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asdf1
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what happens in a free expansion?
What Happens During Free Expansion?
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In summary, a free expansion in thermodynamics refers to the expansion of a gas inside a container where a portion of the container is isolated and then removed, allowing the gas to fill the entire container. The process is adiabatic and no work is done by or on the gas. The first law of thermodynamics states that the initial and final internal energies of the gas are equal, but in reality, there is often a difference in internal energy between the two sides of the container. This process is rarely used in practical applications, but is important in understanding how to apply the first law of thermodynamics.
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Danger
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In my girlfriend's case, I sent her to Weightwatchers.
Sorry, guys; I'm bored.
Sorry, guys; I'm bored.
- #3
russ_watters
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How would that be free, danger?
asdf1, could you be more specific as to what you want to know?
asdf1, could you be more specific as to what you want to know?
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Danger
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The expansion was free. Recompressing her took a few bucks. :grumpy:
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HallsofIvy
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In other words, asdf1, would you please explain what you mean by "free expansion"?
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z-component
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I found this on a Wolfram physics site under Thermodynamic Laws:
"During a free expansion, the energy remains constant."
http://scienceworld.wolfram.com/physics/FreeExpansion.html
"During a free expansion, the energy remains constant."
http://scienceworld.wolfram.com/physics/FreeExpansion.html
- #7
asdf1
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in thermodynamics, what conditions does free expansion have?
what kind of energy is constant? is it the energy absorbed? the work done? internal energy?
what kind of energy is constant? is it the energy absorbed? the work done? internal energy?
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Q_Goest
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Hi Asdf1. A "free expansion" is generally described as the expansion of a gas inside a container in which a portion of the container is isolated from the rest by a diaphragm or wall of some kind. So on one side of the wall you have some gas at a pressure and temperature and on the other side you have a vacuum. The wall is then magically removed and the gas allowed to fill the entire container. Note also this process presumes the contents of the container come to some equilibrium but this is rarely mentioned in the literature but is important because you'll find folks miss this point and redesign the experiment using a valve to separate the two containers. If this happens, such a process really isn't "free expansion" it's a bit different. I'll get to that in a minute.
One can define the process as being adiabatic, though in reality there is always heat transfer but we'll neglect that here. There is also no work done by or on the gas. So if you apply the first law of thermodynamics to this situation, the initial internal energy of the gas is equal to the final internal energy. No energy leaves or enters the volume, so if you wrote the equation for the first law, you'd have dU on one side and all the terms on the opposite side would be zero making dU=0. Not very exciting really. There's an increase in entropy but that's not much fun either. I think the whole point is to get students to consider how to apply the first law, because in reality there's not much you can do with this. I haven't once in almost 20 years come across a case where I'd use it.
There are plenty of cases though where gas might be taken from one container to another through a valve. And I've seen people talk about this in the same terms as the "free expansion" I just explained above, take this one for example: http://www.taftan.com/thermodynamics/FREEEXPA.HTM
Although it is true that the total internal energy is the same in this once the pressures equalize, it is not true that the internal energy for each side is the same. They would have to mix completely and come to equilibrium after the pressures equilized in order for that to occur, so this very misleading. One wouldn't expect mixing to occur very effectively between these two volumes because of the restriction between them. What we find in this case is the gas on the high pressure side (side A) has actually expanded isentropically and all the entropy change is occurring on side B. If you apply the first law to each side independantly, you'll find that to be the case.
One can define the process as being adiabatic, though in reality there is always heat transfer but we'll neglect that here. There is also no work done by or on the gas. So if you apply the first law of thermodynamics to this situation, the initial internal energy of the gas is equal to the final internal energy. No energy leaves or enters the volume, so if you wrote the equation for the first law, you'd have dU on one side and all the terms on the opposite side would be zero making dU=0. Not very exciting really. There's an increase in entropy but that's not much fun either. I think the whole point is to get students to consider how to apply the first law, because in reality there's not much you can do with this. I haven't once in almost 20 years come across a case where I'd use it.
There are plenty of cases though where gas might be taken from one container to another through a valve. And I've seen people talk about this in the same terms as the "free expansion" I just explained above, take this one for example: http://www.taftan.com/thermodynamics/FREEEXPA.HTM
Although it is true that the total internal energy is the same in this once the pressures equalize, it is not true that the internal energy for each side is the same. They would have to mix completely and come to equilibrium after the pressures equilized in order for that to occur, so this very misleading. One wouldn't expect mixing to occur very effectively between these two volumes because of the restriction between them. What we find in this case is the gas on the high pressure side (side A) has actually expanded isentropically and all the entropy change is occurring on side B. If you apply the first law to each side independantly, you'll find that to be the case.
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asdf1
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wow! thank you for the very clear explanation! :)
1. What is free expansion?
Free expansion is a thermodynamic process in which a gas expands into a vacuum or an empty container without any external work being done on the gas.
2. What happens to the temperature during free expansion?
The temperature of the gas remains constant during free expansion. This is because the expansion occurs quickly and there is not enough time for heat transfer to occur.
3. Does the pressure change during free expansion?
Yes, the pressure of the gas decreases during free expansion. This is because the volume of the gas increases while the number of gas molecules remains the same.
4. Is free expansion an irreversible process?
Yes, free expansion is an irreversible process. This means that the gas cannot spontaneously return to its original state without external work being done.
5. What is the equation for calculating work in free expansion?
The equation for calculating work in free expansion is W = -PΔV, where W is work, P is pressure, and ΔV is the change in volume. Since there is no external pressure acting on the gas during free expansion, the work done is zero.
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