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 and v + d v is given by d P = ( 2 π k T m ) 3 / 2 e − 2 k T m v 2 d v x d v y d v z (Maxwell Distribution) where m is the mass of the molecules, 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 > = 3 0 0 m/s , what is the mean of the inverse of the speed < 1 / v > in seconds per meter ?
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The last integral should have P ( v ) rather than 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 that the answer turned out the same. For an extreme example, you wouldn't compute the expectation of 1 by integrating 1 P ( 1 ) ...
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 , look for spherical coordinates.
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
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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 , on which dP is essentially constant. Hence the density parametrized by v is just the 3D joint density times 4 π v 2 .
Alternate way of looking at it :
We are given d V d P , where d V = d v x d v y d v z is volume element in velocity space. Thus the probability of finding a molecule with velocity around 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 V d P × 4 π v 2 d v .Now it is just a matter of finding averages
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Its clear that,
We, somehow, have to find P .
We know (I don't know how to prove it, just know it),
d x d y d z = r 2 sin θ d θ d ϕ d r
⇒ d v x d v y d v z = v 2 sin θ d θ d ϕ d v
where, θ , ϕ are the path angle and course angle respectively
Thus, the expression becomes,
d P = ( 2 π k T m ) 3 / 2 e − 2 k T m v 2 v 2 sin θ d θ d ϕ d v
If we integrate this probability with,
θ going from 0 to (\pi) and,
ϕ going from 0 to 2 π , then,
The integral turns out to be,
P ( v ) = 4 π ( 2 π k T m ) 3 / 2 v 2 e − 2 k T m v 2
Now, the average value of this function is,
< v > = 0 ∫ ∞ v P ( v ) d v
Substituting P ( v ) , and integrating,
we get,
< v > = π m 8 k T as expected.
Putting < v > = 3 0 0 ,
k T m = 2 . 8 2 9 × 1 0 − 5
Back to the average value function, substitute v as v 1 ,
< v 1 > = 0 ∫ ∞ v 1 P ( v 1 ) d v
Integrating this expression, and putting the value of k T m , we get,
< v 1 > = 4 . 2 4 × 1 0 − 3