In this week\'s experiment you will determine the molar mass of carbon dioxide b

Question

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 20.00oC. 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.

Explanation / Answer

So you have to do a bit of converting and then plug numbers into the gas law equation, which is PV = nRT, but in our case we are going to modify it to be PV/RT = n.

First you have to get pressure. so you look at a vapor pressure of water table (I'm assuming you go to msu, because I do too) and you take the V.P. of that temp. Then you multiply it by .5 because we're assuming 50% humidity. Then you convert it into ATM's by dividing by 760. Then subtract that from the Atmospheric Pressure to find P.

Next you find the volume. Basically, you find the mass of the water by subtracting the empty flask weight from the full flask weight. Then, because 1 gram of water is equal to 1 ml of water, convert that number to Liters by dividing it by 1000, theres V.

Get the temperature by adding 273.15 to the Celsius temp.

substitue to get the final answer

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.