The Ideal Gas Law Post-Lab Name Section Nmbor Date Show all work for full credit

Question

The Ideal Gas Law Post-Lab Name Section Nmbor Date Show all work for full credit DATA: Unknown Liquid , final mass of flask 684ag final mass of flask 37 y Hg Trial 1: initial mass of flask 1.44 Trial 2: initial mass of flask S final mass of flask 34 3initialmas of fask 37.52 velume of the fak, n Pressure of the room, in atmospheres 51-mm p CALCULATIONS: Calculate the average mass of unknown liquid collected in your flask from the three trials. 267? Use the ideal gas law to determine the molecular weight of unknown gas in the flask. Assume that the temperature of the flask was 100°C. I The Ideal Gas Law: Post-Lab

Explanation / Answer

Mass from trial 1 = 88.429 - 88.139 = 0.29 gm

Mass from trial 2 = 91.79 - 90.35 =1.44 gm

Mass from trial 3 =87.87 - 87.53 = 0.34 gm

Average mass = (0.29 + 1.44 + 0.34 )/3 = 2.07 / 3 = 0.69 gm

Gas constant, R = 0.082057 L atm mol-1K-1

pressure, P = 757 mm of Hg = 0.0013158 * 757 atm = 0.996 atm

Temperature, T = 273.15 + 100 = 373.15 K

Volume, V = 150 ml = 0.15 mL

Applying ideal law gas,

PV = nRT

n = PV/RT = (0.996 * 0.15) / ( 0.082057 * 373.15) = 0.00488 mol

Thus molecular mass of gas = 0.69 gm / 0.00488 mol = 141.4 gm/mol

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