By Marcel van der Veer
18-11-2017

Published in category Science

More on Chemistry, Physics, Thermodynamics

Recently I met during an event at my Alma Mater, the University of Nijmegen, my high school physics teacher. We discussed the chemistry curriculum, and remarked that quite some chemistry students capture with difficulty the fundamental principles from thermodynamics. Needless to say that thermodynamics is one of those subjects that serve a chemist for a lifetime. In my humble opinion, one reason for this lack of retention may be the abstraction level in freshmen courses, and that this might be improved by spending one or two introductory hours on the basic ideas of thermodynamics in a historic context.

Would such approach work? All I can do is present a first attempt here. I realise that I take the risk that my attempt might demonstrate that I would not have fully retained the matter either.

Context

Thermodynamics is the science of the conversion of energy. It is a discipline where fundamental science and applied engineering go hand in hand. This field made important progress in the time of the industrial revolution and the Napoleonic wars. Mozart and Beethoven composed their beautiful works. The steam engine had arrived, and constructing optimally efficient machinery posed a powerful economic and military incentive - two common drivers for innovation and scientific progress.

Considering its roots in engineering practice, it is understandable that classical thermodynamics applies to large scale devices - to bulk matter at large time scales - and is not concerned with the microscopic structure of matter. Instead this classical theory is expressed in abstract notions as "free energy" or "entropy". The turn of the 18th-19th century was the era when ideas about the microscopic structure of matter were only emerging. Ancient philosophers had proposed "atoms" as building blocks for matter, but the idea only became actual when Dalton had found that chemical elements react in fixed multiples of mass. Do not expect classical thermodynamics to for instance explain where entropy resides in a polymeric solution - in this theory entropy has no physical meaning and molecules just are not a part of its concepts.

Today however, students are taught in high school that matter consists of molecules built from atoms that are miniature solar systems (elementary quantum mechanics only comes later in the high school curriculum). Our chemistry students are used since a young age to explain the natural world in terms of atoms and molecules and are confronted with a theory that does not give mechanistic explanations based on small scale structure. That requires a mental paradigm shift - and here may be the difficulty.

You might wonder why Newton's classical mechanics and his theory of gravity seems to be more easily "captured" by students. This may be psychological - people take for granted that what is part of their day to day experience. Gravity explains the common experience that things fall to the ground, the position of the Moon thereby enabling calculation of timetables for the tides of the seas, et cetera. The difference with classical thermodynamics is that for instance entropy has no physical meaning, while gravity and the motion of celestial bodies are "tangible".

Interestingly a "tangible" concept as gravity is taken for granted while only few ask about its nature - what causes gravity? Gravity was not understood until Einstein explained gravity as mass making a dent in the universe, or more precisely, a "pit" in space-time by which one mass traps another.

Modern physics still struggles with the link between macroscopic gravity and the quantum-world. It is the missing link before finding the holy grail of physics - a single theory that would explain the relation between the four fundamental forces: gravity, electromagnetism and the weak and strong nuclear force. This would be a "theory of everything".

Today we can link thermodynamic quantities to the behaviour of atoms and molecules. That field is called statistical mechanics or statistical thermodynamics which is a beautiful field built on classical thermodynamics and atomic theory. It involves the work of brilliant minds such as Liouville, Boltzmann and Gibbs, that also makes abstract terms as entropy more insightful. Statistical mechanics is the theory behind techniques as molecular dynamics simulations that are run on modern supercomputers. However here we will limit ourselves to classical thermodynamics.

Energy - work and heat

Energy is an abstract quantity that comes in two forms: work which is useful "directed" energy that can exert force and thereby displace weight, and heat that is "undirected" energy that does no work. Before the industrial revolution, there was already consensus on the conservation of energy in an isolated system, from the emperical fact that no-one could demonstrate perpetual motion. The insight that conservation of energy is an essential consequence of the time-invariance of physical laws, only came much later at the beginning of the 20th century with the Noether theorema.

The sum of work and heat needed to create a system is called that system's internal energy. Its symbol is U and we do not know why - maybe because U is a linguistic variant of V while in earlier days potential energy was called Voltage, but really, we do not know. When you progress in the study of thermodynamics you will learn that under circumstances you will want to add to U the work needed to make the system attain its volume and pressure. You can appreciate this when you think of pressure being force per unit surface, or equivalently, energy per unit volume: pressure is an energy-density. With pressure-volume work added, internal energy becomes enthalpy with symbol H, most likely for "Heat".

Pushing the steam engine to its limit

Before the industrial revolution, England suffered from an energy crisis. Building and maintaining the navy and the use of wood as fuel, resulted in deforestation and thus wood getting scarce. Coal was an alternative fuel, but production could not meet demand since many mines were flooded. As always, necessity is the mother of invention. Clever people like Newcomen managed to make coal-fueled steam-operated pumps that could drain a mine. Since these pumps operated in a coal mine, fuel efficiency was not a first priority.

Many believe that James Watt invented the steam engine, but actually he improved steam-pumps like the Newcomen engine. Watt realised that instead of cooling large parts of such engine, one should install a condensor for steam, thereby increasing efficiency, while keeping a versatile and easy-to-maintain design. Better efficiency meant that steam engines could be operated away from a coal mine. Watt invented an accompanying rotary engine that mechanised weaving, spinning and transport. So it is fair to say that Watt's mind made the industrial revolution possible.

An important issue was the economy of mechanisation - for instance, what would be the best efficiency a steam engine could achieve? Watt coined the term "horsepower" and knew there was a limit to the efficiency of the steam engine, meaning that not all heat could be converted into work, but he did not solve this question. For that, we need to go to England's opponent at the time, France.

In France, young army officer Sadi Carnot worked to give his country a military advantage by designing steam engines with maximum efficiency. Whatever he tried, he found that efficiency only increases with increasing temperature difference between boiler and condensor, relative to the temperature of the boiler.

Carnot devised an ingeneous reductio ad absurdum showing that if a perfect heat engine more efficient that this limit would exist, then a heat engine tandem could be made that would do work by only taking heat from a reservoir. Such miracle was never seen so thought impossible - you cannot propel a ship only by cooling the water it floats on. In this way Carnot's work made clear an important asymmetry in nature: work can be completely degraded to heat, but heat cannot be completely converted into work. Not all energy in a system is available to do work. It takes some work to convert "undirected" into "directed" energy.

Efficiency of processes in general

If not all energy in a system is available to do useful work to let the industry hum, then what part of energy is? That amount is "free energy", which is the maximum work you can get out of a process when you avoid leaks and friction and what have you. Note that in the anglosaxon world the symbol for free energy is simply F though in German speaking countries the symbol is A for "Arbeit". As for internal energy, under circumstances you must also include the work needed to give the system its volume and pressure. Then free energy becomes free enthalpy, with symbol G for Gibbs.

The part of energy not available to do useful work is related to a quantity called "entropy" from the Greek term for "in transition" or if you want "in degradation". Entropy is an abstract notion; it is not possible to assign a physical meaning to it like we can with internal energy. An amount of energy equal to temperature times entropy cannot be converted into useful work - it is hiding in whatever functions as Watt's and Carnot's "condensor" in the process you are considering. The symbol for entropy is S and this is thought to be a tribute to Sadi Carnot.

In the mid 19th century work was collected into two basic governing rules. Carnot's work was generalised to other processes. Important scientists as Clausius, Kelvin and Thomson declared conservation of energy as the First Law and different variants of Carnot's and later insights as the Second Law. The First Law says that energy cannot be created nor destroyed. The Second Law says that entropy can be created, but not destroyed.

Spontaneous change - the fate of the universe

Entropy can decrease locally only when at least an equal amount is generated elsewhere in the system. Think for example of your refrigerator. The compressor does work and generates entropy compensating for entropy loss due to making heat flow from a cool to a warmer place, which is an forced process since heat wants to flow from a warm to a cool place.

Free energy is important in designing efficient engines, but is also important in chemistry and physics. Through free energy, thermodynamics explains in what direction spontaneous processes will move. In a closed system at constant entropy and volume which is connected to other systems but unable to exchange matter, the internal energy will decrease and be at minimum value at equilibrium. An isolated system that is not connected to other systems, having fixed internal energy and mass, will attain maximum entropy at equilibrium. In both cases, free energy will decrease, searching so to speak for lowest points in the valleys in a mountainous landscape. Nota bene that free energy can attain a local minimum, and may not arrive at a global minimum!

The universe is an isolated system with ever-increasing entropy moving towards thermal equilibrium at uniform temperature, a so-called "heat death". This is the only principle in physics that gives a direction to time so you remember the past but not the future. Contemplate this. Since Bekenstein and Hawking we know that even the darkest of places in the universe, a black hole, has entropy with corresponding temperature, meaning that it emits thermal radiation and is not completely black.

Concluding remarks

Having read until here, you may want to impress your friends with your insights. You should now be able to understand the following. On a microscopic scale, looking at a gas or fluid and seeing all individual particles, you can appreciate the work involved to introduce or extract just one atom or molecule. Now you know this work equals free energy, in this case the Gibbs free enthalpy per particle, a quantity known among chemists as the "chemical potential". In a metal, electrons fill energy bands and the work needed to shoot an electron at the top of the bands out of the metal is called the Fermi level of that metal. Explain this as the Fermi level being the chemical potential of an electron, and your peers are likely to slip from their chairs.



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