Just learnt about it recently, and I'm curious to understand more. The 'mixing' form of the paradox goes something like this:

Imagine a box partitioned in the middle. The two partitions are the same volume. In each there is a gas, on one side labelled A, and on the other B. The are held at exactly the same temperature and pressure.

Now suppose we get rid of the partition and allow the two to mix. Thus each gas can now occupy twice its original volume. Mathematically we can calculate the expected change of entropy to be

$$\Delta S = (n_A+n_B) ln(2)$$

or something a bit like that anyway, the details of the mathematics are not particularly important I don't think.

But then suppose we had the same gas in each partition, A = B. So mathematically the entropy change would become

$$\Delta S = 2n_A ln(2)$$

However when thought about carefully, it is impossible to achieve an entropy change in this situation. Say each side were to expand into the volume of the other, and we replaced the partition, we'd have exactly the picture as we started with thus no entropy change can have occurred.

What bothers me is, if the maths is predicting something incorrectly, it suggests there is something going wrong perhaps with the details, or the definitions, or the theory. Getting around the problem by saying the particles are indistinguishable is fine, but it doesn't make the mathematical answer correct! Has this been resolved?
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 I don't know if this is answering your question, but I'll just post it. The entropy really does increase. The number of ways you can arrange the individual molecules goes up, because you have all the ways that you had with the partition, plus all the ways you can arrange it by swapping any number of molecule pairs between the two sides (while keeping the gas density equal on both sides). To make the point more clear, imagine a chamber with N molecules, but it is partitioned into N sub-chambers, each with one molecule. Then if you remove all the partitions, there is still the same density of gas overall, but now there are a huge number of ways to arrange the N molecules, where before there was only 1 way.
 Recognitions: Science Advisor There's a great explanation here: http://citeseerx.ist.psu.edu/viewdoc...=rep1&type=pdf In summary, the value of the entropy is related to the amount of information you can extract from the system.

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 Quote by johng23 The entropy really does increase. The number of ways you can arrange the individual molecules goes up...
Consensus physics disagrees. JesseC specified that there is only one gas present; therefore, the molecules are indistinguishable. One can't tell if one has swapped a pair of molecules in this case.
 Recognitions: Science Advisor Andy, I read this article some years ago while I was thinking about the entropy change when mixing substances which consist of larger molecules than O2 or N2 usually considered in text books. Specifically, I had some comment by Roald Hoffmann in mind who pointed out that in the human body there are most probably not two identical molecules of hemoglobine due to the huge amount of possibilities of the different isotopes of hydrogen, carbon, nitrogen and oxygen to distribute in the molecule. Nevertheless, hemoglobine is considered a pure substance on a macroscopical level. So, if we would start a heavy discussion and would end up on the street fighting with our knives, would the entropy of our bloods increase on mixing?
 DrDu, The article by Jaynes suggested by Andy Resnick answers all these questions. Specifically, as long as you do not "probe" properties that could differentiates between molecules, you could just as well neglect the mixing entropy, or pretend there is no mixing entropy. To push it even further, you could even have this reasoning when mixing oxygen and nitrogen. As long as you don't "identify" differences between these two gases, you can just pretend there is no mixing entropy. From Jaynes, I learned that entropy should be related to the properties we make relevant in an experiment (voluntarily or involuntarily, of course!!!!). Making relevant relates either to the preparation of the system or to its observation. For example, if oxygen and nitrogen are separated by a selective membrane, then you better think about the differences between O2 and N2. Similarly, if you can measure the O2/N2 ratio, you also better think about mixing entropy. Gravitation, centrifugal forces and other specific interactions, make it most often necessary to take O2-N2 mixing entropy into account. When we are using the words oxygen and nitrogen, by hypothesis we can assume we know these gases behave differently in various situations. Therefore, implicitely we are forced to consider mixing entropy. As long as you talk about hemoglobine, without pretending you can differentiate different kind of these molecules, then in all your analysis you can drop the mixing entropy. However, if you make distinctions between species, based on molecular weight for example, and if you are going to analyse these distinction -like by measuring concentration of species- then you could not analyse correctly what is going on without the mixing terms. This is actually rather trivial: you can forget about mixing entropy if you don't need it! From Jaynes, I really learned what I missed for many years! Entropy is not a property of system: it really is a property of what we know about a system!!! Exactly as for the quantum mechanical wave function!!! The proof of this statement is in all our experiments and analysis we make of it, as Jaynes explained with his Whifnium tale.

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