Question

Laboratory Report - The Molar Volume of a Gas Experiment 9: The Molar Volume of a Gas Data 285 ml Run 1 Run 2 weight of magnesium 0.15g incl 21. 8 Ĉ temperature of the water (temperature of the hydrogen) in °K 315-8 K volume of water displaced (volume of hydrogen collected) V 285 ML atmospheric pressure (total gas pressure in the flask) 0.9931 atm vapor pressure of water at 0.0261 atm 19.84 mm te pressure of hydrogen collected 0.967 atm

Answer 1

a) mass of Mass of Magnesium metal - 0.15g Atomic mass of magnesium metal - 24g1mo modes of magnesium metal = 0.15 = 0.006s moles 24 Mgcs, + 2HCl MgCl2 cag) + H2 egg = 0.00625 moles Moles of H26g) = moles of Mg x 1 mol H2 Temp of H2(g) = 21.8°C = 273.15 +21.8= 294.95 from epun PH2o - exp(20.386 - 51,32 mmHg. PH2O = 19.29 mmHg Basometric pressure - 0.967 atm = 734.92 ob H2 Volumes of H₂ collect ed = 285ml = 0.2854 c) A4 sTP P2 = 760 mmHg T2= 273 mm Hg 12 = PV x T2 = 734-1) 0285 273 295 760 -0.2550 P2 4) moles op H2 = 62S90 0.00625 moles molar volm - 0.2550 = 40.80 L 0.00625