**Maxwell Speed Distribution**

Classically, an ideal gas' molecules bounce around with somewhat arbitrary velocities, never interacting with each other. In reality, however, an ideal gas is subjected to intermolecular forces. It is to be noted that the aforementioned classical treatment of an ideal gas is only useful when modeling situations in which the particle density is very low. In such situations, the particles themselves can be considered to have approximately zero volume when compared to the volume which contains them, thus giving rise to classical theory. i.e. given that such a situation would have an extremely low probability of having molecules interact with each other.

Consequently, we need to consider these interactions in order to acquire a more accurate sense of how particles behave in a gas. This leads us to **Maxwell's speed distribution (MSD)**, named after James Clerk Maxwell to whom this theory is attributed. MSD is a probability distribution describing the dispersion of these molecular speeds. MSD can only be applied when dealing with an ideal gas. More accurately, we apply MSD to gases that are "almost" ideal, given that no gas is truly ideal. Air, for example, at STP behaves similarly to an ideal gas, allowing MSD to be applied.

Note that speed is a scalar quantity, describing how fast the particles are moving, regardless of direction. Velocity, on the other hand, describes the direction as well as the speed at which the particles are moving. This is a necessary consideration given that space is three dimensional, implying that for any given speed, there are many possible velocity vectors.

The probability of a molecule having a given speed can be found by using the Boltzmann factor. Considering the energy to be dependent only on the kinetic energy, we find that:

where, *m* is the mass of the molecule, *k* is Boltzmann's constant, and *T* is the temperature.

The above equation gives us the probability of a given speed component, which we can assume to be any of without loss of generality. In 3 dimensions, we need to consider that particles can have all possible combinations of speed components, which leads us to the need to consider, as opposed to just considering *v*. In other words, we need to sum all potential combinations of the individual components in 3 dimensional velocity space in order for their vector sum to be the desired value. To get the distribution in 3 dimensions, we need to integrate the above equations in over the entire velocity space such that the component sum is constant. If we picture the particles with speed v in a 3-dimensional velocity space, we can see that these particles lie on the surface of a sphere with radius *v*. The larger *v* is, the bigger the sphere, and the more possible velocity vectors there are. So the number of possible velocity vectors for a given speed is analogous to the surface area of a sphere of radius *v*.

Multiplying these two functions together gives us the distribution, and normalising this gives us the MSD in its entirety.

(Again, *m* is the mass of the molecule, *k* is Boltzmann's constant, and *T* is the temperature.)

Since this formula is a normalised probability distribution, it gives the probability of a molecule having a speed between and *v* + *dv*. The probability of a molecule having a speed between two different values *v*_{0} and *v*_{1} can be found by integrating this function with *v*_{0} and *v*_{1} as the bounds.

Read more about Maxwell Speed Distribution: Averages

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