In this weeks experiment you will determine the molar mass of carbon dioxide by

Question

In this weeks experiment you will determine the molar mass of carbon dioxide by measuring the mass of an Erlenmeyer flask full of the gas. The following calculations are intended to familiarize you with the general procedure: The mass of an empty Erlenmeyer flask and stopper was determined to be 53.51 grams. When filled with distilled water, the mass was 294.0 grams. The atmospheric pressure was measured to be 0.9757 atm, the room temperature was 23.00 degree C. At this temperature, the vapor pressure of water is 21.10 torr -- but assume a 50% relative humidity as outlined in the procedure for this experiment. What is the number of moles of air in the flask? Moles of air in the flask = mol If the average molar mass of the gases present in air is 28.960 g mol^-1, what is the mass of air in the flask? Mass of air in the flask = grams What would be the mass of carbon dioxide in the flask? In this case the CO2 will be saturated with water vapor so assume 100% humidity as outlined in the experiment. Mass of carbon dioxide = grams What would be the mass of the flask (and stopper) when filled with carbon dioxide gas? Mass of flask and stopper filled with CO2 gas = grams

Explanation / Answer

A. Moles of air in the flask = mol The mass of an empty Erlenmeyer flask and stopper was determined to be 55.94 grams. When filled with distilled water, the mass was 298.3 grams. Therefore the water displaced x' amount of grams of air. 298.3grams - 55.94grams = 242.36 grams of air.... The molar conversion given is as 28.960g/mol .... 242.36g of Air = (1mol/28.960g of Air) = 8.37 mol of Air

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