By ucapjo0, on 9 February 2015
You’re probably familiar with the second law of thermodynamics in one of its many forms:
Anything that can possibly go wrong, does.
— Murphy’s law
“Happy families are all alike; every unhappy family is unhappy in its own way.”
— Leo Tolstoy in Anna Karenina, almost 20 years before Boltzmann’s Kinetic Theory of Gases
— ancient proverb
Because every day we feel the consequences of the second law. Even Homer Simpson has been known to admonish his children: “In this house, we obey the laws of thermodamynics!” Not that Bart or Lisa would have much choice. The second law of thermodynamics governs much of the world around us – it tells us that a hot cup of tea in a cold room will not spontaneously heat up; it tells us that unless we are vigilant, our homes will become untidy rather than tidy; it tells us how efficient the best engines can be and even helps us distinguish the direction of time – we see vases shatter, but unless we watch movies backwards, never see the time-reverse – a shattered vase reforming with just a nudge.
The second law tells us that order tends towards disorder, something we are all very familiar with — trying to achieve a very specific state of affairs can be very difficult, because there are many different ways things can go wrong. Murphy’s Law (anything that can go wrong, will go wrong), is a reasonable statement of the second law of thermodynamics. As is its less precise version “Shit happens”.
More concretely, the second law tells us that for isolated systems, the entropy, a measure of disorder, can only increase. I like to think of the second law as constraining what can happen to a system — left on its own, things don’t get more ordered.
But the laws of thermodynamics only apply to large classical objects, when many particles are involved. What do the laws of thermodynamics look like for microscopic systems composed of just a few atoms? That laws of thermodynamics might exist at the level of individual atoms was once thought to be an oxymoron, since the laws were derived on the assumption that systems are composed of many atoms.
Are there even laws of thermodynamics at such a small scale?
The question is becoming increasingly important, as we probe the laws of physics at smaller and smaller scales.
Statistical laws apply when we consider large numbers. For example, imagine we toss a coin thousands of times. In this case, we expect to see roughly equal numbers of heads as tails, while the chance that we find all the coins landing heads is vanishingly small. If we imagine tossing a larger and larger number of coins, the chance of having an anomalous coin tossing such as all tails goes to zero and our confidence that we’ll have roughly half heads, half tails, increases until we are virtually certain of it.
However, this is not true when tossing the coin just a few times. There’s a reasonable chance we will find all the coins landing tails. So, can we say anything reasonable in such a case? Similar phenomena occur when considering systems made out of very few particles, instead of very many particles. Can we make reasonable thermodynamical predictions, about systems which are only made up of a few particles.
Surprisingly, the answer is yes, and the mathematical tools from a field known as quantum information theory help us to understand the case when we don’t have a large number of particles. What we find, is that not only does the second law of thermodynamics hold for quantum systems, and those at the nano-scale, but there are even additional second laws of thermodynamics. In fact, there is an entire family of second laws. So, while Murphy’s law is still true at the quantum scale — things will still go wrong; the ways in which things go wrong is further constrained by additional second laws. Because remember, the second law is a constraint, telling us that a system can’t get more ordered. These additional second laws, can be thought of as saying that there are many different kinds of disorder at small scales, and they all tend to increase as time goes on. What we find is a family of other measures of disorder, all different to the standard entropy, and they must all increase.
This means that fundamentally, there are many second laws, all of which tell us that things become more disordered, but each one constrains the way in which things become more disordered. Why then does there only appear to be one second law for large classical systems? That’s because all the second laws, although different at microscope scales, become similar at larger scales. At the scale of the ordinary objects we are used to, all the quantum second laws are equal to the one we know and love.
What’s more, it can sometimes happen that the traditional second law can appear to get violated – quantum system can spontaneously become more ordered, while interacting with another system which barely seems to change. That means some rooms in the quantum house may spontaneously become much tidier, while others only become imperceptibly messier.
What do these additional second laws look like? Well, first let’s get a bit more technically dirty. If you already know your thermodynamics fairly well, this is a good point to join us. For those who’ve had enough, here is a picture of Watt’s steam engine. It’s big enough that none of these additional second laws matter.
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The first thing we want to do, is formulate the ordinary second law slightly differently. Because actually, the formulation — that entropy increases for isolated systems, is not always the most useful one. The formulation which tends to be a bit more useful is that for an isolated system or one which is allowed to interact with a heat bath at temperature T, the free energy F=E-TS can only go down. Here E is the total energy of the system, and S is its entropy. The free energy can be thought of as the energy which is available to perform work (since some of the energy will be dissipated as heat). Now imagine we have a system, and consider two possible states of that system (for example if our system is a vase, we could consider two states of the vase, one in which it is unbroken, and the other when it’s shattered). If we want to know whether one state can evolve into another, we just need to check whether the free energy of the first state is higher than the free energy of the second. If so, the initial state (the unbroken vase) can evolve into the target state (the shattered vase). In fact, for macroscopic systems with short interactions, an initial state can evolve into a target state, if and only if the free energy goes down in the process.
So what are the additional second laws for small systems? They just correspond to additional free energies. For those that want to know their exact form, they’re given by:
where Z is the partition function, k is Boltzmann’s constant, p is the probability distribution of the state of interest, and q is the distribution of the thermal state of the system. α runs from 0 to ∞. For α=1, this quantity is just equal to the ordinary free energy, so one of these second laws correspond to the ordinary one. For α=0, the quantity is just equal to the amount of work which can be distilled from the system, while for α→∞ we get the work required to create the system from the thermal state. And as we increase the size of the system, it turns out that all these free energies become approximately equal to the standard one F. Thus for larger, more complicated systems, the many second laws of thermodynamics becomes just one. Things are so much simpler when they’re much more complicated!
If you find any of this interesting, then you might want to give the paper itself a try — we’ve tried to write it in a way which is reasonably accessible. In it, we also discuss how to reformulate the laws of thermodynamics in what is called a resource theoretic framework. We also prove something which we call the zeroth law of quantum thermodynamics, which helps define the notion of temperature. We focus our discussion on second laws for cyclic processes, which is how Clausius originally formulated the second law. Of course no physical process is perfectly cyclic, so we need to consider approximately cyclic processes. However, it turns out that there are different families of second laws depending on how cyclic our processes are. But what do we mean by approximately cyclic? You might think that it’s safe to demand that the process is close to perfectly cyclic, to within some amount ε. But no matter how small you make ε, strange things can happen, and one can violate the ordinary second law. It’s a bit like being able to embezzle. Except instead of embezzling money from a bank, we embezzle work from a single heat bath (something forbidden by the second law). The field of quantum thermodynamics seems to contain some strange phenomena, and trying to understand them better is becoming an exciting ride.
- Jonathan Oppenheim is Professor of Quantum Theory at UCL. He is co-author of a new paper on the quantum second laws of thermodynamics – with Fernando Brandao, Michal Horodecki, Nelly Huei Ying Ng and Stephanie Wehner – which is published this week in the Proceedings of the National Academy of Sciences.