Exploring the Ideal Gas Law: A Balloon Problem

In summary: The balloon is filled with air, and as it ascends, the pressure outside the balloon decreases because the balloon is getting higher and the atmospheric pressure is greater. The difference in pressure creates a force that pushes the air out of the balloon.
  • #1
Taulant Sholla
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Homework Statement


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Homework Equations


Ideal gas law

The Attempt at a Solution


The solution to this problem assumes the pressure inside the balloon is the same as the outside pressure, i.e. atmospheric pressure. Is this a valid assumption? I would guess otherwise.
 

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  • #2
Taulant Sholla said:
Is this a valid assumption? I would guess otherwise
Don't hot-air balloons have a big opening at the lower end :rolleyes: ?
 
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  • #3
Does this opening mean the inside pressure is always the same as the outside pressure? During it ascent wouldn't the pressure inside differ from the outside pressure?
 
  • #4
It's a big hole.

Let's work out how fast the air must escape to keep the pressure constant... These are only ball park figures. If you disagree post your own sums!...

Atmospheric pressure halves between sea level and about 18,000ft. So the volume of the balloon would double if no air could escape during such a climb. A typical balloon has a volume of 77,000 cubic feet and climbs are typically limited to 500ft/min. So roughly...

77,000* 500/18,000 = 2100 cubic feet/min

Must escape.

If the opening is say 10ft in diameter (a guess) then it has an area of 78 square foot. So the flow rate is..
2100/78= 27 feet per minute or about 6 inches per second. That shouldn't be a problem.

Just for info... At 500ft/min the air flowing down around the outside of the balloon is 500/60=8 feet per second. So the occupants won't notice the air coming out of the balloon.(Although I guess the might when the burner is running.)
 
  • #5
This is *very* clever - thank you! Yes, I suspect that enough air does indeed escape to keep the inside pressure the same as the outside pressure. Thank you again!
 
  • #6
Taulant Sholla said:
This is *very* clever - thank you! Yes, I suspect that enough air does indeed escape to keep the inside pressure the same as the outside pressure. Thank you again!
Of course, there is pressure variation with altitude both inside and outside the balloon. And a [normally plugged] vent hole at the top as well as the one at the bottom. https://www.quora.com/Do-hot-air-balloons-have-a-hole-at-the-top

At the top of the balloon, internal pressure is greater than external pressure. This creates a net upward and outward force on the balloon material near the top. At the bottom of the balloon, internal and external pressure are equalized due to the hole. There is little net downward/inward force.

This pressure variation is the essence of buoyancy. "buoyancy" is nothing more than a word for local fluid pressure integrated appropriately over the surface area of an object. [Which is more conveniently calculated as a volume integral of fluid weight density: the weight of the displaced fluid]
 
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1. What is the ideal gas law and how is it relevant to the balloon problem?

The ideal gas law is a mathematical equation that describes the behavior of an ideal gas. It states that the pressure of an ideal gas is directly proportional to its temperature and number of moles, and inversely proportional to its volume. In the balloon problem, the ideal gas law can be used to predict the behavior of a gas-filled balloon as it is heated and expands.

2. What are the variables in the ideal gas law and how are they related?

The variables in the ideal gas law are pressure (P), volume (V), temperature (T), and number of moles (n). They are related through the equation PV = nRT, where R is the gas constant. This equation shows that as one variable increases, another variable must decrease in order to maintain constant pressure and temperature.

3. Can the ideal gas law be applied to real gases?

The ideal gas law is an approximation and does not perfectly describe the behavior of real gases. However, it can be applied to real gases under certain conditions, such as low pressures and high temperatures. At these conditions, the behavior of real gases is similar to that of an ideal gas.

4. How can the ideal gas law be used to solve the balloon problem?

In the balloon problem, the ideal gas law can be used to calculate the final volume of the balloon after it has been heated. The initial conditions of the gas (pressure, volume, temperature, and number of moles) are known, and by rearranging the ideal gas law equation, the final volume can be calculated.

5. What are some limitations of using the ideal gas law to solve the balloon problem?

Some limitations of using the ideal gas law to solve the balloon problem include not accounting for the effects of gravity or the elasticity of the balloon material. Additionally, the ideal gas law assumes that the gas particles are non-interacting, which may not be the case in real gases. These limitations may result in small discrepancies between the predicted and actual behavior of the gas-filled balloon.

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