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University of Memphis *

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Chemistry

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Apr 26, 2024

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CHEM 1111: General Chemistry I Lab APPARENT MOLAR MASS OF AIR Procedure: Results: Trial Data Mass (in grams) of the open flask at room temperature with the stopper, tubing and clamp assembly attached to the flask (m 1 ) 114.814g Mass (in grams) of the closed flask (after it has cooled to room temperature) with the stopper, tubing and clamp assembly attached (m 2 ) This is the mass of the flask assembly after it was submerged in the boiling water bath 114.796g Calculated mass of air (in grams) lost upon heating (Δm = m 1 – m 2 ) 114.814g-114.796g=0.018 Δm=0.018g Temperature (°C) of the air in the flask before heating (T 1 ) 18.9degC 273.15K Temperature (°C) of the boiling water (T 2 ) This is the temperature of the air in the flask when sealed off in the boiling water 69degC 342.15K Air pressure (atm) barometer reading (P) 1.02atm= 912 mmHg Volume (L) of air sealed in the flask (V) Be sure to convert from mL to L 137mL = 0.137L 1 (narrate the procedure observed in the video)
CHEM 1111: General Chemistry I Lab Trial Data Calculated moles of gas contained in flask at room temperature (n 1 ) Use rearranged ideal gas equation (n 1 = PV / RT 1 ) Calculations: Calculated moles of gas contained in flask at boiling water temperature (n 2 ) Use rearranged ideal gas equation (n 2 = PV / RT 2 ) Calculations: Change in moles (Δn) Δn = n 1 – n 2 Calculations: Calculate the apparent molar mass (MM) MM air = Δm (in grams) /Δn (in moles) Calculations: 2
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