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13 Dec 2019

In this week's 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 59.65 grams. When filled with distilled water, the mass was 299.4 grams. The atmospheric pressure was measured to be 0.9556 atm, the room temperature was 20.00^oC. At this temperature, the vapor pressure of water is17.50 torr -- but assume a 50% relative humidity as outlined in the procedure for this experiment.

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Elin HesselLv2

17 Dec 2019

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n this week's 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 43.59 grams. When filled with distilled water, the mass was 291.1 grams. The atmospheric pressure was measured to be 0.9916 atm, the room temperature was 19.00^oC. At this temperature, the vapor pressure of water is 16.50 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?

Mass of carbon dioxide = grams

What would be the mass of the flask (and stopper) when filled with carbon dioxide gas? In this case the CO₂ will be saturated with water vapor so assume 100% humidity as outlined in the experiment.

Mass of flask and stopper filled with CO₂ gas = grams

Objective : Calculate the molar mass of CO2 (dry ice). Make sure this is handwritten in the lab notebook.

Procedure :

Note : During the lab, look for a qualitative observation that proves CO2(g) is denser than air.

(1)Weigh the empty 250mL Erlenmeyer flask with a rubber stopper on.

(2)Obtain few small pieces of CO2(s) in the flask. The total amount should be close to the given rubber stopper in size. Let it sublime. Make sure the pieces are small enough so you can see them âsingâ and âdanceâ.

(3) When sublimation is done, cap it with the stopper and weigh it. We are assuming that the container is completely filled with CO2 at this point.

(4) Measure the temperature of CO2.

(5) Fill the flask all the way to the rim with water and put the rubber stopper on. Water will spill over. Pour the water into 50mL/100mL graduated cylinder (multiple times) and measure the total volume of water.

(6) Measure pressure of the air using the barometer on the wall.

Analysis

(A1) Calculate the moles of CO2 using PV=nRT.

(A2) Calculate the molar mass of CO2.

Question:

I have provided all of the procedure.

ANswer this question only -->

What would happen to the final result if the CO2(s) sample was too small (not enough) to fill the flask?

<--

answer this one question above clearly. explain step by step.

thanks

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