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4.10 The Maxwell-Boltzmann Distribution

Take-home message: The density of states can be used to derive the Maxwell-Boltzmann distribution of molecular speeds in a gas.

The speed $v$ of a particle is related to the wavenumber $k$ by $mv=\hbar k$. We already know the probability of a particle having $k$ in the range $k\to k+{\rm d}k$, and so we can immediately write down the corresponding probability of the speed being in the range $v\to {\rm d}v$:

\begin{eqnarray*}
P(k\to k+{\rm d}k)\!\!\!&=&\!\!\!{D(k)  e^{-\varepsilon(k)\be...
...style B}T}\right)^{3/2} v^2 e^{-mv^2/2k_{\scriptscriptstyle B}T}
\end{eqnarray*}



This is called the Maxwell-Boltzmann distribution, and it is plotted below.

\begin{figure}\begin{center}\mbox{\epsfig{file=max_boltz.eps,width=6truecm,angle=0}}
\end{center}\end{figure}

We can find the most probable speed (from ${\rm d}P(v)/ {\rm d}v=0$), as well as the mean speed and the rms speed:

\begin{eqnarray*}
v_p\!\!\!&=&\!\!\!\sqrt{{2k_{\scriptscriptstyle B}T\over m}}\a...
...T\over m}}\approx 1.73\sqrt{{k_{\scriptscriptstyle B}T\over m}}
\end{eqnarray*}



These are marked on the graph above.

Note that $\hbar$ has disappeared from $P(v)$, which can be derived from the Boltzmann distribution in a purely classical theory provided the normalisation is obtained from requiring the integral of $P(v)$ to be one.

References


next up previous contents index
Previous: 4.9 The ideal gas
Judith McGovern 2004-03-17