The Maxwell-Boltzmann distribution Flashcards
In classical thermodynamics, the energy of a molecule is strictly considering transitional motion and neglecting what two types of motion.
Rotational and Vibraitonal.
What assumptions are being made when determining the distribution of molecular velocity?
- Molecular size is much less than the inter-molecular separation, so that we assume that molecules spend most of their time whizzing around only rarely bumping into each other. 2. We will ignore any inter-molecular forces.
If molecules are equally likely to have all types of velocities then the name of the fraction of molecules with velocities in, say, the x direction, between vx and vx + dvx, as g(vx) dvx is given to be what? Specifically, what is the name of g(vx).
Velocity Distribution Function.
The point of ___________ is to make variables comparable to each other. _______________ is the process of reducing measurements to a “neutral” or standard scale.
Normalization.
Each molecule can exchange energy with each other due to collisions, but everything remains in equilibrium. Each molecule therfore behaves like a small system connected to a heat reservoir at temperature T, where the heat reservoir is “all the other molecules in the gas”. Hence the results of the _____________ distribution of energies.
Boltzmann.
Explain the intuition behind x = 0, that is to explain why the average velocity is 0. Where x is the average of x.
Particles are moving in all directions with all types of velocities. Since a gas’ particles are in random motion, it is plausible that there will be about as many moving in one direction as in the opposite direction, meaning that the average velocity for a collection of gas particles equals zero.
What is the mean velocity, v<strong>x</strong>2, of a collection of gas equal to?
kBT / m.
Describe the distribution function for molecular speeds?
Slightly skewed right.
Give the probability distribution for a given component of velocity. Specifically, what is the probability distribution proportional to?
g(vx) ∝ e-m(vx·vx) /2kBT.
What is the probability distribution of molecular speeds proportional to and what is the name given for it.
f(u) ∝ u2 e-m(u·u)/2kBT
Maxwell-Boltzmann Distribution.
What is u2 = ?
Note: Boldness of the letter is to mean the average of that letter.
3kBT / m.
<u2> = <v2> = vx2 + vy2 + vz2,
where vx2 = vy2 = vz2 = kBT / m.
What is used to overcome the “directional” component of velocity and simultaneously acquire the particles’ average velocity?
Vrms = [u2]1/2 = [3kBT/m]1/2.
This is understood to be the root mean squared speed.
The average energy of a molecule in a gas depends only on what thermodynamic variable?
Temperature.
EKE = mu2/2 = mu2/2 = 3kBT/2.
Again the bolding represents the average of whatever is being bolded.
An electronvolt (symbol eV, also written electron-volt and electron volt) is the amount of kinetic energy gained by a single electron accelerating from rest through an electric potential difference of one volt in vacuum. When used as a unit of energy, the numerical value of 1 eV in joules (symbol J) is equivalent to the numerical value of the charge of an electron in coulombs (symbol C). So what does 1 ev = ?
1 eV = 1.602176634×10−19 J.
W = qΔV = e-(1 volt) = 1.60217662 × 10-19 coulombs x 1 volt = 1.602176634×10−19 J = 1 eV.
_________ _______ (also called separation energy) is the minimum energy required to disassemble a system of particles into separate parts. A bound system is typically at a lower energy level than its unbound constituents.
Binding energy.