its about the thermodynamics where we see the entropy and also using the 2nd law of thermodynamics.
205765
Please go to this website to find your answer:\nhttp://en.wikipedia.org/wiki/Exergy\n\nIn thermodynamics, the exergy Ξ of a system with respect to a reservoir is the maximum work done by the system during a transformation which brings it into equilibrium with the reservoir.[1] The term was coined by Zoran Rant in 1956. The concept, however, has existed since W. Gibbs (1873), i.e. ‘available energy of the body and medium’, and G. Gouy (1889), i.e. ‘possibility of obtaining work’.\n\nThe term exergy is also used, by analogy with its physical definition, in information theory related to reversible computing. Exergy is also synonymous with: availability, available energy, exergic energy, essergy (considered archaic), utilizable energy, available work, maximum (or minimum) work, reversible work, and ideal work.\n\nExergy of heat available at a temperature\nCarnot efficiency is\n\n n = 1-(T<c>/T<h>)\nwhere TH is the higher temperature and TC is the lower temperature, both as absolute temperature. From Equation 1 it is clear that in order to maximize efficiency one should maximize TH and minimize TC.\n\nFor calculation of exergy of heat available at a temperature there are two cases: the body releasing heat is higher than the surrounding, or, the temperature of the body is lower than the surrounding.\n\nExergy fraction of heat available at a temperature higher than the surrounding is:\n\nE/Q = 1 - (T<o>/T<h>)\n \nwhere Th is the temperature of the heat source, and To is the temperature of the surrounding.\n\nExergy of cold is though:\n\nE/Q = 1 - (T<c>/T<o>) \n\nwhere Tc is the temperature of the cold body that is receiving heat from the surroundings.
9501
Some systems actually cool as they deliver power.  A rubber band is most common example I can think of.  If you expend energy to stretch a rubber band, it actually heats up, but it cools slightly as it contracts, which could potentially power some small device like a toy car.  Why this occurs is a little complicated, but the exact same principle of entropic cooling is used to achieve the lowest temperatures currently possible.\n\n***Response to first answerer***\nWhat basic law of motion are you talking about?  The second law of thermodynamics? Because that deals with entropic differences, and doesn't apply. The "laws of motion" aren't even relevant to this thermodynamics question.  \n\nI used the example of a rubber band because it is a clean example of entropic cooling, but in fact ANY  heat engine will result in a decrease in thermal energy of the system. It's true that there is some heat produced from friction in the engine, but on a whole more MORE heat flows into the engine than flows out.  The average temperature of the system decreases. That's why we can use heat engines to power things.
122077
The description of entropy as the tendency to descend into chaos is incorrect. Entropy actually describes the amount of usuable energy in a material. It has a statistical interpretation, but even that is closer to saying that the state of a system gets more probable over time.\n\nNext, when working with entropy, it's important to realize that it is only required to increase in a closed system, that is, one that has *no* heat or energy exchange with anything else. For a tree, there is a lot of energy coming in through sunlight. And, in fact, it is the energy of sunlight that drives the local decrease in entropy.\n\nThere is another quantity, called the Gibbs free energy, that is a combination of entropy, temperature, and the energy of a reaction that is more appropriate for non-closed systems. It is described by H-TS, where H is the energy of the reaction, T is the temperature, and S is the entropy. The Gibbs free energy is what must decreasein systems that are not closed (and under constant pressure).
53640
Don't listen to the first answer, he didn't even bother to look it up.\n\nThe second law of thermodynamics is more about the direction of energy flow.  It is really a statement about the 1st law and how many of it's processes never take place.\n\nFrom it, you get things like "Heat will not flow spontaneously from a colder body into a warmer body." And "Heat energy can not be compleaely transformed into mechanical work." Also, "It is impossible to construct an operational perpetual motion machine."\n\nIf evolutionists heads explode over this it is because of the consistant and repeated misuse of this by creationists.  In fact, most of the major creationists now conceede that they have been way off on this for a long time.  It does really make me worry about the education system in this country when creationists still think they can go around saying this.  \n\nOK, one more time: The second law and entropy apply to CLOSED SYSTEMS.  Since you haven't even bothered to research this - news flash! - THE EARTH IS NOT A CLOSED SYSTEM.  This may be new to some creationists but their is a big ball of fire out there called the sun where the earth gets most of it's energy.  Living things use energy from lower trophic levels to assemble new molecules.\n\nEvery time one of these creationist think that this is a valid argument, how come they never wonder why their aren't a bunch of physicits pointing this out to biologists?
353989
Entropy is the change in heat energy, Q, over a given temperature, T.\n\nIf you are familure with calculus, the ideal gas law, and the first law of thermodynamics then you can derive it.\n\ndS = dQ/ T  (change in entropy per change in heat)\n\nSince the tempurature is not constant you will have to use the first law of thermodynamics\n\ndQ - dW = dEint   \n\nUsing the ideal gas law \n\nPV = nRT \n\nand the fact work is \n\ndW = PdV \n\nand \n\ndEint = nCvdT \n\nyou can write an equation for a non-isothermal and non-isochoric situation:\n\nS = nR ln (Vf/Vi) + nCvln(Tf/Ti)\n\nWhere\nS - change in entropy\nn - number of moles\nR - gas constant\nVf - Final Volume\nVi - Initial Volume\nCv - specific heat\nTf - Final temperature\nTi - Initial temperature
314453
This would not be possilbe.  In the process of digesting and assimilating these essential elements, our bodies create some waste or by-products.  We have to get rid of it somehow.\n\nOur bodies are not Carnot engines - we cannot attain 100% efficiency.  The second law of thermodynamics tells us this (entropy is increasing).\n\nPlus, there are very few pleasures as great as sitting down and passing a nice well-formed turd.
654789
First Law of Thermodynamics: Energy can be changed from one form to another, but it cannot be created or destroyed. \n\n"You can't win."  Because you can never get more energy than you start with.\n\nThe Second Law of Thermodynamics states that "in all energy exchanges, if no energy enters or leaves the system, the potential energy of the state will always be less than that of the initial state." \n\n"You can't break even."  Because you lose potential energy.  It changes to heat.
264089
Its infinitely larger than any other heat capacity measured for a substance on earth.  Hence it is infinite relative to all other heat capacities.
8002
Also note that entropy formulation has a modified form to include relativity which is the case for black holes.
459581
The second law of Thermodynamics has to do with Entropy.  Entropy is the tendancy of a closed system to move to a higher degree of disorder (lower energy state).  Life itself breaks the second law of thermodynamics, at least for the short term.  When a seed is planted, or when an animal or child is created by it's parents, a single cell grows into a more complicated, higher energy structure (life).  However, on the way there, the organism does consume more energy than it gives back, so conservation of energy is never lost either.  \n\nThe theory of evolution would be another example that would break the 2nd Law.  I am not arguing for or against the theory of evolution, I am just stating the the theory.  If a single celled organism evolves into a multi-celled organism, that's a more complicated structure with more energy.  Again, this is considered to be a short-term gain.  The one thing that Entropy has working against it is time.  In the short-term, physical processes like life seem to beat Entropy, then entropy seams to catch up (death).  However, in the extremely long term (cosomolically speaking, 1 * 10 ^76 years or more), entropy never completely catches up with time.\n\nHere's a quote from a great book on cosmology (The Five Ages of the Universe. by Fred Adams and Greg Laughlin, published by Simon and Schuster New York, copyright 1999, Page 168.)\n\n"The universe effectively doles out a fixed amount of energy over an infinite span of time.  This conservation practice underscores the energy crisis of the future and defines exactly what it means for the universe to 'slow down' as it gets older.\n     The universe thus slows down dramitically, but never quite runs out of steam.  Can one think of the universe, with this never-ending quality as having an eternal life?  Perhaps, but that would be rather optimistic point of view, Paul Davies, a renowned physicist and writer, has described this late phase of the evolution of the universe as an 'eternal death'.  This ever dying universe continues to evolve and continues to slow down, but never reaches a final moment of deathlike closure.\n   No matter how old the universe becomes, interesting physical processes continue to operate."
440686
Bernoulli's principle can be tried.\nLaws of forces can be demonstrated.\nThermodynamics-transfer of heat.....etc
70633
It depends on exactly what you are after here. Is the intention to make the point that since entropy is a thermodynamic property of the system, if the entropy of state 1 is s1 and that of state 2 is s2, then the entropy difference is s2-s1, regardless of how one transits between the states? However, in any real process there is, if one considers both the system and the surroundings, always a net increase in entropy. Of course, reversible processes are ideal constructs. In this sense the irreversible process will have the higher entropy increase.
361050
1. concentration and pressure\n2. see sources
129839
Basically its just when something goes from a liquid to a solid the entropy decreases and so you show the decrease in entropy values which should be in your chemistry. And when something goes from a solid to a liquid, the entropy increases and liquid to a gas, it increases. You should use the entropy values and show the change between the states. That would be the work I would show
74634
No, according to the third of THERMODYNAMICS. \nThe TOTAL ENTROPY of the Universe increases with every SPONTANEOUS PROCESS.\n\nThere you have it, the answer is clear.\nI hope I helped!\nThankyou!
454524
Entropy -- the second law of thermodynamics.\n\nThis law states that in the absence of other forces, any system becomes less orderly over time.  This is because of the way energy can be converted to different forms but not lost -- most energy that gets used for work transforms into heat, which radiates into space and can't be used to do useful work ever again.  In other words, energy gets used up, and with no more energy input things fall apart into entropy, or complete disorder.\n\nBUT -- the key there is "in the absence of other forces."  We, for example, on earth have our sun which continuously supplies energy to us with which useful work can be done.  As long as there is an external supply of energy, entropy can be avoided.  Once our sun burns out, however, our solar system is indeed doomed to entropy.
244112
Well, if you get something with the second to lowest potential energy in the world, that energy can go to the lowest potential energy thing in the world and that's it.  Otherthan that, no.  And there's nothing inherent in the material, unless you're talking about chemical reactions, in which case, I just don't know what those two things are.  I hope that's clear.