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hadoque
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Homework Statement
From Milton Ohrings "Materials science of thin films", problem 3.5.
An Al film was deposited at a rate of ~1[tex]\mu[/tex]m/min in vacuum at 25°C,
and it was estimated that the oxygen content of the film was [tex]10^{-3}[/tex]. What
was the partial pressure of oxygen in the system?
Homework Equations
Vapor pressure of liquid Al
[tex]\log(P) = 15.993/T + 12.409 - 0.999\log{(T)} - 3.52 \cdot 10^{-6}T[/tex]
P, pressure(torr)
K, temperature (kelvin)
Impurity concentration (evaporant vapor impingement rate/gas molecule impingement rate)
[tex] C_i = 5.82 \cdot 10 ^{-2}\frac{P M_a}{\rho d \sqrt{M_g T }}[/tex]
[tex]M_a[/tex], evaporant gas molecular weight
[tex]M_g[/tex], gas molecular weight
d, deposition rate (cm / s)
[tex]\rho[/tex], density of deposition
P, residual gas vapor pressure (torr)
The Attempt at a Solution
I haven't made much calculations yet, I mainly wan't to check that I understand everything correctly.
My idea is that I can calculate the total pressure of the chamber with the impurity equation. After that I could subtract the pressure caused by the Al vapor to get the oxygen pressure.
I'm having a bad feeling about this though. Isn't the T of the vapor pressure equation the temperature of the melt?
Also, I asked an assistant in school. He hadn't looked at the problem yet, but he talked about not being able to use the impurity equation in that form because something wasn't a perfect gas. Well, the oxygen at that pressure surely must be a perfect gas? And the vapor impingement rate is not calculated with the perfect gas law, so I wonder if he was thinking about the right problem...