Question

Mass of Magnesium Volume of gas produced Height of water column Trial 2 0.03029 Trial 1 0.03309 34.4mL 18.26cm 21.7 mmity 23.5°C 751 torr Pressure of water column Temperature of water Atmospheric pressure 23.76 mm Hg 25.0°c 751 torr Water vapor pressure CALCULATIONS: Perform calculations for both trials. 1. Calculate the total pressure of the gases inside the eudiometer at the end of the experiment. Trial 1 Trial 2 2. Calculate the partial pressure of the hydrogen gas in the eudiometer tube. Trial 1 Trial 2 59 Laboratori Stoichiometric Measurement of a Gas Product

Answer 1

- hoog, atin - hdg x 760 too da desse - Amospheric pressure = Pressure of gas misture in the endiometer(P) + Pressure of water column. . Pressure of gas möcture in the eiidiometer (P)= Atmospheric . pressuré ~ Pressure of water columni Trial #1: P = 3751-(18.6] *981)*760} torrum Pressure of water 2 013X106 =(751-13-69) = 737.31 tors . dynefun Trial #20 T =(751 - 1981*981x760) torr T 1013x106 an 1.0138106 (751- 13.98) torr h = height of water = 7376 02 torr ga gravity-981106 Total pressure of gas misiture in the endiometer .(P) = Partial pressure of Hz CPH) + Vapor pressure of Wales Trial # 1 73731. = P + 21.71 [vapor foressure of wales or bits =(737-31 - 21:71) = 715.6 torr Trial #2 : 737.02 = + + 23.76 [vapor pressure of water atac or Pit =(737.02 – 23.76) = 713.26 torr 3 Now, PV = nRT Tocal # 1: No. of moles of Hz gas produced = Phyx V RT . 715.6 x 34:41 760° ^TOOO 0:082x(23.5+275. = 0.00133mol. 713.26 x 32.8 Lice? - ** 760 X 1000 X0.082 298 =0.001259 moli

• 1 mol. 24.3 0.001263 ©. Mg(s) + 2H41 (09) + MgA2 (29) + H2(9) i mot i Trial #1: No. of moles of H2 gas = no. of moles of Mg = (0.0330) -0.0013526 Trial # 2 ; No. of moles of H2 gas = no. of moles of Mg : : = 10.0307) - 1 24.3 6 percent yield = Exeberimental yield xico y Theoretical field Trial # 1: 4 yield = 0.00133X100 - 98.52% 0:00135 = 18.52%. . . . Trial # 2°; 7. yield = 0.001259810069,92%. 0.00126- © Average percent yield - Trial # 1 + Trial #2_198152 +99927 =99:22 %. CA