How Does Raising Air Pressure in a Flask Affect Temperature and Maximum PSI?

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Discussion Overview

The discussion revolves around the effects of raising air pressure in a flask on temperature and maximum pressure, specifically in the context of using a 100 psi air compressor to add air to a one-liter glass flask. Participants explore the implications of the ideal gas law and related gas laws.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant suggests that using a 100 psi compressor could raise the pressure in the flask by 100 psi, leading to a temperature increase by a factor of 14, based on the ideal gas law.
  • Another participant challenges this view, indicating that the application of Boyle's law may not be appropriate in this scenario, as it assumes a fixed mass of gas and does not account for the compressor's outlet temperature.
  • A later reply acknowledges the correction regarding the dynamics of air being pushed into the flask, indicating a shift in understanding of the situation.

Areas of Agreement / Disagreement

Participants express differing views on the application of gas laws in this scenario, with no consensus reached on the correct interpretation of how pressure and temperature will change in the flask.

Contextual Notes

There are limitations related to the assumptions made about the behavior of gases under varying conditions, particularly regarding the fixed mass of gas and the dependence on the compressor's characteristics.

Batata
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Hi! I'm a biologist so be easy on me:)

Say I had a one liter glass flask filled with air and I had a 100 psi air compressor attached to it. (I don't want to suck air out but blow more inside!) How would the air in this flask react - according to the law of ideal gas the temperature of the air should start rising, but would I be able to increase the pressure in the flask as well? How much would I be able to raise the psi in the flask?

Thanks!
 
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i think if you had a 100PSI compressor, you could raise the pressure by 100PSI.
the volume would remain the same, so T would go up by the same factor.
100PSI is 14 times atmospheric pressure, so the temperature would increase by a factor of 14.

but I'm not 100% sure. hopefully someone else can either confirm I'm correct, or let you know what i did wrong.
 
dnp33
I'm sorry you are wrong, you seem to be applying Boyles law P1*V1/T1=P2*V2/T2 but this only works for a fixed mass of gas. The temperature of the gas in the flask in this instance would be about the same as the outlet temperature of the air compressor, which would depend on a huge number of factors.
 
ah i see.
thank you for the correction, i seem to have missed the fact that there was obviously air being pushed into the flask.
 

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