7.1.7

Molecular Kinetic Theory Model 2

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Average molecular kinetic energy

The average molecular energy can be used to find the pressure of radiation.

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Kinetic energy

  • We assume that a gas is homogeneous (the same everywhere) and isotropic (has the same value when measured in different directions).
  • This means that the average speed of a molecule in the x-direction must be the same as the y and the z-directions. So we can write:
    • cx=cy=cz\langle{c_x}\rangle=\langle{c_y}\rangle=\langle{c_z}\rangle
  • This means that the average kinetic energy in each direction is the same.
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Momentum

  • We consider a cube of length l which contains a gas.
  • If we only look at the x-direction, we can say that the time taken for a particle to travel from one end to the other is:
    • t=lcxt=\frac{l}{\langle{c_x}\rangle}
  • If a particle collides with the wall of the box and is absorbed, we can write the change in momentum as:
    • Change in momentum = mass x velocity
    • P=mcxP=m\langle{c_x}\rangle
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Force

  • We can write the force exerted on the wall when it absorbs a particle as:
    • Force = change in momentum ÷ change in time
    • F=PtF=\frac{P}{t}
  • We can substitute in the equations for momentum and time to get:
    • F=mcx2lF=\frac{m\langle{c_x}^2\rangle}{l}
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Pressure

  • The pressure on the wall of the box when it absorbs one particle is given by the equation:
    • Pressure = force ÷ area
    • p=FAp=\frac{F}{A}
  • We can use the value for force and that the area is length squared to get:
    • p=mcx2l3p=\frac{m\langle{c_x}^2\rangle}{l^3}
  • Since volume is length cubed we get:
    • p=mcx2Vp=\frac{m\langle{c_x}^2\rangle}{V}
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Pressure 2

  • We have found the pressure for one particle if N particles hit the wall the pressure would be:
    • Total pressure = number of particles x pressure from one particle.
    • pt=Np{p_t}=Np
  • We can substitute the pressure in to give:
    • pt=Nmcx2V{p_t}=N\frac{m\langle{c_x}^2\rangle}{V}
Illustrative background for Kinetic equation Illustrative background for Kinetic equation  ?? "content

Kinetic equation

  • Recalling that the velocity is the same in all directions, we can write an equation for the total velocity squared as:
    • c2=cx2+cy2+cz2\langle{c}^2\rangle= \langle{c_x}^2\rangle+\langle{c_y}^2\rangle+\langle{c_z}^2\rangle
  • Because the velocities are equal, we can simplify to give:
    • cx2=13ct2\langle{c_x}^2\rangle=\frac{1}{3}\langle{c_t}^2\rangle
  • So the equation for pressure can be written as:
    • pV=13Nmc2pV=\frac{1}{3}Nm\langle c^2\rangle

Kinetic Energy of a Molecule

Using the results we obtained from the molecular kinetic theory derivation, we can find the temperature dependence of the kinetic energy of a molecule.

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Ideal gas law

  • Recall that the ideal gas law in terms of the Boltzmann constant, kk is:
    • pV=NkTpV=NkT
  • And the equation of the molecular kinetic theory is:
    • pV=13Nmc2pV = \frac{1}{3} Nm\langle c^2\rangle
  • Equating the two gives:
    • NkT=13Nmc2NkT=\frac{1}{3}Nm\langle c^2\rangle
Illustrative background for Kinetic energy of a moleculeIllustrative background for Kinetic energy of a molecule ?? "content

Kinetic energy of a molecule

  • We can cancel a factor of NN from each side to give:
    • kT=13mc2kT=\frac{1}{3}m\langle c^2\rangle
  • Finally, multiplying each side by 32\frac{3}{2}, we obtain an expression for the average kinetic energy for a molecule:
    • 12mc2=32kT\frac{1}{2}m\langle c^2\rangle = \frac{3}{2}kT
  • The average kinetic energy for a molecule is proportional to the temperature.

Molecular Kinetic Theory - Developments Over Time

Ideas about the underlying structure of materials have changed considerably over time.

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Early ideas

  • The idea that the atom, or atoms that are too small to directly view, move around is ancient. This dates from Lucretius in approx 50 BCE.
  • This idea was largely ignored because of the predominance of Aristotelian ideas about elements such as fire, earth, air and water.
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Particle nature of matter

  • The modern theory of the particle nature of matter was attributed to Bernoulli.
  • This was prior to the ideas of conservation of energy and how collisions between particles could be elastic.
  • The model did not predict anything in itself.
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More complex ideas

  • Clausius developed a much more complex set of ideas.
  • The observation of Brownian motion is the first direct evidence of the existence of particles.
  • The kinetic theory of gases became universally accepted because of Einstein and Smoluchowski’s theoretical model, which made specific predictions about Brownian motion and diffusion.

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