- #1
cwill53
- 220
- 40
- Homework Statement
- Calculate the mean free path of air molecules at ##3.5\cdot 10^{-13}atm## and 300K. Model the air molecules as spheres of radius ##2.0\cdot 10^{-10}m##
- Relevant Equations
- $$\lambda =\frac{k_{b}T}{4\pi \sqrt{2}r^2p}$$
I used the form of the mean free path equation taking advantage of the fact that the Boltzmann constant is equal to the ideal gas constant R divided by Avogadro's number, because I didn't know if I could use the Boltzmann constant in the ##1.381\cdot 10^{-23}J/(molecules\cdot K)## form:
$$\lambda =\frac{RT}{4\pi \sqrt{2}r^2pN_{A}}=\frac{(008206(L\cdot atm)/(mol\cdot K))(300K)}{4\pi \sqrt{2}(2.0\cdot 10^{-10}m)^2(3.5\cdot 10^{-13}atm)(6.022\cdot 10^{23}mol^{-1})}=164308154.9m$$
There is no answer written in the back of the book for this particular question and when I looked the question up online I'm getting answers far from mine. I would have thought we would have to use the R constant with the units ##\frac{L\cdot atm}{mol\cdot K}##.
$$\lambda =\frac{RT}{4\pi \sqrt{2}r^2pN_{A}}=\frac{(008206(L\cdot atm)/(mol\cdot K))(300K)}{4\pi \sqrt{2}(2.0\cdot 10^{-10}m)^2(3.5\cdot 10^{-13}atm)(6.022\cdot 10^{23}mol^{-1})}=164308154.9m$$
There is no answer written in the back of the book for this particular question and when I looked the question up online I'm getting answers far from mine. I would have thought we would have to use the R constant with the units ##\frac{L\cdot atm}{mol\cdot K}##.