Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: lolhaha on March 30, 2020, 08:05:11 AM
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Hello. Encountered the following question:
"Calculate the number of molecules in 1cm^3 of an ideal gas at 27C and a pressure of 10mm Hg. Mean kinetic energy of a molecule at 27C is 4*10^-14 erg; the density of mercury is 13.6gm/cm^3"
I tried solving this using PV = nRT (as it is applicable to ideal gases)
(10/760) atm * (1/1000)L = n * 0.0821 (L)(atm) * 300K ... [760mmHg = atmospheric pressure]
n = no. of moles ~= 5.34 * 10^(-7)
no. of molecules ~= 3.22 * 10^17
HOWEVER: the question is solved using the given mean KE value and using the relation - P = 2/3 KE
The final answer given is 4.9*10^17 molecules
My question is - why is my approach wrong?
Isn't the use of the ideal gas equation correct?
Thanks a lot.
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I see nothing wrong with your result.
Fact that the answer found with the approach from kinetic theory of gases gives different result means just that the data given is inconsistent.
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Thanks Borek :D
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The value they give for mean kinetic energy is actually kT, not 3/2 kT.
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A pressure equalling an energy?
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A pressure equalling an energy?
Actually PV.
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from the kinetic theory for gases
3 (8.324 J/molK) 300.15K 1x10^7 erg 6x10^-14 erg
KE = ---- x --------------------------------- x ---------- x -------------- = ----------------
2 6.022x10^23 molecules / mol 1 1 J molecule
were did you get 4x10^-14 erg?
was the 3/2 factor left off?
what was your next equation? -P = 2/3 * KE ?
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