Generator

Molecular speeds at 4 temperatures

One function in the thermal library, called 26 times across 5 essays. Below: what it draws at its defaults, what it draws at every branch an essay asks for, whether the site's own gate puts a claim to it, and everywhere it is called.

At its defaults it draws molecular speeds at 4 temperatures. The distribution of molecular speeds in a gas, with each curve enclosing the same area. Raising the temperature moves the peak right and lowers it: the same molecules, spread over a wider range of speeds.

speed-distribution is one function in lib/figures/thermal.js — cycles, distributions and the statistics underneath them. Everything below came out of it during this build, at parameters taken from the essays rather than invented for this page. A figure here is the figure a reader meets in an essay, and if the generator changes, this page changes with it.

At its defaults

Drawn even though every essay passes options, because a default nothing exercises is a trap for the next essay to call this with none — which has happened here twice.

Molecular speeds at 4 temperatures. The distribution of molecular speeds in a gas, with each curve enclosing the same area. Raising the temperature moves the peak right and lowers it: the same molecules, spread over a wider range of speeds.

The distribution of molecular speeds in a gas, with each curve enclosing the same area. Raising the temperature moves the peak right and lowers it: the same molecules, spread over a wider range of speeds.

Pressure, counted as momentum arriving at a wall

The options are the ones Pressure is a rate of arrival, and the gas law falls out of counting passes. A branch drawn at its own defaults instead would be a picture no essay asked for and no assertion has been run against.

Pressure, counted as momentum arriving at a wall. Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Pressure, counted as momentum arriving at a wall

The options are the ones Pressure is a rate of arrival, and the gas law falls out of counting passes. A branch drawn at its own defaults instead would be a picture no essay asked for and no assertion has been run against.

Pressure, counted as momentum arriving at a wall. Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Pressure, counted as momentum arriving at a wall

The options are the ones Pressure is a rate of arrival, and the gas law falls out of counting passes. A branch drawn at its own defaults instead would be a picture no essay asked for and no assertion has been run against.

Pressure, counted as momentum arriving at a wall. Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Pressure, counted as momentum arriving at a wall

The options are the ones Pressure is a rate of arrival, and the gas law falls out of counting passes. A branch drawn at its own defaults instead would be a picture no essay asked for and no assertion has been run against.

Pressure, counted as momentum arriving at a wall. Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

Molecules with speeds drawn from the Maxwell–Boltzmann distribution and directions drawn uniformly in the plane of the figure. Those moving toward the wall will bounce off it, reversing the component perpendicular to it and delivering twice that momentum each — and pressure is nothing but the rate at which that momentum arrives. Because the directions here lie in a plane rather than in space, the perpendicular component carries half the energy rather than the third it carries in a real gas.

The gas that leaves is not the gas inside

The options are the ones The gas that leaves is not the gas inside passes. A branch drawn at its own defaults instead would be a picture no essay asked for and no assertion has been run against.

The gas that leaves is not the gas inside. The distribution of molecular speeds inside a container at 300 K and in the beam that escapes through a small hole in it, each normalised to its own peak. They are not the same distribution. A molecule's chance of reaching the hole in a given time is proportional to how fast it is going, so the beam carries one more factor of speed than the gas does — v³ rather than v² times the Boltzmann factor — and the beam is therefore faster and hotter than what it came from. The mean speed inside is 476 m/s and in the beam 561 m/s, a ratio of 1.1781 against the exact 3π/8; and the mean kinetic energy is 1.500 kT inside against 2.000 kT in the beam, which are exactly 3/2 and 2. That difference is not a subtlety. A molecular beam made by effusion has a temperature, in the sense of a mean energy, a third higher than its source; a gas slowly leaking from a container leaves the remainder cooler than it would be if a fair sample had gone; and every calculation of a rate through an aperture that uses the bulk distribution is wrong by this factor.

The distribution of molecular speeds inside a container at 300 K and in the beam that escapes through a small hole in it, each normalised to its own peak. They are not the same distribution. A molecule's chance of reaching the hole in a given time is proportional to how fast it is going, so the beam carries one more factor of speed than the gas does — v³ rather than v² times the Boltzmann factor — and the beam is therefore faster and hotter than what it came from. The mean speed inside is 476 m/s and in the beam 561 m/s, a ratio of 1.1781 against the exact 3π/8; and the mean kinetic energy is 1.500 kT inside against 2.000 kT in the beam, which are exactly 3/2 and 2. That difference is not a subtlety. A molecular beam made by effusion has a temperature, in the sense of a mean energy, a third higher than its source; a gas slowly leaking from a container leaves the remainder cooler than it would be if a fair sample had gone; and every calculation of a rate through an aperture that uses the bulk distribution is wrong by this factor.

What checks it

physicscheck asserts something about speed-distribution that could fail — it draws it and measures the result against a value reached some other way.

Across the library: 100 interrogated, 2 exercised only, 1 untouched, of 103. Read out of the gate's source by the gate's own two patterns — and the gate's last claim fails the build if that read disagrees with what it was handed while running.

Where it is called

Changing this generator changes every figure on this list. That is what makes the list worth publishing rather than keeping in a check script.

Thermodynamics

Pressure is a rate of arrival, and the gas law falls out of counting

Nothing in a gas is pushing on the walls. Molecules arrive, bounce, and leave, and pressure is the momentum they deliver per second — from which the ideal gas law follows with no thermodynamics in it at all.

Thermodynamics

The gas that leaves is not the gas inside

Put a small hole in a container of gas and what comes out is faster and hotter than what stays behind — its mean kinetic energy is 2kT against the 3/2 kT of the gas it came from. Nothing has heated it. A fast molecule simply reaches the hole more often than a slow one, so the sample that escapes is biased by exactly one factor of speed, and every consequence of effusion is that factor.

Thermodynamics

The gradient that drives the other thing

A concentration gradient drives a flow of matter and a temperature gradient drives a flow of heat. Each also drives the other, by coefficients that are equal — a relation nobody could have guessed and which follows from the fact that the underlying motion runs the same forwards and backwards in time.

Thermodynamics

The speeds in a still room

The air in a quiet room is not still. Every molecule in it is moving at hundreds of metres per second, and temperature is a single number summarising an entire distribution.

Thermodynamics

Why the air thins with height, and why that is the same law as the speeds

The pressure of the atmosphere falls exponentially with altitude, and the distribution of molecular speeds falls exponentially with energy. These are not two results that happen to look alike. They are one statement read on two axes.

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