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Ideal-Gas Law Question

  • Thread starter kop442000
  • Start date
34
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1. Homework Statement
A hot-air balloon has a volume of 1.5m^3 and is open at the bottom. If the air inside the balloon is at temperature of 75C, while the temperature of the air outside the balloon is 24C, at a pressure of about 1 atm, what is the net force on the balloon and its contents? (Neglect the Weight of the balloon itself).



2. Homework Equations



3. The Attempt at a Solution
I know that this question is about the ideal-gas law, but for some reason I just can't think how to do it.
 

Kurdt

Staff Emeritus
Science Advisor
Gold Member
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Force is pressure times area. This is all about the pressure of the gas inside the balloon.. That should be enough to get you going.
 

Doc Al

Mentor
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Consider Archimedes' principle. How does the density of the air inside the balloon compare to that outside?
 
34
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So to find the density, I presume I first find the number of moles in the balloon using the ideal gas law. But to do so, can I assume that the pressure inside the balloon is the same as the pressure outside?

When I do this, I calculate 35 moles per m^3. This leads me to a density of just over 1kg/m^3. This is compared to the density of the air outside of 1.19kg/m^3

Oh.. ok I got it. So now I just figure out how much more gravity would pull down 1.5m^3 of the normal density air, and this is the force on the balloon.

Initially my problem was just that I wasn't sure if I could assume pressure inside to be equal to outside - because I thought the material of the balloon would add its own elasticity to the forces making the balloon smaller - but I guess because the bottom of the balloon is open this never becomes an issue.

Anyway, thanks for the help!
 

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