Fun With Maxwell Distribution

The Maxwell distribution describes the velocities of the molecules of an ideal gas at equilibrium. The probability for finding a molecule with velocities between v \vec{v} and v + d v \vec{v}+d\vec{v} is given by d P = ( m 2 π k T ) 3 / 2 e m v 2 2 k T d v x d v y d v z (Maxwell Distribution) dP=\left(\frac{m}{2\pi k T}\right)^{3/2} e^{-\frac{m v^{2}}{2 k T}} dv_{x} d v_{y} d v_{z} \quad \text{(Maxwell Distribution)} where m m is the mass of the molecules, k k is the Boltzmann constant and T is the temperature of the gas. If the mean speed of the molecules of a gas is < v > = 300 m/s <v>=300~\text{m/s} , what is the mean of the inverse of the speed < 1 / v > <1/v> in seconds per meter ?


The answer is 0.00424.

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1 solution

Anish Puthuraya
Feb 7, 2014

Its clear that,
We, somehow, have to find P P .

We know (I don't know how to prove it, just know it),
d x \displaystyle dx d y dy d z = r 2 sin θ dz = r^2\sin\theta d θ d\theta d ϕ d\phi d r dr

d v x \Rightarrow dv_x d v y dv_y d v z = v 2 sin θ dv_z = v^2 \sin\theta d θ d\theta d ϕ d\phi d v dv
where, θ , ϕ \displaystyle \theta,\phi are the path angle and course angle respectively

Thus, the expression becomes,
d P = ( m 2 π k T ) 3 / 2 e m v 2 2 k T v 2 sin θ d θ d ϕ d v \displaystyle dP = \left(\frac{m}{2\pi kT}\right)^{3/2} e^{-\frac{mv^2}{2kT}} v^2 \sin\theta d\theta d\phi dv

If we integrate this probability with,
θ \theta going from 0 0 to (\pi) and,
ϕ \phi going from 0 0 to 2 π 2\pi , then,

The integral turns out to be,
P ( v ) = 4 π ( m 2 π k T ) 3 / 2 v 2 e m v 2 2 k T P(v) = 4\pi\left(\frac{m}{2\pi kT}\right)^{3/2} v^2e^{-\frac{mv^2}{2kT}}

Now, the average value of this function is,
< v \displaystyle v > = 0 v P ( v ) d v \displaystyle = \int\limits_0^{\infty} v P(v) dv

Substituting P ( v ) P(v) , and integrating,
we get,
< v \displaystyle v > = 8 k T π m \displaystyle = \sqrt{\frac{8kT}{\pi m}} as expected.

Putting < v v > = 300 = 300 ,
m k T = 2.829 × 1 0 5 \displaystyle \frac{m}{kT} = 2.829\times 10^{-5}

Back to the average value function, substitute v \displaystyle v as 1 v \displaystyle \frac{1}{v} ,
< 1 v \displaystyle \frac{1}{v} > = 0 1 v P ( 1 v ) d v \displaystyle = \int\limits_0^{\infty} \frac{1}{v} P(\frac{1}{v}) dv

Integrating this expression, and putting the value of m k T \displaystyle\frac{m}{kT} , we get,
< 1 v \displaystyle \frac{1}{v} > = 4.24 × 1 0 3 \displaystyle = \boxed{4.24\times 10^{-3}}

The last integral should have P ( v ) P(v) rather than P ( 1 / v ) P(1/v) : the density function hasn't changed, only the quantity whose expectation you're taking. It's only by virtue of the fact that the logarithmic differential dv/v happens to be invariant under v 1 / v v\mapsto 1/v that the answer turned out the same. For an extreme example, you wouldn't compute the expectation of 1 by integrating 1 P ( 1 ) 1 P(1) ...

Erick Wong - 7 years, 3 months ago

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Yes it should be P ( v ) P(v)

Sumanth R Hegde - 4 years, 4 months ago

Hey Anish! :)

If you are interested in knowing where the following comes from: d x d y d z = r 2 sin θ d θ d ϕ d r dx\,dy\,dz=r^2\sin\theta d\theta d\phi dr , look for spherical coordinates.

Pranav Arora - 7 years, 4 months ago

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Thanks, I will.

Anish Puthuraya - 7 years, 4 months ago

what about r ? Shouldn't we be integrating from 0 to all possible values of v ? (possibly from -c to c in each axes) where c is the velocity of light. Are you looking at using flux of particles out of a surface area divided by the area so that the r term drops out. If we look at volume, there will be an r term left. But there seem to be too many unknowns

Sundar R - 7 years, 4 months ago

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The probability distribution would not integrate to 1 if you restrict to speeds to less than c, so the question implicitly ignores relativistic effects. The calculation of P(v) is essentially a roundabout way to project the 3D distribution onto the single variable of speed: the region between v and v+dv is a spherical shell of thickness dv and surface area 4 π v 2 4\pi v^2 , on which dP is essentially constant. Hence the density parametrized by v is just the 3D joint density times 4 π v 2 4\pi v^2 .

Erick Wong - 7 years, 3 months ago

Alternate way of looking at it :

We are given d P d V \frac{dP}{dV} , where d V = d v x d v y d v z dV = dv_{x}dv_{y}dv_{z} is volume element in velocity space. Thus the probability of finding a molecule with velocity around v v would be d P = p r o b a b i l i t y d e n s i t y × V o l u m e e l e m e n t = d P d V × 4 π v 2 d v dP = probability ~density × Volume~element = \frac{dP}{dV}×4πv^2dv .Now it is just a matter of finding averages

Sumanth R Hegde - 4 years, 4 months ago

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