second tube filled with water in place, don't lift it, bend or tilt the healermo w from the tube, and replace it with a clean and dry pre-weighed 400 ml benker Your instructor will demonstrate this. piece of Al and record its mass (0.11 to 0.26 g). Place it in the bottom Obtain a piece of Al an pour about 20 mL of 6 M HCl into the flask and quickly insert the of the reaction flask. Pour about 20 mL of 6 M HClinton first tube. Remove the pinch clamp! As the reaction proceeds, water will stopper with the first tube. Remove th

Answer 1

trial sandes of Aluminium = Mass Al Molar Mass Al = 0.16 g 0.0059 mol 26.98 g molt 6 Theoretical field of hydrogen gas : moles of H₂ = 3 moles of Al (as per ) of equation, 2Al(s) + 6HCl(aq) — 3H₂(g) + 2 Alcez (aq) Moles of H₂ = 340.0059 mol Al = 0.0088 mal (Theoretical yield @ Volume of water collected = mass of water collected Nut density of water Mass of water collected = (mass of beaker twater) 1 - (Mass of beaker) = 385.269 - 152.959° = 232.319 Volume = 232.31 g 232.31 ml = 0.2326 - 1gml @ Temperature of water (K) = 273-15° + 2400 0 = 297.15K @ Vapour pressure of water = 22.4 tore at 246 @ Pressure of dry H₂ = Atmospheric pressure - Vapour to - 75 8.4 torr-2204 torr = 736.0 torr 6 Pressure of dry hydrogen (atm): I atm = 760 torr 736 torr = 0.968 atin. ch) Experimental yield PV=MRT T in 0.968 atm x 0.232 L = n och 0.0821 Latmk mot x 297.15k to Live moles = 0.0092 moles en pressure of water

☺ plu error = theoretical - experimentally too theoretical = 10.0088 -0.00921 x 100 0.0088 = 4054%