Illustrated Physics
physics, drawn
Concept

Chemical potential — where it appears

The free-energy cost of adding one more particle to a system, which fixes how particles distribute themselves between phases and reservoirs. For anything whose number is not conserved — photons in a cavity, for instance — it is exactly zero, and every unusual property of a photon gas follows from that.

Named by 21 essays across 4 fields — each of them below, with the objects they name alongside it.

The column a dissolved thing holds up. Two arms of one vessel, joined below by a membrane that passes water and not solute. On the right is 10 mol/m³ of dissolved particles at 25 °C; on the left, pure water. Water crosses into the solution until the extra weight of the right-hand column has raised its pressure by the osmotic pressure — 24.8 kPa, which is 2.53 m of water, drawn here to scale. Nothing is pulling. The solvent is at a lower chemical potential where it is mixed, so it moves that way, and it stops when mechanical pressure has made up the difference. A solute a thousand times more dilute than seawater lifts a column taller than a person.

The pressure that comes from counting

Dissolve a teaspoon of anything in a litre of water, put a membrane between it and pure water, and the solution will hold up a column of water two and a half metres tall. Nothing is pulling. The pressure does not depend on what was dissolved, only on how many particles it made — which is the ideal gas law, with the solute in place of the gas.

fluids · Osmosis Energy, pressure and entropy of a gas nobody counted. The energy density, pressure and entropy density of blackbody radiation against temperature, on logarithmic axes, together with the pressure a monatomic gas of the same energy density would have. Every curve is a power of the temperature — the fourth for energy and pressure, the third for entropy — because the only length in the problem is the thermal wavelength and the only energy is kT. The pressure is exactly a third of the energy density, where an ordinary gas's is two thirds, a factor of 2: a photon carries momentum E/c and a slow molecule carries √(2mE), and that difference is the whole of it. Some values: at room temperature the radiation pressure is 1.86e-6 pascals, which is a ten thousand millionth of an atmosphere; at 1e+7 kelvin it is 2.52e+12, which is where radiation rather than matter holds a star up.

The gas that nobody counted

A box of gas holds however many molecules were put in it. A box of radiation holds however many photons the temperature says, because the walls make and destroy them until the free energy is least — and one dropped assumption changes every result. The pressure becomes a third of the energy density instead of two thirds, the entropy goes as the cube of the temperature, and the adiabatic index comes out at exactly four thirds.

thermodynamics · Blackbody Three curves that can only meet at a point. Water's phase diagram within a kelvin of its triple point, with each boundary drawn at the slope Clausius and Clapeyron give it from measured latent heats and densities: 44.4 Pa/K for boiling, 50.3 for sublimation, and -135 bar per kelvin for melting — negative, and so steep that it is drawn vertical here, because ice is the less dense phase and pressure therefore melts it. Two things follow that no amount of measurement could adjust. The three slopes are not independent: the sublimation and vaporisation curves differ in slope by 5.92 Pa/K, which is exactly what the fusion latent heat predicts, because going solid → gas directly and solid → liquid → gas must cost the same enthalpy. And the sublimation curve is the steeper of the two, so the two cross rather than touch — which is why the triple point is a crossing and not a tangency, and why ice sublimes below it and melts above it.

Why the triple point is a point

Three phases of one substance coexist at one temperature and one pressure and nowhere else, and the reason is arithmetic rather than chemistry: count the numbers that describe the state, count the conditions equilibrium imposes, and subtract. The same subtraction says four phases of one substance are impossible, and it says so without knowing what the substance is.

thermodynamics · Phase change The pressure a charged gel develops. The swelling pressure against the gel's fixed charge density, for several salt concentrations, on logarithmic axes. Each curve has two straight parts with different slopes, and both limits are checked against the solution rather than read off the plot. Where the fixed charge is small compared with the salt the pressure goes as the square of the charge divided by four times the salt: the bath's ions screen the fixed ones, and doubling the salt halves the pressure. Where the fixed charge dominates, every counterion it demands is an extra particle in the gel and the pressure goes as the charge itself. At 15 mM salt, a gel with 200 mM of fixed charge develops 427 kPa; At 50 mM salt, a gel with 200 mM of fixed charge develops 306 kPa; At 150 mM salt, a gel with 200 mM of fixed charge develops 150 kPa; At 500 mM salt, a gel with 200 mM of fixed charge develops 49 kPa. Cartilage carries a fixed charge of a couple of hundred millimolar from the sulphated sugars on its proteoglycans, sits in a bath of about 150 mM, and develops a swelling pressure of an atmosphere and a half — which is what holds a joint apart and carries the load across it.

The swelling a membrane cannot stop

Give the thing a membrane holds back an electric charge and the small ions that can cross are no longer free to distribute themselves. Two conditions — neutrality on each side, and equal chemical potential for the salt — fix where every ion goes, and they leave the charged side with more particles than the other. That excess is what holds a joint apart, and it is why a cell has to spend a third of its energy pumping.

fluids · Osmosis The pore size the air decides. The largest pore radius that holds condensed water in equilibrium with air at a given relative humidity, for water at 25 °C, on a logarithmic radius axis. A concave meniscus lowers the vapour pressure over it by exp(−2γVₘ/rRT), so a pore whose meniscus would be tighter than a radius set by the humidity is in equilibrium only when full. The upper curve is the emptying condition, through a hemispherical meniscus with two curvatures; the lower is the filling condition, through the cylindrical film that lines a pore before it closes, with one — so the same pore fills at a higher humidity than it empties at. At 50% humidity a pore empties below 1.51 nm and fills below 0.76 nm; at 90% humidity a pore empties below 9.96 nm and fills below 4.98 nm; at 99% humidity a pore empties below 104 nm and fills below 52 nm. The radii run from molecular at low humidity to a tenth of a micrometre at 99 per cent, and every one was checked by putting it back into the vapour-pressure relation.

The pore that fills from dry air

Water condenses when the air is saturated — on a flat surface. Over a curved one the vapour pressure is different, higher over a drop and lower over a meniscus, and in a pore a few nanometres across it is low enough that the pore fills with liquid from air at half humidity. The water it holds is under a tension of a hundred megapascals, and the pore empties at a lower humidity than it filled at, for a reason that needs no roughness at all.

fluids · Capillarity A fridge with no work going into it, and its ceiling. How much heat a three-reservoir machine can lift out of a cold space per unit of heat supplied to drive it, against the temperature of the driving heat, for 3 cold temperatures and an ambient of 300 kelvin. No work enters or leaves: the machine takes heat in at the top, takes heat in at the bottom, and rejects the sum at ambient. That it can do anything at all is the surprise — the second law allows heat to be moved up a gradient provided a larger flow is moved down one, and the accounting is a single inequality in the three entropy flows. The ceiling is the product of two familiar expressions, and at 450 kelvin driving a 253-kelvin space it is 1.79. The marks are what real machines achieve, which is a fifth to a third of it — absorption refrigeration is not efficient and is chosen when the heat is free and the silence and the absence of moving parts are worth something.

A fridge with no work going into it

Every engine here so far turns heat into work or work into a heat flow. A machine exchanging heat with three reservoirs and doing no work at all can still move heat from cold to hot, and the ceiling on how much is the product of two Carnot expressions — an engine's efficiency times a fridge's coefficient of performance. A gas flame makes ice, and the accounting is one inequality in three entropy flows.

thermodynamics · Heat engines Every reaction's free energy has its lowest point inside. An ideal reaction A ⇌ B at 298 K. Across: how far it has gone, from pure A towards pure B. Up: the Gibbs energy of the mixture per mole, relative to pure A. Left, for standard reaction Gibbs energies ΔG° of −4, 0, +4 kJ/mol: the dashed straight lines are what the energy would be if A and B did not mix, and the solid curves add the entropy of mixing them. For ΔG° = −4 kJ/mol the lowest point is at 83.4 per cent B; for ΔG° = 0 kJ/mol the lowest point is at 50.0 per cent B; for ΔG° = +4 kJ/mol the lowest point is at 16.6 per cent B. Right, magnified near pure A, a reaction with ΔG° = +10 kJ/mol, whose straight line climbs from the start and which looks as if it should not proceed at all: its curve first falls, to a minimum of −43 J/mol at 1.74 per cent B, because the mixing term falls infinitely steeply away from a pure end. Each minimum was found by search and sits where the ratio of B to A equals exp(−ΔG°/RT).

The reaction that cannot go all the way

Chemistry speaks of reactions that go to completion and reactions that do not happen, and at equilibrium there are neither. The reason is a logarithm. The free energy of a half-finished reaction contains the entropy of mixing, whose slope is infinite at both pure ends, so every reaction's lowest point lies strictly inside — and the slope of that free energy, the chemical potential, is to particles what temperature is to heat.

thermodynamics · Chemical potential The light of a diode at room temperature is as bright as a surface thousands of kelvin hot. How many photons occupy each mode of the light, on a logarithmic scale, against photon energy. The lowest curve is the thermal glow of a 1.42 eV semiconductor at 300 K with no voltage across it. The solid curve above it is the same device with 1.3 V across it, emitting only above its gap. The dashed curve is a blackbody at 2571 K, the temperature whose light has the same occupation as the diode's at 1.472 eV, just above the gap. They cross there and nowhere else: the diode's occupation falls a factor e every 25.9 meV, as its lattice's temperature requires, and the blackbody's every 222 meV. No single temperature describes the diode's light. At each photon energy it has a brightness temperature, and that temperature is 300 K multiplied by ε/(ε − qV).

The glow that carries a voltage

Thermal radiation has no chemical potential, because walls make and destroy photons freely. A light-emitting diode is a body that glows at room temperature with a voltage written into its light — Planck's law with the voltage as the photons' chemical potential — which is why its light can be as bright as a surface thousands of kelvin hot, why at low voltage it can put out more light than the power it draws and cool itself doing so, and why a reverse voltage makes a surface look colder than it is.

thermodynamics · Chemical potential How full a surface is, against the pressure of the gas above it. The fraction of adsorption sites occupied on a surface that binds a molecule with 0.35 eV, against the gas pressure on a logarithmic axis, at 250, 300, 350 K. Each curve is θ = p/(p + p½) — Langmuir's isotherm — and each is the same S-shape moved along the axis: on a logarithmic pressure scale the coverage is a function of ln p alone, shifted by the binding energy over kT. The half-full pressure is 5.58 Pa at 250 K, 132 Pa at 300 K, 1341 Pa at 350 K. Warming the surface does not change the shape; it slides the curve to higher pressure by a factor that is a Boltzmann factor, e^(ε/kT), which is how a binding energy is read off a family of isotherms.

The site that fills like an electron level

A patch of catalyst holding a gas molecule, a haem in a muscle cell holding oxygen, an energy level in a metal holding an electron: each is a place that can hold one particle or none, in contact with a reservoir it trades particles with. Each fills according to the same function of one variable — how far the reservoir's chemical potential lies above the energy of the site. Langmuir's isotherm and the Fermi function are not analogous. They are the same law, and haemoglobin works because its sites break it.

thermodynamics · Chemical potential Electrons and holes in silicon against the donors added. The concentrations of free electrons and holes in silicon at 300 K against the concentration of donor atoms added, on logarithmic axes, solved from charge neutrality and the product law n·p = nᵢ². Below the intrinsic concentration of 10¹⁰ per cubic centimetre the donors change almost nothing. Above it the electrons follow the donors one for one and the holes fall in exact proportion: a hundred times more donors, a hundred times fewer holes. At 10¹⁶ donors the electrons outnumber the holes by 10¹² to one. The dashed line is √(n·p), which does not move at all across ten decades of doping — checked to a part in a billion.

The product doping cannot move

Add one phosphorus atom for every five million silicon atoms and the crystal's free electrons multiply a millionfold — and its holes fall a millionfold, although nothing was done to them. Add a drop of acid to water and the hydroxide ions vanish in exactly the proportion the hydrogen ions grow. Both are one law: when a reaction makes two species together, equilibrium fixes the sum of their chemical potentials, and so the product of their concentrations. Every semiconductor device is built on the minority carriers that law leaves behind.

thermodynamics · Chemical potential Fifty-nine millivolts for every factor of ten. The voltage that holds a singly charged ion at one concentration on one side of a boundary and another concentration on the other, in equilibrium, against the ratio of the concentrations on a logarithmic axis: (kT/e) ln(c₁/c₂), from requiring the electrochemical potential to be the same on both sides. At 0 °C, 54.20 mV per decade; at 25 °C, 59.16 mV per decade; at 37 °C, 61.54 mV per decade; at 100 °C, 74.04 mV per decade. The voltage depends on the ratio and the temperature and on nothing about the ion, the solvent or the boundary: it is the entropy of dilution, expressed per unit charge.

The voltage that is a chemical potential

A battery, a nerve cell and a pH meter all turn a difference in chemical potential into a voltage, and the conversion is the same in each: fifty-nine millivolts for every factor of ten in concentration, at room temperature, whatever the ion. The voltage a battery holds as it discharges is the chemical potential of the atoms stored in its electrodes — and a battery whose voltage barely changes is one whose electrode is going through a phase transition.

thermodynamics · Chemical potential The stiffness that falls below four-thirds. The first adiabatic exponent Γ₁ — how steeply pressure rises when a gas is squeezed without heat escaping — of hot oxygen with its radiation and its equilibrium electron–positron pairs, against temperature, at densities of 10³, 10⁴, 10⁵, 10⁶ g/cm³. At 10³ g/cm³ its least value is 1.222, near 1.2 billion kelvin; at 10⁴ g/cm³ its least value is 1.235, near 1.3 billion kelvin; at 10⁵ g/cm³ its least value is 1.285, near 1.8 billion kelvin; at 10⁶ g/cm³ its least value is 1.339, near 3.1 billion kelvin. A star can hold itself up only if its core's Γ₁ averages above 4/3, the value for a gas of light alone; a core that dips below it has no stable size, and the pair production that pulls it below is strongest where the gas is hot and thin — the cores of the most massive stars.

The heat that turns into matter

Thermodynamics counts particles and relativity lets them be made. Heat a gas to a billion kelvin and its light carries enough energy to create electrons and positrons, which the gas then holds in equilibrium like any other ingredient. The heat spent making them raises neither the temperature nor the pressure, so the gas grows soft — softer, in the cores of the most massive stars, than a star can survive. Those stars collapse, ignite their oxygen all at once and blow themselves entirely apart; and the same pairs, vanishing a few seconds after the Big Bang, left the universe's light hotter than its neutrinos by a factor that is the cube root of eleven over four.

relativity · Relativistic thermodynamics Hydrogen comes apart far below its binding temperature. The fraction of hydrogen that is ionised in equilibrium, against temperature on a logarithmic axis, for densities of hydrogen nuclei of 10²³, 10¹⁸, 10¹², 10⁶ per cubic metre, from Saha's equation. Hydrogen's binding energy, 13.6 eV, corresponds to 157,803 K. It is half ionised at 13,980 K at 10²³ per cubic metre, 7,235 K at 10¹⁸ per cubic metre, 4,519 K at 10¹² per cubic metre, 3,270 K at 10⁶ per cubic metre — at a temperature where kT is between an eleventh and a fiftieth of the energy needed to free the electron. The thinner the gas, the cooler the temperature at which it comes apart, because a free electron in a thin gas has vastly more room to be in than a bound one.

The electron that leaves because there is room

It takes 13.6 electronvolts to pull the electron off a hydrogen atom, the energy of a particle at a temperature of 158,000 kelvin. Hydrogen is half ionised at the surface of a star at 14,000 kelvin, in a thin nebula at 7,000, and in the early universe at under 4,000 — a fortieth of its binding energy. The electron leaves not because it has enough energy but because a free electron has so much more room to be in than a bound one, and at equilibrium room counts as much as energy. Saha's equation is that trade written down, and it turned out to be the key to what stars are made of.

thermodynamics · Chemical potential Hydrogen ionised by heat at one end and by crowding at the other. The ionised fraction of hydrogen against the density of nuclei, at 5,000 K, 10,000 K, 20,000 K, from Saha's equation with the binding energy lowered by the neighbouring charges (solid) and without the lowering (dashed). Thin gas is ionised by the room a free electron gains; compression takes the room away and the gas recombines, as the dashed curves continue to do for ever. The solid curves turn round: at 5,000 K the gas is least ionised, 2.5·10⁻⁴ per cent, near 10²⁶ per cubic metre; at 10,000 K the gas is least ionised, 0.41 per cent, near 10²⁷ per cubic metre; at 20,000 K the gas is least ionised, 12 per cent, near 10²⁸ per cubic metre, and by 6·10²⁸ per cubic metre — 0.10 g/cm³ — every curve is fully ionised, because the ground state no longer exists. That density does not depend on the temperature at all.

The pressure that ionises

Squeeze a hot gas of hydrogen and Saha's equation says it recombines: a free electron has less room to be in, and room was what paid for its freedom. Squeeze it far enough and it comes apart again, completely, at any temperature — not because the room has grown but because the atom has nowhere left to be. Crowded to within a few atomic radii of each other, hydrogen atoms have no bound state, and their electrons, freed by pressure alone, form a metal. Deep inside Jupiter most of the planet's hydrogen is in that state.

thermodynamics · Chemical potential The proton fraction a cold star settles at. The fraction of nucleons that are protons in cold matter in beta equilibrium, where the neutron's chemical potential equals the proton's plus the electron's, against density on logarithmic axes, for free neutrons, protons and electrons with no nuclear forces. Below 1.22·10⁷ g/cm³ the electrons cannot pay the 1.29 MeV difference between a neutron and a proton and the matter is all protons. Above it the fraction collapses, to 0.014 per cent at its lowest near 7.9·10¹¹ g/cm³, and at nuclear density, 2.66·10¹⁴ g/cm³, it is 0.49 per cent. At higher densities it climbs slowly towards one ninth, 11 per cent, which it never reaches. The dashed part lies where real matter is made of nuclei rather than free nucleons.

The protons a star cannot afford

A free neutron decays in fifteen minutes into a proton, an electron and an antineutrino. Inside a neutron star it cannot, and the star is made of neutrons because of it. Beta decay is a reaction like any other, and at equilibrium the neutron's chemical potential must equal the proton's plus the electron's. In a crowded star an electron can only be added at the top of a sea tens of megaelectronvolts deep. So the matter settles where protons are rare: half a per cent of the nucleons at nuclear density, if nucleons were free, and never more than one in nine at any density.

thermodynamics · Chemical potential How a solute moves both ends of the liquid range. The molar chemical potential of water against temperature near its freezing point (left) and its boiling point (right): liquid (blue), ice (green), vapour (red), each a line whose slope is minus its entropy, drawn relative to the liquid at the transition. A solute at mole fraction 0.05 — about 2.9 mol/kg — lowers the liquid's line by RTx (dashed) and leaves the ice and the vapour unchanged. The crossings move: the freezing point down by RTx divided by the entropy of melting, 5.16 K, the boiling point up by RTx divided by the entropy of boiling, 1.42 K. The same vertical shift moves the freezing crossing 3.6 times as far, because ice's line is nearly parallel to the liquid's — melting changes the entropy by 22.0 J/mol K — while the vapour's line crosses steeply, with 109 J/mol K between them. Lowering the liquid makes it the winner over a wider range of temperature at both ends: the solution is liquid from below 0 °C to above 100 °C.

The degree a spoonful of solute buys

Dissolve anything in water and the water freezes lower and boils higher. The two shifts come from one cause — the solute lowers the liquid water's chemical potential, so the liquid wins against ice and against vapour over a wider range — but they are not the same size. For every mole of particles per kilogram the freezing point falls 1.86 degrees and the boiling point rises only 0.51, three and a half times less, and the reason is in the entropies: ice and water are so alike that a small push moves their crossing a long way. The same arithmetic says salting pasta water does nothing a cook could notice, weighed molecules for a century of chemistry, and in 1887 showed that salts in water are made of ions.

thermodynamics · Chemical potential How supersaturated a cloud is, to an ice crystal. The supersaturation over ice of air that is just saturated over liquid water, eᵥᵥ/eᵢ − 1, in per cent, against temperature; dashed, the same computed from the chemical potentials, exp(LΔT/RT·Tₘ) − 1, with L the latent heat of melting per mole, ΔT the supercooling and Tₘ the melting point. A supercooled cloud is in balance with its droplets, so to any ice crystal inside it the air is 5.1 per cent supersaturated at −5 °C, 10.5 at −10, 22.0 at −20 and 41.2 at −35. Over the droplets themselves it is exactly saturated, so they neither grow nor shrink by vapour. The excess is the chemical-potential difference between supercooled water and ice, 217 J per mole at −10 °C, expressed as a pressure ratio.

The ice that grows by stealing from the droplets

Most clouds colder than freezing are not made of ice. They are made of droplets of liquid water, some tens of degrees below their freezing point, waiting for something to start them freezing. When a few ice crystals do appear among them, the crystals grow and the droplets shrink, without touching, because supercooled water has a higher chemical potential than ice and so a higher vapour pressure: air balanced with the droplets is ten per cent supersaturated, to an ice crystal, at minus ten degrees. A few crystals among a hundred thousand droplets each take everything, grow heavy enough to fall, and that is how most of the rain outside the tropics begins — as snow.

thermodynamics · Chemical potential Why silt heaves and sand and clay do not. The relative rate at which water is drawn to a growing ice lens, against grain diameter on a logarithmic scale, for three loads on the soil above it, in a capillary model: the rate is the soil's permeability, which grows as the grain diameter squared, times the suction the lens can sustain less the load. The suction is capped both by the supercooling at the lens, here 2 K, and by the Gibbs–Thomson pressure at which ice would break into the pores. Coarse soil has open pores that ice simply invades, so the suction never exceeds the load: under 10 kPa, half a metre of soil, nothing heaves above 58 μm. Fine clay can sustain the full suction but passes water too slowly to feed it. Between lies a fastest grain size, 29 μm under 10 kPa, 10 μm under 30 kPa and 2.9 μm under 100 kPa: silt, the soil engineers have long called frost-susceptible. Real heave pressures exceed this model's, and the fit is to the shape, not the scale.

The frost that lifts by drinking

Frozen ground rises in winter, sometimes by tens of centimetres, and the usual explanation — water expands by nine per cent when it freezes — is wrong: soil soaked in benzene, which shrinks as it freezes, heaves too. The lift comes from layers of clear ice that grow by pulling liquid water up through the soil from below. Ice and water touching each other need not be at the same pressure, and when the water is free to flow, ice a degree below its melting point can push with 1.12 megapascals while it drinks — twelve times less than freezing water in a sealed pipe, and enough to lift a house at a tenth of a degree.

thermodynamics · Chemical potential Latent heat of boiling against boiling point. The heat needed to boil one mole of a liquid at its normal boiling point, against that boiling point, both on logarithmic axes, for twenty-one substances from helium to sodium. The line is ΔH = 87.2 J/(mol K) × Tb, the mean entropy of boiling of the ordinary liquids boiling between 250 and 700 K, which scatter about it by 3.3 per cent; the ordinary liquids as a whole (blue), from neon at 27 K to sodium at 1,156 K, by 10.0 per cent, the coldest lying low. Water, ammonia and the alcohols (red) need more heat than the line predicts, acetic acid (green) less; the quantum liquids helium and hydrogen (violet) fall far below.

The entropy every liquid gains on boiling

Divide the heat it takes to boil a liquid by the temperature at which it boils, and for benzene, chloroform, acetone, hexane, ether and carbon tetrachloride the answer comes out within a few per cent of the same number — about ten and a half times the gas constant. Frederick Trouton noticed it in 1884. It is a statement about entropy, and once it is read that way the liquids it fails for become the interesting ones: water and the alcohols, whose hydrogen bonds hold the liquid in order; acetic acid, whose vapour is made of pairs; and helium, whose liquid is already as disordered as quantum mechanics allows.

thermodynamics · Phase change The peak that rises out of a cloud. A slice through the shadow a released cloud of a million atoms casts after it has expanded, the measurement by which condensates are seen, at 1.1, 0.8 and 0.5 times the transition temperature: the thermal atoms, whose spread of speeds sets the cloud's width, give a broad rounded profile; the condensed atoms, all in one state with only the small spread of momenta their trap allowed, give a narrow peak at the centre, drawn here with the shape repulsion between the atoms gives it. Above Tc there is only the broad cloud. At 0.8 Tc a sharp peak stands up from its middle, holding 47 per cent of the atoms; at 0.5 Tc the peak holds 87 per cent and the thermal wings have shrunk. The two-component shape — a narrow peak on a broad base — was the signature that announced the first gaseous condensates in 1995.

The condensate a trap makes

A gas of atoms held in a magnetic trap and cooled to a few hundred billionths of a degree does something no gas in a box does at any temperature it can reach: a large share of its atoms falls into the trap's single lowest state, and a sharp peak rises out of the cloud. The reason is counting. The trap's excited states can hold only so many atoms at a given temperature, and the number grows as the cube of the temperature — so below one temperature the atoms run out of room, and every atom that does not fit has only one place to go.

quantum · Superfluidity Salt that takes in water from the air at three-quarters humidity. The water held by a crystal of common salt, in grams per gram of salt, against the relative humidity of the air around it at 25 °C, with the humidity rising (solid) and falling (dashed). Rising, the crystal stays dry until 75.2 per cent and then dissolves at once into a drop holding 2.79 g of water per gram — the saturated solution — which goes on drinking as the air gets damper: 4.24 g at 85 per cent, 11.5 g at 95. Falling, the drop does not crystallise at 75 per cent. It sheds water along the same curve, becomes supersaturated, and stays liquid down to about 45 per cent before a crystal finally nucleates and it dries out at once.

The salt that dissolves in the air's own water

Leave a dish of salt in a bathroom and it does not just clump; on a humid enough day it turns into a puddle, though no water was poured on it. Above 75 per cent humidity, common salt pulls water out of the air until it has dissolved itself. The number is not a property of salt's attraction for water in any vague sense. It is the vapour pressure of a saturated salt solution, read as a fraction of pure water's: wherever the air holds more water than that, the solution is the state with the lower chemical potential. Bring the humidity back down, and the puddle does not turn back into salt until the air is far drier — about 45 per cent.

thermodynamics · Chemical potential

Named alongside it

The objects these essays reach for when they reach for this one.

EntropyEquilibriumLatent heatThe Boltzmann factorClausius clapeyronVapour pressureAdiabatic indexBand gapBlackbodyChemical equilibriumDegenerate matterDetailed balance

All concepts