Ideal Gas Kinetic Theory Simulator
Connect the microscopic chaos of bouncing atoms to the macroscopic laws of thermodynamics and ideal gases.
About this simulation
- What
- An interactive Physics simulation of Ideal Gas Kinetic Theory Simulator.
- Who
- Designed for AP, IB, and A‑Level Physics students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-03-25
Key Concepts
Pressure origin ($p = F / A$)
Pressure isn't magic; it's just the combined force of billions of tiny molecules constantly crashing into the walls of their container.
Temperature = Kinetic Energy
Temperature is literally just a measure of how fast the molecules are jiggling. Hotter gas = faster moving atoms.
Maxwell-Boltzmann Distribution
Even though a gas has a specific temperature, individual molecules move at wildly different speeds. The distribution curve shows the statistical spread of these speeds.
Chaos creates Order
When you inflate a balloon, why does it stay expanded? Is air 'pushing' from the inside like a solid object? Not at all. Air is mostly empty space littered with tiny molecules flying around at the speed of a jet airliner.
In this simulator, you can watch these microscopic bullets in action. Every time a dot hits the wall and bounces back, it imparts a tiny kick. Billions of these kicks together create the steady force we call 'Pressure' ($p$).
Try turning up the Temperature slider. Notice how the dots fly faster (higher kinetic energy), hitting the walls harder and more often, which drives the Pressure up. This is the microscopic origin of the Ideal Gas Law: $pV = nRT$.