Question

Experimental Determination of the Gas Constant Experimental Data . (a) Mass of Magnesium metal used (b) Volume of H, gas collected mi (C) Temperature of H2 gas collected (d) Atmospheric Pressure (e) Temperature of Water in bath (bucket) Vapor Pressure of Water at above temperature Trial 0.03419 36.0 ml 22 • 766-5 mm/Hg 2214 oc 19.3 mmHg Trial 2 0.02129 20.5 mL 23-0's 766 5mnHg 224 °C 22 mmHg Data Analysis Using your experimental data, determine the value of R, the gas constant. Show all your conversions and calculations for each step clearly in the table below. Pay attention to units and significant figures. Trall Trial 2 Volume of H, ens (in L) Temperature of Hą gas (in K) Moles of H; gas Pressure of H; gas (in atm) Page 1 of 2

Answer 1

Date: -/- Trial 2 Trial 1 volume of gas (in L) 36 mL = 36 2015 ml 1670 20.5 0.02052 = 0.0362 Temperature of H₂ gas link) 22.1 +273.15 = 295.25k 23.0 + 273.15 = 276.15K Moles of ₂ gas Mg(s) + H₂O (8) - Imde Mg produces MgO (19 th ) - Imole H₂ = 0.0341 g = 0.0014 mol 24.5g/mol = 0.ool 4 mol H moles of bid 2 0.00087 mol 0.0212 24.3 0.00087 mot H2 =

Date: -/- Pr - Puzo 766.5- 19.3 747.2 torr 747.2 760 30.9& 32 atm 1 toid 2 - Pu = 766.5-22.1 = 744.4 torr = 744.4 0.9794 atm 760 Trial 1 0.9832 atm xo 1036L AO 0.0014 mol X 295025k 0.0856 atonil mol.K trial 2 0.9794 atm x 0.02052 0.00087 mol x 276.15k 0.0836 atm. L mot. K