|WikiProject Physics||(Rated C-class, Mid-importance)|
|WikiProject Meteorology||(Rated C-class, Mid-importance)|
- 1 Accuracy Dispute & Changes, 2008-03-26
- 2 Continental and local scale
- 3 Edit, 2006/01/30
- 4 added 2006-01-04
- 5 Symbol for the ratio of specific heats
- 6 Adiabat?
- 7 Derivation of TV^gamma-1
- 8 Adiabatic Internal combustion Engine
- 9 Discrete Formula
- 10 No heat being transferred is necessary but not sufficient
- 11 plot
- 12 Adiabatic process in liquid (for instance, water)
- 13 Possible Plagiarism
- 14 Just wrong
- 15 Relation to adiabatic theorem
- 16 When is adiabatic not adiabatic?
- 17 Needs a correction....
- 18 Adiabatic vs adiathermal
- 19 Equation derivation
- 20 question about "derivative"
Accuracy Dispute & Changes, 2008-03-26
I made several changes to the article, and more may be needed. In order of appearance on the page:
1) Paragraph 3 previously stated:
"...A transformation of a thermodynamic system can be considered adiabatic when it is quick enough that no significant heat is transferred between the system and the outside. The adiabatic process can also be called quasi-static..."
The second sentence is confusing or simply incorrect; a quasi-static process is one in which all states can effectively be considered equilibrium states (see quasi-static), which seems to apply better to a case when the gas does come into thermal equilibrium with the outside of the system. Although a quasi-static assumption may be necessary for a reversible process (don't know this for sure), it is certainly not necessary for an adiabatic process (e.g., a rapid, irreversible gas expansion where inertial effects are important). I have removed it to avoid confusion.
2a) In the "Adiabatic Heating and Cooling" section, Paragraph 2 previously stated:
Adiabatic cooling occurs when the pressure of a substance is decreased, such as when it expands into a larger volume. An example of this is when the air is released from a pneumatic tire; the outlet air will be noticeably cooler than the tire.
The phrase "such as when it expands into a larger volume" suggests a gas flowing into a larger volume or reservoir, which is incorrect. The spirit of the sentence is that gas increasing in volume undergoes adiabatic cooling, but this is ambigious in the original wording. I have replaced it with "...the pressure of a substance is decreased as it does work on its surroundings," which is closer to the reality. However, this still doesn't mention a volume increase, which would be nice to have (i.e., an explanation of the fact that a gas increasing in volume and thus decreasing in pressure--or vice versa--does work on its environment, and thus cools).
You failed to note refrigeration and industrial air compression.
Heat becomes a real problem in pneumatic systems, requiring intercoolers on two and three stage machines over about 10 HP. It would be simpler and clearer to note that all gasses (except Bose Einstein condensates at 0 K) contain heat. Compressing the gas increases the temperature. Draw off air and the tank -- and the tool -- both cool down considerably.
You also failed to note precipitation. ALL adiabatic (as compared to isothermal) compressor systems precipitate water, dust, CO, CO2, and other materials from atmospheric air. Linde's Principle states that gas will not liquefy until it reaches the Linde Limit. Pressurize air sufficiently, cool the compressed gasses enough, and the gasses will condense to liquids, one at a time. Pardon me if I defer to release proprietary information.
The primary use for adiabatic technology is refrigeration. Condenser units pressurize refrigerant, run air (or with chilled water systems, water) over the coils, pulling heat from the refrigerated space. Reverse the process (by valving) and we suddenly have the normal home heat pump. —Preceding unsigned comment added by 184.108.40.206 (talk) 20:24, 17 April 2008 (UTC)
2b) I removed the example of air being released from a pneumatic tire in the quote above, as the cooling is partially due to the Joule-Thomson effect, not entirely due to adiabatic expansion. Some cooling due to adiabatic expansion may be observed inside the tire itself (the volume of gas which remains in the tire at any given time is expanding and doing work on the exiting air), but this does not account for the reason air may feel cold as it just begins to exit the tire. Adiabatic expansion may be noticeable as a decrease in the temperature of the tire though how much so depends on the heat capacity and mass of the rubber relative to those of the gas.
A good analogy here is an aerosol can. The can cools in your hand as it is sprayed due to evaporation of the fluid inside (similar to adiabatic expansion), and the stream coming out of the nozzle is cooled by some combination of adiabatic expansion and the Joule-Thomson effect.
It would be nice if someone could find a good "everyday life" example for this section that does not include a dissipative/irreversible process, though... the best I can think of right now is a vacuum pump (when gas is expanded by a piston inside a cylinder), but I don't think many people will be able to relate to this, and it's not immediately apparent that the gas does net work on the piston as is required for adiabatic cooling (it seems to be the other way around at first glance). Perhaps a pneumatic piston motor would work well, where expanding high-pressure gas does work on a piston, and should come out colder than it went in?
3) In the "Ideal Gas" section, Paragraph 1 previously stated:
"The mathematical equation for an ideal fluid undergoing an adiabatic process is"
This entire section is only valid for a reversible (isentropic) process, and does not apply to, say, a mass passing through a throttle (even though this is an adiabatic process). I've updated the section heading, introductory sentence, and the beginning of the second paragraph ("For adiabatic processes, it is also true that") to reflect this. However, more changes may be needed throughout the section, and it would be nice to have an explanation of why this applies only in the reversible case... in short, it's because the work on a gas volume does not equal PdV any more, but some things may be said about inertial or viscous effects, quasi-statics (relating to pressure changes and reversibility, not thermal interactions with the system boundary), etc.
Thanks in advance for any contributions to the article!
Continental and local scale
can you help me with a continental or global scal in the atmosphere and a local or regional scale
Continental or Global scale would be the Hadley cell and a local or regional scale would be sea and land breezes. Hope this helps!
I edited the section on adiabatic heating/cooling. The "coolness" felt when pursing one's lips and blowing on one's own skin is due almost entirely to enhanced convective heat transfer; the actual air temperature drop is so small (due to the tiny pressure drop involved) that if one blows on a thermometer in this manner, there will be a negligible temperature change.
I instead offered the different example of deflating a tire, where the pressure drop is on the order of several hundred KPa (several dosen psi); I have seen frost form on valve stems because of this.
Also added the more extreme heating example of a motorized air compressor operating at higher pressures than a bicycle pump.
Joe Frickin Friday 17:54, 30 January 2006 (UTC)
Very similar effect occurs when looking at a Methonol Cannon, you can observe this phenomenon very easily
in 'Derivation of formula' section equation (3) there is dE = something - shouldn't it be dU ?
Symbol for the ratio of specific heats
I fully realize that the Greek letter gamma () is used by physicists and others as the symbol representing the ratio of specific heat at constant pressure to the specific heat at constant volume. However, I would like to point out that thousands of engineers worldwide use a lowercase k to represent that ratio. I strongly believe that this article should mention that fact. mbeychok 00:10, 1 March 2006 (UTC)
So, what exactly is an adiabat shit? The article doesn't make this clear. Jonabbey 04:31, 7 June 2006 (UTC)
- I belive it is a line on a graph that indicates 0 heat flow along that line, like an isotherm is a line denoting constant temperature.
- Correct. An adiabat is a curve on the pV graph where Q=0. An adiabatic process is one that follows one of these curves. An adibat is always steeper than an isotherm. 220.127.116.11 00:51, 11 December 2006 (UTC)
- No, an adiabat is a curve with constant entropy (i.e. its an "isentrope"). Q (or δQ) is not a state function, so there are many curves through the same point that could be adiabatic, but only one that is isentropic. PAR 02:58, 11 December 2006 (UTC)
Derivation of TV^gamma-1
The derivation of TV^gamma-1 is a lot longer than the one in my physics text book (Young & Friedman 11th ed.) and doesn't explain what Cv is. I'd fix this myself, but my mathML sucks. 18.104.22.168 00:51, 11 December 2006 (UTC)
We are doing a project on the adiabatic process and we need a lot of help. Can anyone help us? 22.214.171.124 13:42, 28 February 2007 (UTC)Paco and Taco
Something seems wrong to me: Equation (1) states that dU = - δW, whereas first equation below equation (4) states that δW = - p dV = α p dV + α V dp = dU, i.e. δW = dU. Giving that the end of the derivation is correct, there should be a confusion between the physical definition of work (work done by the system) and the chemical one (work done on the system). Equation (1) is valid for physical work definition. Question: is equation (2) valid for physical work or chemical work ? Parey (talk) 08:07, 25 January 2008 (UTC)
Adiabatic Internal combustion Engine
Fountain Powerboats of Washington NC claims to have created an adiabatic internal combustion engine based upon a marinized Chevrolet engine. Though the project has not proven publicly it is really an adiabatic cycle engine it has demonstrated extreme power production. Anyone care to propose how this would work?
Jsmithnc 20:25, 13 August 2007 (UTC)
It looks like something is wrong with the final form of the discrete formula derived - if you just plug in the ideal gas law for t2 and t1 and cancel things, you get alpha=-1 always. This can't be right - alpha depends on the degrees of freedom for the particular molecules (ndof/2), and could take on many values. —The preceding unsigned comment was added by 126.96.36.199 (talk) 07:15, August 21, 2007 (UTC)
No heat being transferred is necessary but not sufficient
E.g. if an isolated system undergoes a rapid change leading to entropy production, then that is not an adiabatic change. At least not in theoretical physics (I'm not sure about engineering or chemistry, they often teach physics in a flawed way) :)
In practice, it may well be the case that systems undergoing a rapid change are closer to the ideal adiabatic process than systems that change slowly, because in practice the heat transfer issue may be more important than entropy production. But one always has to explain things from the fundamentals and then explain how it is (approximately)realized in real world phenomena.
I believe that the figure is incorrect, as it shows "work done" as the region between the adiabatic expansion line and the x-axis. Work done should be the region between the adiabat line to the final state.188.8.131.52 (talk) 08:32, 17 April 2009 (UTC)
- Each thermodynamic cycle can be split into separated to multiple thermodynamic processes, with an adiabatic process being just one of several types of thermodynamic processes.siNkarma86—Expert Sectioneer of Wikipedia
86 = 19+9+14 + karma = 19+9+14 + talk 22:48, 16 September 2011 (UTC)
Adiabatic process in liquid (for instance, water)
The article describes case of ideal gas; there is no information about real gases or liquids. Consider the following problem, for instance:
Temperature of water in ocean is 12oC, and temperature coefficient of expansion is equal to 9.2*10-5 K-1. Some water moves from the surface to the bottom (1km under surface) quickly (thus, it doesn't exchange heat with other water). Find the approximate change of its temperature. Wikiwide (talk) 23:46, 13 April 2009 (UTC)
Here's the deal. I give you the solution to the problem: Here it is:
(the reply by me (Count Iblis), of course :) )
While reading the article I've seen a few lines that look eerily familiar. At the same time some of the derivations are literally straight out of a textbook. I'll be the first to admit that a derivation is a derivation so I highly doubt that those are clear indicators, but the article really does read like it may have been copied out of one or many textbooks.
At the moment I cannot substantiate this claim, but I think it warrants some research. If in fact the article is copied word for word we should be careful not to delete the page wholesale but salvage the bits of it that are legitimate, namely the derivations and equations which, as far as I know, cannot be copy-written.
- "If in fact the article is copied word for word we should be careful not to delete the page wholesale but salvage the bits of it that are legitimate, namely the derivations and equations which, as far as I know, cannot be copy-written." When will the world realize that there are only so many ways to say something concisely? We will reach a point where certain small points are off-limits to a free encyclopedia simply because copy-written material has all but exhausted every way of making a point that doesn't waste the reader's time.siNkarma86—Expert Sectioneer of Wikipedia
86 = 19+9+14 + karma = 19+9+14 + talk 22:04, 16 September 2011 (UTC)
An adiabatic process must involve both no heat transfer with the surroundings (adiathermal) AND it must be reversible. See "Concepts in Thermal Physics" by Blundell and Blundell. — Preceding unsigned comment added by 184.108.40.206 (talk) 21:28, 4 December 2011 (UTC)
- I agree that some textbooks define it that way, but many don't. In theoretical physics, one would rather not define adiabatic to be also (potentially) an irreversible process (because that would bring it in conflict with another notion of "adiabatic" used in physics). But in engineering it is common to use "adiabatic" also for irreversible processes. I think in the book by Reif a comment is made about this, and Reif prefers not to use the word "adiabatic" at all to avoid confusion. Count Iblis (talk) 22:29, 4 December 2011 (UTC)
Relation to adiabatic theorem
Could someone explain the relation to adiabatic theorem. One says that family of differential equations $L(x',x,t,p)=0$ parametrized by parameter $p$ satisfies adiabatic theorem, if denoting solutions of $L(x',x,t,p)=0$ by $x(t,p)$, one has $x(t,p(t))$ are close to the solutions of $L(x',x,t,p(t))=0$, if dependence of $p(t)$ is "slow" (derivative is small). I know, that Hamiltonian dynamics satisfies adiabatic theorem, but relation to heat transfer eludes me. Slava Matveev. 220.127.116.11 (talk) 14:00, 10 December 2012 (UTC)
When is adiabatic not adiabatic?
.... when it's contained in this article.
- Adiabatic heating also occurs in the Earth's atmosphere when an air mass descends, for example, in a katabatic wind or Foehn or chinook wind flowing downhill over a mountain range. When a parcel of air descends, the pressure on the parcel increases. Due to this increase in pressure, the parcel's volume decreases and its temperature increases, thus increasing the internal energy.
If the internal energy (which can only be kinetic, i.e. heat) increases the process cannot be adiabatic. Increasing pressure doesn't affect the kinetic energy of the molecules. That violates the first law of thermodynamics. This article is as muddled as Lapse rate is as far as the description of adiabatic processes goes. Rambler24 (talk) 23:02, 2 March 2013 (UTC)
- Increasing the pressure DOES increase the kinetic energy of the molecules. Compressing a given amount of gas adiabatically increases its temperature. For a fixed amount of gas undergoing a reversible (i.e. slow) process, and for an adiabatic process, so that . You do work on a gas and subtract none by thermal means, its internal energy increases. Increasing the pressure by compression increases the kinetic energy of the particles. Intuitively, if you have piston that is compressing the gas, the particles are bouncing off the piston wall, which is moving towards them, so their energy after the collision is increased. If the process is done very slowly, then yes, the amount of energy added per collision becomes very small, but it takes a longer time, (so more collisions) to accomplish a given volume decrease. So the product of the two stays the same, its the amount of work done during that volume decrease, and that's the increase in internal energy (i.e. kinetic energy of the particles). PAR (talk) 05:38, 3 March 2013 (UTC)
Here are 2 flaws in the article's wording and why PAR's response doesn't answer Rambler's objection: 1) "Adiabatic heating occurs when the pressure of a gas is increased from work DONE ON IT by its surroundings, e.g. a piston compressing a gas contained within an adiabatic cylinder." If this process is adiabatic, the compression occurs without hitting any of the gas in the cylinder. The gas is the system, the piston is part of the environment, and you only move the piston when there's a thin disk of evacuated volume next to the piston. The gas's pressure increases not because its molecules are sped up, but because they are confined to less volume. The article's wording implies to some readers that the gas itself is being moved by the compression, but it's the gas's BOUNDARIES that are moved. We don't have to fudge anything or bring up differentials and round them to 0.
2) The part that says "the parcel's volume decreases and its temperature increases, thus increasing the internal energy" and the part below that says "as the volume increases, the temperature falls and internal energy decreases" are technically correct for the real gases described, but they imply that the internal energy change is a result of the adiabatic change in system volume. The change in internal energy happens only due to the interactions that AREN'T adiabatic, the ones that we fudge over to call the process adiabatic. A change in internal energy directly contradicts the process being adiabatic. An ideal gas in the pure adiabatic process would have no change in internal energy. 18.104.22.168 (talk) 23:38, 27 March 2013 (UTC)
- Rambler24 has written If the internal energy increases the process cannot be adiabatic. I ask that he explain where that comes from, or why he believes it to be correct.
- I believe it to be incorrect. I can offer the following explanation of my belief. Imagine a gas in an insulated cylinder, underneath a movable piston. Mechanical work is done on the piston in order to reduce the volume of the gas and increase its pressure and temperature. Unless heat begins to flow into the walls of the cylinder and piston, no transfer of heat occurs so the process is adiabatic (and reversible). However, the temperature of the gas has increased significantly so its internal energy has increased too. In fact, the increase in internal energy exactly matches the mechanical work done on the gas (and on the piston). Dolphin (t) 23:54, 27 March 2013 (UTC)
Dolphin, an increase in temperature doesn't have to equal an increase in internal energy. You can add heat to a system, increasing its internal energy, without changing its temperature, if it's allowed to expand. Likewise, you can increase a system's temperature by adiabatically compressing it (imagine a really diffuse gas that would be easier to compress without hitting the gas), without adding any internal energy to the gas's molecules. A volume's temperature is a function of not just average kinetic energies of its molecules, but also of the total number of molecules and the total volume. Adding heat to a system by definition increases its internal energy. 22.214.171.124 (talk) 00:14, 28 March 2013 (UTC)
- I"m afraid that the article as it stands, as well as PAR and Dolphin51 are all quite correct. "Adiabatic" means that no heat is being transfered in or out of a sytsem, not that no work is being done on or by the system. In an adiabatic process, the system is quite free to do work, or have work done upon it. It's simply insulated from HEAT transfers, but NOT from "heating up" or "cooling off" (changing temperature). It is only forbidden to change temp as a result of HEAT going in or out directly. Temperature of the system can go up, down, or stay constant. The same is true of the internal energy of the system, which now is simply driven by the PV work done by (or to) the sytsem.
I do not know where Ramber24 and the IP (perhaps they are the same?) got the odd idea that "adiabatic" had something to do with no PV work.
Finally, I don't know how we started to treat the odd idea of a "Maxwell's demonic" spontaneous compression, where we confine a gas to a smaller volume merely by waiting until it exerts no piston pressure, then quickly move the piston in, so we get the compression free with no PV work. You can let a gas expand that way, and an ideal gas indeed does not change temperature. But you can't compress a gas that way unless you're Maxwell's demon. Good luck with that, as you'd be able to do all kinds of entropy-decreasing things. In the real world, the problem of figuring out where the gas molecules are located, so you can figure out when to move the piston without moving it against the force of impacts (thus doing PV work), would defeat you. BTW, even if you managed this (defeating the second law) the first law would ensure that you got nothing directly for it, and the gas temperature (ideal gas) would no more change in such a "spontaneous contraction" than it does in a sponteous isothermal expansion. After all, where would the energy come from, to change the temperature of the gas? You did no work on it. You didn't heat it. Its internal energy must therefore stay the same as always. SBHarris 02:40, 28 March 2013 (UTC)
We got the maxwell's demon part from me not understanding that even though I would say in conversation that compressing a gas 'heats' it, that is formally wrong. Not realizing that, then to make sense of adiabatic processes involving no heat transfer, I had to imagine a way to increase the system's pressure without giving it any energy. On top of that I thought the temperature would go up in a volume if its molecules maintained their energies but were concentrated into a smaller volume, using the colloquial notion that my cozy room would feel colder if the air was rarer but the molecules still had the same average kinetic energy. Bam, there you have it. I cringe at how epically wrong I was on this page and am glad to be corrected. 126.96.36.199 (talk) 04:27, 28 March 2013 (UTC)
Needs a correction....
Three-fourths down this thread it is stated "Substituting γ=(α+2)/α" that seems incorrect. Should it not be "Substituting γ=(α+1)/α" ? If so, the following derivation may need updating. — Preceding unsigned comment added by 188.8.131.52 (talk) 17:01, 12 May 2013 (UTC)
Pondhockey (talk) 04:14, 18 April 2014 (UTC) It seems to be a tradition within thermodynamics to omit the variable of differentiation (differentiation with respect to what?) A link to an explanation would be very helpful to outsiders (such as myself) who have no clue what dU = ... even means.
Adiabatic vs adiathermal
- The two terms describe very different and mutually exclusive systems. Which term is more suited depends on what kind of system is being described. VQuakr (talk) 18:11, 10 June 2014 (UTC)
- With respect, I think an adiathermal wall is just the same thing as an adiabatic wall, at least in macroscopic thermodynamics. They both pass energy as work but not as heat, and do not pass matter.
- I would be interested in VQuakr's reasons for his apparently differing view when talking of a process as distinct from a wall. Perhaps he is thinking of the near inversion of meaning that is described in the article in the section Usage of the word adiabatic, referring to a special usage in quantum statistical mechanics?
question about "derivative"
- It is customary to start a new section at the bottom of the page, as here, for a question like this. If the first character in a line of edit is a blank, then the line is put into a box.