Gas Expansion and Compression: Solving for Volume and Pressure Changes

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Homework Help Overview

The discussion revolves around gas behavior, specifically focusing on gas expansion and compression as described by Boyle's Law. Participants are exploring how a gas in a cylinder can fill a balloon of significantly larger volume, raising questions about pressure and volume relationships.

Discussion Character

  • Exploratory, Assumption checking, Conceptual clarification

Approaches and Questions Raised

  • Participants discuss the application of Boyle's Law, questioning how a smaller volume can inflate a larger one. There are inquiries about the relationship between pressure in the cylinder and the balloon, as well as the material limits of the balloon.

Discussion Status

The discussion is active, with participants questioning assumptions about pressure and volume. Some guidance has been offered regarding the implications of Boyle's Law and the physical properties of gases and materials, but no consensus has been reached.

Contextual Notes

Participants note that the problem does not specify the pressure conditions in the balloon or the cylinder, only that the temperature remains constant. There is an ongoing exploration of the implications of these assumptions.

Ronaldo95163
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The first two are the forces questions with my attempt at them...however I don't have the solutions for them and I wanted to know if what I did was correct.

wrt to the gas questions I'm referring to part e


How can a cylinder with only 0.5m^3 fill a balloon to 5m^3

what I was going to do was use the equation for Boyle's law which is V1P1 = V2P2 and use V2 as difference between the volume in the cylinder and the balloon but seeing that the volume in the cylinder is smaller I started questioning that method... :/
 

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Ronaldo95163 said:
How can a cylinder with only 0.5m^3 fill a balloon to 5m^3

what I was going to do was use the equation for Boyle's law which is V1P1 = V2P2 and use V2 as difference between the volume in the cylinder and the balloon but seeing that the volume in the cylinder is smaller I started questioning that method... :/

Why? Don't you realize that gases can be stored at very high pressure in metal cylinders?
 
But if the cylinder has a volume of 0.5m^3 how can it inflate an empty balloon to 5m^3?
 
Is the pressure in the balloon after it is inflated equal to the pressure of the gas in the cylinder?
 
The question didn't say...only thing that was the same was the temperature
 
Think. Is it reasonable to assume that a balloon could withstand being at the same pressure as a gas in a metal cylinder? Why wouldn't gases be stored in balloons instead of metal cylinders?
 
No
The material of the balloon would expand past its elastic limit and it would burst
 
still not getting it :/
 
Go back and ponder Boyle's Law some more. What happens to the volume of a gas originally kept at a high pressure if the pressure is reduced?
 
  • #10
The volume increases

would the work done by the balloon be equal to the work done by the gas in the metal cylinder??

so

(VΔP) of balloon = V(P2-P1) of the cylinder
 
Last edited:

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