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template_exp_5

# template_exp_5 - EXP 5 MOLAR MASS OF A LOW BOILING LIQUID...

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PURPOSE AND METHOD DATA AND CALCULATIONS A. Unknown # 2 Run 1 Run 2 Run 3 Mass of flask + cap + air 50.39 50.39 50.39 1 pt Mass of flask + cap + vapor 50.49 50.49 50.49 B. Barometric pressure, mm Hg 771.1 100 1 pt Water (room) temperature 21.6 Mass of flask + cap + water 176.24 Density of air, g/L 1.21 1 pt Sample temperature (~100 o C) 1. Calculate the density of air in g/L assuming air is 20.0% O 2 and 80.0% N 2 at the temperature and the pressure of the laboratory 32*1/5 + 28*4/5 = 28.8 Because PM = dRT So d = (1.1046 * 28.8) / (0.08206 * 294.6) = 1.21 (g/l) EXP 5: MOLAR MASS OF A LOW BOILING LIQUID Grading WebAssign prelab: 5 pts This template: 30 pts Lab Notebook (Duplicate): 5 pts The purpose is to determine the molar mass of a low boiling liquid. Explain how this is accomplished. (4 pts) Gases may be accurately described by the ideal gas law: PV = nRT. Where P is the pressure, V is the volume, R is the gas constant, and T is the absolute temperature. If P, V and T are measured, then n, the number of mole, can be determined. If the mass of the gas (m) is also known, then the molar mass (MM) of the gas can be found: MM = m / n In this experiment you will determine the molar mass of a low boiling liquid. This method was

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template_exp_5 - EXP 5 MOLAR MASS OF A LOW BOILING LIQUID...

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