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Confusion Regarding Most Probable Kinetic Energy of an Ideal gas

  1. Mar 23, 2013 #1
    1. The problem statement, all variables and given/known data

    Find the most probable kinetic energy of an ideal gas molecule.

    2. Relevant equations
    v=sqrt(2RT/M)
    where v= most probable velocity
    k= Boltzmann's constant
    T= temperature of the system
    M= molar mass of the gas

    Maxwell's formula of probability distribution of kinetic energy

    3. The attempt at a solution

    The standard solution, as prescribed by many textbooks and reference materials, involves differentiation of the probability distribution equation w.r.t. kinetic energy to find the maximum and hence showing that the most probable kinetic energy is kT/2. This seems logical and I assume it is correct.

    But my doubt arises due to a different approach that I employed. Instead of differentiating the probability distribution equation if I simply plug in the value of most probable velocity in the equation for kinetic energy (mv^2/)2 then my answer turns out to be kT. I'm confused as isn't it logical to assume that the molecules with most probable velocity have the most probable kinetic energy. Please help.
     
    Last edited: Mar 23, 2013
  2. jcsd
  3. Mar 23, 2013 #2

    mfb

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    2016 Award

    Staff: Mentor

    The most probable value of v is not the most probable value of v^2. This is an unintuitive mathematical property, and can be seen for other nonlinear functions as well.
     
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