This simulation demonstrates the kinetic molecular theory, showing how macroscopic gas properties emerge from microscopic particle collisions.
The Maxwell-Boltzmann Distribution
Watch the histogram—it shows the Maxwell-Boltzmann speed distribution:
- Most particles move at moderate speeds (the peak)
- Very few particles are extremely slow or extremely fast
- The shape emerges naturally from random collisions
- Derived independently by Maxwell (1860) and Boltzmann (1872)
Key Relationships
- Temperature ∝ Kinetic Energy: Faster particles = higher temperature
- Pressure ∝ Wall Collisions: More impacts = higher pressure
- PV = nRT: The ideal gas law emerges from these mechanics
Elastic Collisions
Particles undergo perfectly elastic collisions—total kinetic energy is conserved. During collision:
- Momentum is exchanged between particles
- Heavier particles transfer more momentum
- This leads to energy redistribution over time
Try This
- Click "Add Heat" to increase average kinetic energy
- Watch the distribution shift right (faster particles)
- Notice pressure increases as particles hit walls harder
- Change particle mass to see different distribution shapes