Ideal Gas Simulation

Interactive demonstration of ideal gas behavior, Maxwell-Boltzmann distribution, and thermodynamics

Temperature: 300 K
Pressure: 0.00 Pa
Volume: 1.00 L
Average Speed: 0 m/s

Speed Distribution

Theoretical Maxwell-Boltzmann
Actual Distribution

Parameters

Physical Equations

Ideal Gas Law: pV = Nk_BT
RMS Speed: v_rms = √(3k_BT/m)
Maxwell Distribution: f(v) = 4π(m/2πk_BT)^(3/2)·v²·e^(-mv²/2k_BT)

Display Options

Gas Presets

What is an Ideal Gas?

An ideal gas is a theoretical gas composed of many randomly moving point particles that are not subject to interparticle interactions. The ideal gas model is useful because it obeys the ideal gas law, a simplified equation of state, and is amenable to analysis under statistical mechanics.

Maxwell-Boltzmann Distribution

The Maxwell-Boltzmann distribution describes the distribution of speeds among the particles in a gas. At a given temperature, particles have a range of speeds: some move slowly, some rapidly, but most have speeds near the most probable speed. The distribution shifts to higher speeds and broadens as temperature increases.

Pressure and Molecular Collisions

Pressure in a gas results from the collisions of particles with the container walls. Each collision imparts a tiny impulse to the wall. The sum of these impulses per unit area per unit time is the pressure. Higher temperature means faster particles and more frequent, harder collisions, resulting in higher pressure.

Root-Mean-Square Speed

The root-mean-square (RMS) speed is a measure of the average speed of particles in a gas. It depends on temperature and particle mass: v_rms = √(3k_BT/m). Lighter particles move faster at the same temperature. For example, helium atoms move about 2.6 times faster than nitrogen molecules at the same temperature.

Applications

The ideal gas law and Maxwell-Boltzmann distribution are fundamental to understanding: atmospheric physics (why temperature decreases with altitude), engineering (design of engines, compressors, and HVAC systems), chemistry (reaction rates and equilibrium), and astrophysics (stellar atmospheres and interstellar gas clouds). The ideal gas model, while simplified, provides excellent predictions for real gases under ordinary conditions.