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The Ideal Gas Law Data Sheet Part A: The Dead Volume Data Temperature of the water in the beaker (°C) 22.8 Mass of the dry empty beaker (g) 30.987 Mass of the beaker plus water (g) 37.837 Part B: Collection of the Hydrogen Data Mass of the magnesium ribbon (g) 0.0428 Volume reading of the burette with hydrogen (mL) 13.55 Temperature of the water in the cylinder (°C) 22.6 Atmospheric pressure in the lab (mmHg) 764.3

Table 1: Density and vapor pressure of liquid water Temperature/tc Density/gcm Vapor Pressure /mm Hg 15 16 12.79 17 13.5 14.53 18 19 15.48 20 16.48 21 17.54 0.99910 0.99895 0.99878 0.99860 0.99841 0.99821 0.99800 0.99777 0.99754 0.99730 0.99705 0.99679 0.99652 18.65 22 19.83 23 21.07 24 25 22.38 23.76 26 27 28 25.21 26.74 28.35 30.04 0.99624 29 0.99595 30 0.99565 31.82

Part B: Reaction of magnesium with hydrochloric acid 1- From the mass of Mg(s), calculate the theoretical number of moles of Mg and of H2(gas) that should be produced during the reaction (see Equation (2)). (4 marks) nH2(g) = 2-Determine the Vapor Pressure of water (Pwater) at the temperature of the water used in your experiment (use table 1 and see Equation (9)). (4 marks)