Calculating Ethane Pressure and Mass in a Flask

AI Thread Summary
The discussion revolves around calculating the final pressure and mass of ethane in a flask after a series of temperature changes. Participants clarify that while the volume of the gas may change during heating, it becomes constant once the stopcock is closed. The ideal gas law (PV = nRT) applies after this point, with pressure being constant during the heating phase. The initial confusion regarding the changing volume is resolved, emphasizing that the problem's complexity lies in understanding the system's state after the stopcock is closed. Overall, the key takeaway is the importance of recognizing the constant volume condition for accurate calculations.
WY
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Hey - I'm doing this question (see below) but I don't hav a clue where to start!

A flask with a volume of V, provided with a stopcock, contains ethane gas at a temperature of T_0 and atmospheric pressure p_0. The molar mass of ethane is M. The system is warmed to a temperature of T, with the stopcock open to the atmosphere. The stopcock is then closed, and the flask cooled to its original temperature.

What is the final pressure of the ethane in the flask?

and

How many grams of ethane remain in the flask? Use R for the ideal gas constant.

for the first part i tried relating the initial and final pressures and volumes as a ratio... but that didn't work and since I don't have the volume of the actual gas which changes I can't apply the pV=nCRT equation...
Can someone tell me how to start?

Thanks in advance!
 
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WY said:
Hey - I'm doing this question (see below) but I don't hav a clue where to start!

A flask with a volume of V, provided with a stopcock, contains ethane gas at a temperature of T_0 and atmospheric pressure p_0. The molar mass of ethane is M. The system is warmed to a temperature of T, with the stopcock open to the atmosphere. The stopcock is then closed, and the flask cooled to its original temperature.

What is the final pressure of the ethane in the flask?

and

How many grams of ethane remain in the flask? Use R for the ideal gas constant.

for the first part i tried relating the initial and final pressures and volumes as a ratio... but that didn't work and since I don't have the volume of the actual gas which changes I can't apply the pV=nCRT equation...
Can someone tell me how to start?

Thanks in advance!

I don't know about the C in pV=nCRT. The usual representation of the ideal gas law is PV = nRT, where R is a constant. In this problem, the pressure is constant during heating, and the volume of the flask is constant for the whole problem. During heating, PV is constant and you are raising the temperature. What has to change, and how is that change related to the temperature change?
 
Thanks for replying! Sorry I wrote down the wrong equation -_-
but in this problem doesn't the volume of gas change? So why doesn't it effect the way we caluclate it?
 
Nope, the problem essentially starts when the cork is closed, after which the volume is constant. I don't know why they included all that information, its just confusing, they should have just stated that the system started at a certain temperature and dropped.
 
oh I see! thanks for clearing that up now - its all crystal clear now!
 
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