How Do You Calculate the Rate of Incidence and Mean Free Path of Gas Molecules?

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SUMMARY

The discussion focuses on calculating the rate of incidence and mean free path of gas molecules, specifically addressing four parts of a homework problem. Part (a) derives the rate of incidence using the flux equation, resulting in R = (2/3)(rρg)/(m⟨c⟩). Part (b) calculates the speeds v1 and v2 of gas molecules, with v2 approximated at 1112 m/s and the temperature of the chamber at approximately 972K. Part (c) computes the mean free path for faster molecules as 176m, while part (d) finds the mean free path for molecules traveling at 10 m/s to be 0.24m, indicating a significant difference in behavior based on velocity.

PREREQUISITES
  • Understanding of gas kinetics and molecular dynamics
  • Familiarity with statistical mechanics and speed distribution functions
  • Knowledge of momentum and flux in physics
  • Basic grasp of thermodynamic principles, including temperature and pressure relationships
NEXT STEPS
  • Study the derivation of the Maxwell-Boltzmann speed distribution
  • Learn about the calculation of mean free path in different gas conditions
  • Explore the relationship between molecular mass and flux in gas dynamics
  • Investigate the implications of temperature on molecular speed and behavior
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Students and professionals in physics, particularly those focusing on thermodynamics, gas dynamics, and statistical mechanics, will benefit from this discussion.

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Homework Statement



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Part(a): Find rate of incidence of gas molecules.
Part(b): Find v1 and v2.
Part (c): Find mean free path for faster molecules.
Part (d): Find mean free path of 10m/s molecules.

Homework Equations


The Attempt at a Solution



Part (a)

Letting ##\phi## be flux, and ##\Delta p## be change in momentum of rebounding molecule,
\phi \Delta p = \left(\frac{4}{3}\pi r^3\right)\rho g
\phi (2m\overline c) = \left(\frac{4}{3}\pi r^3\right)\rho g
R = \frac{2}{3}\frac{r\rho g}{m \overline c}

Funny how the mass of the molecule is not given. But this make sense as the more massive the atom traveling at a certain speed, the less flux you need to support the weight.

Part (b)

t5lhs3.png


The speed distribution of molecules coming out of the oven is given by ##f = 2\alpha^2 v^3 e^{-\alpha v^2}##.

v_2 = \int_0^{\infty} v f dv
= \frac{3}{4}\sqrt{\frac{\pi}{\alpha}}
= \sqrt{\frac{9}{8}\frac{\pi kT_1}{m}}

For interest, let's calculate the temperature of the Chamber:

v_2 = \sqrt{\frac{8kT_2}{\pi m}} = \sqrt{\frac{9}{8}\frac{\pi kT_1}{m}}
T_2 = \left(\frac{3}{8}\pi\right)^2 T_1\approx 972K

To calculate ##v_1##, we use the speed distribution of the chamber (not the one coming out of the oven!)

g = 2\alpha_2^2 v^3 exp(-\alpha_2 v^2)

v_1 = 2\alpha_2^2 \int_0^{\infty} v^4 exp(-\alpha_2 v^2)
= \sqrt{\frac{9}{8}\frac{\pi kT_2}{m}}
= \pi \sqrt{\frac{81}{512}\frac{\pi k T_1}{m}} \approx 1112 ms^{-1}

Part (c)
I'm not sure whether the mean free path calculated here is correct.

The relative speed is ##v_r = |v_2 - v_1| = 1112 - 944 = 168 ms^{-1}## and ##n = \frac{P}{kT} = 2.47*10^{17}## and ##\sigma = 1.52*10^{-19}##.

Mean free path = (Distance travelled)/(No. of collisions during that distance)

\lambda = \frac{v_2t}{v_r n \sigma t} = 176m

Part (d)
In this case, ##v_r = |1112 - 10| = 1102##.

\lambda = \frac{10t}{v_r n \sigma t} = 0.24 m

This is roughly 700 times less than above.

This means that the atoms in the beam have a much larger mean free path than the atoms in the chamber. Thus velocity of the beam reduces much only after 176m into its flight path.
 
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bumpp , anyone mind checking my answers?
 

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