Chemistry - Ideal gas equation question

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Discussion Overview

The discussion revolves around a problem involving the ideal gas equation, specifically how to calculate the new pressure of oxygen gas in a steel bottle after a portion of the gas is released, while assuming constant temperature. Participants explore the application of the ideal gas law in this context.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant presents a problem involving the release of gas and seeks help in calculating the new pressure, expressing difficulty in isolating P in the ideal gas equation.
  • Another participant suggests using the ideal gas law (PV = nRT) and notes that the number of moles (n) changes while the volume (V) remains constant.
  • A different participant proposes calculating pressure per mole and arrives at a pressure of 5429 Pa, indicating they are still learning the subject.
  • Another response reiterates the ideal gas law and provides a formula for calculating the new pressure based on the initial pressure and the change in moles, yielding a different result of 5482 Pa.

Areas of Agreement / Disagreement

There is no consensus on the final pressure value, as participants arrive at different results (5429 Pa and 5482 Pa) based on their calculations. The discussion remains unresolved regarding the correct pressure after the gas release.

Contextual Notes

Participants do not clarify the assumptions regarding the ideal gas behavior or the specific conditions under which the calculations are made, such as the exact volume of the gas bottle or the temperature stability.

Who May Find This Useful

Students learning about the ideal gas law and its applications in practical scenarios may find this discussion relevant.

david18
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A steel gas bottle contains 4500g of oxygen. The pressure of the gas inside the bottle is 6492Pa. If 700g of gas are slowly released from the bottle, what will be the new pressure of the remaining gas? (Assume that the temperature stays constant when the oxygen is released)

I'm having trouble with this question as I can only find PV but not P on its own.

Thanks
 
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Use PV = nRT before and after the release.
You know the change in 'n' the number of moles, and V stays the same, volume of bottle doesn't change.
 
Would you take the Pa/mol and multiply that by the final mol. I get 5429 Pa. I am learning this subject as well, so I am curious.
 
PV = nRT
V is constant, T is constant, R is constant (obviously!) so all you need is P/n before and after. YOu can work in totally arbitrary units for n since we are cancelling thme out

P1/n1 = P2/n2
P2 = P1 n2/n1 = 6492 * (4500-700)/4500 = 5482 Pa
 

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