Gibbs paradox

In statistical mechanics, a semi-classical derivation of the entropy that does not take into account the indistinguishability of particles, yields an expression for the entropy which is not extensive (is not proportional to the amount of substance in question). This leads to a paradox known as the Gibbs paradox, after Josiah Willard Gibbs who proposed this thought experiment in 1874‒1875. The paradox allows for the entropy of closed systems to decrease, violating the second law of thermodynamics. A related paradox is the "mixing paradox". If one takes the perspective that the definition of entropy must be changed so as to ignore particle permutation, the paradox is averted.
Illustration of the problem.
Gibbs himself considered the following problem that arises if the ideal gas entropy is not extensive. Two identical containers of an ideal gas sit side-by-side. The gas in container #1 is identical in every respect to the gas in container #2 (i.e. in volume, mass, temperature, pressure, etc). There is a certain entropy "S" associated with each container which depends on the volume of each container. Now a door in the container wall is opened to allow the gas particles to mix between the containers. No macroscopic changes occur, as the system is in equilibrium. The entropy of the gas in the two-container system can be easily calculated, but if the equation is not extensive, the entropy would not be 2"S". In fact, the non-extensive entropy quantity defined and studied by Gibbs would predict additional entropy. Closing the door then reduces the entropy again to 2"S", in supposed violation of the Second Law of Thermodynamics.
As understood by Gibbs, and reemphasized more recently, this is a misapplication of Gibbs' non-extensive entropy quantity. If the gas particles are distinguishable, closing the doors will not return the system to its original state - many of the particles will have switched containers. There is a freedom in what is defined as ordered, and it would be a mistake to conclude the entropy had not increased. In particular, Gibbs' non-extensive entropy quantity for an ideal gas was not intended for varying numbers of particles.
The paradox is averted by concluding the indistinguishability (at least effective indistinguishability) of the particles in the volume. This results in the extensive Sackur–Tetrode equation for entropy, as derived next.
Calculating the entropy of ideal gas, and making it extensive.
In classical mechanics, the state of an ideal gas of energy "U", volume "V" and with "N" particles, each particle having mass "m", is represented by specifying the momentum vector "p" and the position vector "x" for each particle. This can be thought of as specifying a point in a 6N-dimensional phase space, where each of the axes corresponds to one of the momentum or position coordinates of one of the particles. The set of points in phase space that the gas could occupy is specified by the constraint that the gas will have a particular energy:
and be contained inside of the volume V (let's say "V" is a cube of side "X" so that "V"="X"3):
for formula_3 and formula_4
The first constraint defines the surface of a 3N-dimensional hypersphere of radius (2"mU")1/2 and the second is a 3N-dimensional hypercube of volume "V"N. These combine to form a 6N-dimensional hypercylinder. Just as the area of the wall of a cylinder is the circumference of the base times the height, so the area φ of the wall of this hypercylinder is:
The entropy is proportional to the logarithm of the number of states that the gas could have while satisfying these constraints. In classical physics, the number of states is infinitely large, but according to quantum mechanics it is finite. Before the advent of quantum mechanics, this infinity was regularized by making phase space discrete. Phase space was divided up in blocks of volume formula_6. The constant h thus appeared as a result of a mathematical trick and thought to have no physical significance. However, using quantum mechanics one recovers the same formalism in the semi-classical limit, but now with h being Planck's constant. One can qualitatively see this from Heisenberg's uncertainty principle; a volume in N phase space smaller than "h"3N ("h" is Planck's constant) cannot be specified.
To compute the number of states we must compute the volume in phase space in which the system can be found and divide that by formula_6. This leads us to another problem: The volume seems to approach zero, as the region in phase space in which the system can be is an area of zero thickness. This problem is an artifact of having specified the energy U with infinite accuracy. In a generic system without symmetries, a full quantum treatment would yield a discrete non-degenerate set of energy eigenstates. An exact specification of the energy would then fix the precise state the system is in, so the number of states available to the system would be one, the entropy would thus be zero.
When we specify the internal energy to be "U", what we really mean is that the total energy of the gas lies somewhere in an interval of length formula_8 around U. Here formula_8 is taken to be very small, it turns out that the entropy doesn't depend strongly on the choice of formula_8 for large "N". This means that the above "area" formula_11 must be extended to a shell of a thickness equal to an uncertainty in momentum formula_12, so the entropy is given by:
where the constant of proportionality is "k", Boltzmann's constant. Using Stirling's approximation for the Gamma function which omits terms of less than order "N", the entropy for large "N" becomes:
This quantity is not extensive as can be seen by considering two identical volumes with the same particle number and the same energy. Suppose the two volumes are separated by a barrier in the beginning. Removing or reinserting the wall is reversible, but the entropy increases when the barrier is removed by the amount
which is in contradiction to thermodynamics if you re-insert the barrier. This is the Gibbs paradox.
The paradox is resolved by postulating that the gas particles are in fact indistinguishable. This means that all states that differ only by a permutation of particles should be considered as the same state. For example, if we have a 2-particle gas and we specify "AB" as a state of the gas where the first particle ("A") has momentum p1 and the second particle ("B") has momentum p2, then this state as well as the "BA" state where the "B" particle has momentum p1 and the "A" particle has momentum p2 should be counted as the same state.
For an "N"-particle gas, there are "N"! states which are identical in this sense, if one assumes that each particle is in a different single particle state. One can safely make this assumption provided the gas isn't at an extremely high density. Under normal conditions, one can thus calculate the volume of phase space occupied by the gas, by dividing Equation 1 by "N"!. Using the Stirling approximation again for large "N", ln("N!") ≈ "N" ln("N") - "N", the entropy for large "N" is:
which can be easily shown to be extensive. This is the Sackur–Tetrode equation.
The mixing paradox.
A closely related paradox to the Gibbs paradox is the "mixing paradox". In fact the Gibb's paradox is a special case of the "mixing paradox" which contains all the salient features. The difference is that the mixing paradox deals with "arbitrary" distinctions in the two gases, not just distinctions in particle ordering as Gibbs had considered. In this sense, it is a straightforward generalization to the argument laid out by Gibbs. Again take a box with a partition in it, with gas A on one side, gas B on the other side, and both gases are at the same temperature and pressure. If gas A and B are different gases, there is an entropy that arises once the gases are mixed. If the gases are the same, no additional entropy is calculated. The additional entropy from mixing does not depend on the character of the gases; it only depends on the fact that the gases are different. The two gases may be arbitrarily similar, but the entropy from mixing does not disappear unless they are the same gas - a paradoxical discontinuity.
This "paradox" can be explained by carefully considering the definition of entropy. In particular, as concisely explained by Edwin Thompson Jaynes, definitions of entropy are arbitrary.
As a central example in Jaynes' paper points out, one can develop a theory that treats two gases as similar even if those gases may in reality be distinguished through sufficiently detailed measurement. As long as we do not perform these detailed measurements, the theory will have no internal inconsistencies. (In other words, it does not matter that we call gases A and B by the same name if we have not yet discovered that they are distinct.) If our theory calls gases A and B the same, then entropy does not change when we mix them. If our theory calls gases A and B different, then entropy "does" increase when they are mixed. This insight suggests that the ideas of "thermodynamic state" and of "entropy" are somewhat subjective.
The differential increase in entropy (dS) as a result of mixing dissimilar gases, multiplied by the temperature (T), equals the minimum amount of work we must do to restore the gases to their original separated state. Suppose that two gases are different, but that we are unable to detect their differences. If these gases are in a box, segregated from one another by a partition, how much work does it take to restore the system's original state after we remove the partition and let the gases mix?
None – simply reinsert the partition. Even though the gases have mixed, there was never a detectable change of state in the system, because by hypothesis the gases are experimentally indistinguishable.
As soon as we can distinguish the difference between gases, the work necessary to recover the pre-mixing macroscopic configuration from the post-mixing state becomes nonzero. This amount of work does not depend on how different the gases are, but only on whether they are distinguishable.
This line of reasoning is particularly informative when considering the concepts of indistinguishable particles and correct Boltzmann counting. Boltzmann's original expression for the number of states available to a gas assumed that a state could be expressed in terms of a number of energy "sublevels" each of which contain a particular number of particles. While the particles in a given sublevel were considered indistinguishable from each other, particles in different sublevels were considered distinguishable from particles in any other sublevel. This amounts to saying that the exchange of two particles in two different sublevels will result in a detectably different "exchange macrostate" of the gas. For example, if we consider a simple gas with "N" particles, at sufficiently low density that it is practically certain that each sublevel contains either one particle or none (i.e. a Maxwell–Boltzmann gas), this means that a simple container of gas will be in one of "N!" detectably different "exchange macrostates", one for each possible particle exchange.
Just as the mixing paradox begins with two detectably different containers, and the extra entropy that results upon mixing is proportional to the average amount of work needed to restore that initial state after mixing, so the extra entropy in Boltzmann's original derivation is proportional to the average amount of work required to restore the simple gas from some "exchange macrostate" to its original "exchange macrostate". If we assume that there is in fact no experimentally detectable difference in these "exchange macrostates" available, then using the entropy which results from assuming the particles are indistinguishable will yield a consistent theory. This is "correct Boltzmann counting".
It is often said that the resolution to the Gibbs paradox derives from the fact that, according to the quantum theory, like particles are indistinguishable in principle. By Jaynes' reasoning, if the particles are experimentally indistinguishable for whatever reason, Gibbs paradox is resolved, and quantum mechanics only provides an assurance that in the quantum realm, this indistinguishability will be true as a matter of principle, rather than being due to an insufficiently refined experimental capability.
Non-extensive entropy of two ideal gases and how to fix it.
In this section, we present in rough outline a purely classical derivation of the non-extensive entropy for an ideal gas considered by Gibbs before "correct counting" (indistinguishability of particles) is accounted for. This is followed by a brief discussion of two standard methods for making the entropy extensive. Finally, we present a third method, due to R. Swendsen, for an extensive (additive) result for the entropy of two systems if they are allowed to exchange particles with each other.
Setup.
We will present a simplified version of the calculation. It differs from the full calculation in three ways:
We begin with a version of Boltzmann's entropy in which the integrand is all of accessible phase space:
The integral is restricted to a contour of available regions of phase space, subject to conservation of energy. In contrast to the one-dimensional line integrals encountered in elementary physics, the contour of constant energy possesses a vast number of dimensions. The justification for integrating over phase space using the canonical measure involves the assumption of equal probability. The assumption can be made by invoking the ergodic hypothesis as well as the Liouville's theorem of Hamiltonian systems.
Liouville's theorem assumes a fixed number of dimensions that the system 'explores'. In calculations of entropy, the number dimensions is proportional to the number of particles in the system, which forces phase space to abruptly change dimensionality when particles are added or subtracted. This may explain the difficulties in constructing a clear and simple derivation for the dependence of entropy on the number of particles.
For the ideal gas, the accessible phase space is an (n-1)-sphere (also called a hypersphere) in the formula_19 dimensional formula_20 space:
To recover the paradoxical result that entropy is not extensive, we integrate over phase space for a gas of formula_19 monatomic particles confined to a single spatial dimension by formula_23. Since our only purpose is to illuminate a paradox, we simplify notation by taking the particle's mass and Boltzmann's constant equal to unity: formula_24. We represent points in phase-space and its "x" and "v" parts by "n" and "2n" dimensional vectors:
To calculate entropy, we use the fact that the (n-1)-sphere, formula_28 has an ("n"-"1")-dimensional "hypersurface volume" of,
For example, if n = 2, the 1-sphere is the circle formula_30, a "hypersurface" in the plane. When the sphere is even-dimensional ("n" odd), it will be necessary to use the gamma function to give meaning to the factorial; see below.
Gibbs paradox in a one-dimensional gas.
Gibbs paradox arises when entropy is calculated using an formula_19 dimensional phase space, where formula_19 is also the number of particles in the gas. These particles are spatially confined to the one-dimensional interval formula_33. The volume of the surface of fixed energy is
The subscripts on formula_35 are used to define the 'state variables' and will be discussed later, when it is argued that the number of particles, formula_19 lacks full status as a state variable in this calculation. The integral over configuration space is formula_33. As indicated by the underbrace, the integral over velocity space is restricted to the "surface area" of the "n"-"1" dimensional hypersphere of radius formula_38, and is therefore equal to the "area" of that hypersurface. Thus
After approximating the factorial and dropping the small terms, we obtain
In the second expression, the term formula_41 was subtracted and added, using the fact that formula_42. This was done to highlight exactly how the "entropy" defined here fails to be an extensive property of matter. The first two terms are extensive: if the volume of the system doubles, but gets filled with the same density of particles with the same energy, then each of these terms doubles. But the third term is neither extensive nor intensive and is therefore wrong.
The arbitrary constant has been added because entropy can usually be viewed as being defined up to an arbitrary additive constant. This is especially necessary when entropy is defined as the logarithm of a phase space volume measured in units of momentum-position. Any change in how these units are defined will add or subtract a constant from the value of the entropy.
Two standard ways to make the classical entropy extensive.
As discussed above, an extensive form of entropy is recovered if we divide the volume of phase space, formula_43, by "n"!. An alternative approach is to argue that the dependence on particle number cannot be trusted on the grounds that changing formula_19 also changes the dimensionality of phase space. Such changes in dimensionality lie outside the scope of Hamiltonian mechanics and Liouville's theorem. For that reason it is plausible to allow the arbitrary constant to be a function of formula_19. Defining the function to be, formula_46, we have:
which has extensive scaling:
Swendsen's particle-exchange approach.
Following Swendsen, we allow two systems to exchange particles. This essentially 'makes room' in phase space for particles to enter or leave without requiring a change in the number of dimensions of phase space. The total number of particles is formula_49:
Taking the integral over phase space, we have:
formula_60
The question marks (?) serve as a reminder that we may not assume that the first "nA" particles (i.e. 1 through "nA") are in system-"A" while the other particles ("nB" through "N") are in system-"B". (This is further discussed in the next section.)
Taking the logarithm and keeping only the largest terms, we have:
formula_61 formula_62
This can be interpreted as the sum of the entropy of system-A and system-B, both extensive. And there is a term, formula_63, that is not extensive.
Visualizing the particle-exchange approach in three dimensions.
The correct (extensive) formulas for systems "A" and "B" were obtained because we included all the possible ways that the two systems could exchange particles. The use of combinations (i.e. "N" particles choose "NA") was used to ascertain the number of ways N particles can be divided into system-A containing nA particles and system-"B" containing" nB "particles. This counting is not justified on physical grounds, but on the need to integrate over phase space. As will be illustrated below, phase space contains not a single "nA"-sphere and a single "nB"-sphere, but instead
pairs of "n"-spheres, all situated in the same "N"+1-dimensional velocity space. The integral over accessible phase space must include all of these "n"-spheres, as can be seen in the figure, which shows the "actual" velocity phase space associated with a gas that consists of three particles. Moreover, this gas has been divided into two systems, "A" and "B".
If we ignore the spatial variables, the phase space of a gas with three particles is three dimensional, which permits one to sketch the n-spheres over which the integral over phase space must be taken. If all three particles are together, the split between the two gasses is 3|0. Accessible phase space is delimited by an ordinary sphere (2-sphere) with a radius that is either formula_65 or formula_66 (depending which system has the particles).
If the split is 2|1, then phase space consists of circles and points. Each circle occupies two dimensions, and for each circle, two points lie on the third axis, equidistant from the center of the circle. In other words, if system-A has 2 particles, accessible phase space consists of 3 pairs of n-spheres, each pair being a 1-sphere and a 0-sphere:
Note that 