Linked from

The 18 pages that link to Maxwell–Boltzmann distribution, each with the reason it gives.

• Kinetic theory of gasesRelated: It shows why gas particles have a range of speeds rather than one shared speed.

• Ludwig BoltzmannRelated: Boltzmann helped derive the distribution that predicts molecular speeds in thermal equilibrium.

• Ideal gasRelated: It describes the range of molecular speeds behind gas pressure and temperature.

• Doppler broadeningRelated: Thermal particle velocities supply the spread of shifts that produces the line profile.

• Boltzmann equationRelated: It is a stationary solution of the collision dynamics under equilibrium conditions.

• Molecular beamRelated: It predicts the speed spread of molecules emerging from a thermal source.

• Collision theoryRelated: It determines what fraction of collisions exceed the activation energy at a given temperature.

• Gas constantRelated: In its molar-energy form, R sets the distribution’s temperature scale.

• Gas-phase chemistryRelated: It predicts what fraction of gas molecules has enough energy to overcome a reaction barrier.

• Number densityRelated: Its velocity distribution is normalized using the gas's number density.

• Collision frequencyRelated: Thermal speed variation means collision frequencies are averaged over a distribution, not one speed.

• Graham's lawRelated: Effusion samples faster-than-average molecules, while preserving the mass-dependent speed scaling.

• Atomic and molecular collisionsRelated: It connects single-collision energy dependence to rates averaged over a gas.