Physics Help Forum kinetic theory of gases

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 Oct 5th 2017, 11:33 AM #1 Junior Member   Join Date: Oct 2017 Location: west bengal,India Posts: 1 kinetic theory of gases I am confused in the collision frequency(Z). somewhere it is: Z={rms speed/mean free path} and some where Z={average speed/mean free path} which is correct and why? where collision frequency defines as the collisions made by a molecule in unit time. from, sayang
 Oct 7th 2017, 11:22 AM #2 Senior Member     Join Date: Jun 2016 Location: England Posts: 333 This link: Relates Z to the average velocity. However I think the main problem with your 2 equations is the equals sign, I think it should be a proportional sign. The speed distribution of the molecules in a gas means that the RMS and the average are closely related. See this link: __________________ ~\o/~
 Oct 8th 2017, 07:12 AM #3 Senior Member   Join Date: Aug 2010 Posts: 242 The term "average" can mean a number of different things: The "mean" where you add up the values and divide by the number of them: the "mean" of {1, 3, 3, 3, 6, 8} is (1+ 3+ 3+ 3+ 6+ 8)/6= 24/6= 4. The "median" which is the "middle" of all the numbers. Here, there are 6 numbers. The "middle" is between the third and fourth numbers. Since both third and fourth numbers are 3, that is 3. The "mode" which is the most common number. Here, that is 3. The "midrange" which is simply half way between the smallest and largest numbers. Here the "range" is "1 to 8" so the "midrange" is (1+ 8)/2= 4.5. The "root mean square" which is the square root of the mean of all the square. The mean of the squares is (1+ 9+ 9+ 9+ 36+ 64)/6= 128/6= 21.3. The square root of that is 4.6. The "average speed" could be any one of those, though most likely the "mean" as that is the most commonly used "average". The "root mean speed" specifically uses the last.

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