Thermodynamics - Thermal Energy of a gas

  • #1
WolfeSieben
20
0

Homework Statement



The rms speed of the molecules in 1.2 g of hydrogen gas is 1800 m/s.
What is the thermal energy of the gas?

Homework Equations



m = Mass of 1 H molecule: 1.67 x 10^-27 kg
N = Total # of molecules = 7.19 x 10^23 molecules
c = rms speed

The equation provided by my tutor was:

E(therm) = N x (1/2)(m)(c)^2



The Attempt at a Solution




Using the formula i was provided with above:

E(therm) = (7.19 x 10^23 molecules)(1/2)(1.67x10^-27 kg)(1800^2 m/s)

Which equates to 1,945 J.

This answer is wrong, and I am also confused because this number seems oddly close to the translational energy (e=1/2mv^2) which equates to 1.9 KJ earlier in the assignment)

Can someone tell me if I way out to left field and provide some hints?

Thanks
 

Answers and Replies

  • #2
Andrew Mason
Science Advisor
Homework Helper
7,722
430
"Thermal energy" can refer to the total internal energy of the gas, not just the translational kinetic energy. The H2 molecule has two degrees of rotational freedom in addition to the three degrees of translational freedom. So you have to multiply the translational energy by 5/3 to get the total internal (thermal) energy.

AM
 
  • #3
WolfeSieben
20
0
Perfect, so I multiplied 1.9 KJ by 5/3 and it gave me the correct answer.

However I am interested in understanding the concept behind the question. Why is it that the degrees of rotational freedom and 3 degrees of translational freedom equate to multiplying by 5/3?

Thanks for your help!
 
  • #4
Andrew Mason
Science Advisor
Homework Helper
7,722
430
Perfect, so I multiplied 1.9 KJ by 5/3 and it gave me the correct answer.

However I am interested in understanding the concept behind the question. Why is it that the degrees of rotational freedom and 3 degrees of translational freedom equate to multiplying by 5/3?

Thanks for your help!
It is a bit complicated. You should review the kinetic theory of gases and the equipartition law.

A monatomic gas (single atoms) has no moment of inertia (virtually all the mass is located at the tiny centre). So the atoms have translational kinetic energy in three directions and no rotational or vibrational energy. According to the equipartition theory, at thermal equilibrium N atoms having 3 degrees of freedom will have 3NkT/2 energy (each degree of freedom carrying NkT/2 energy).

Now, with an H2 molecule the molecular mass is spread out because there are two nuclei separated by a comparatively large space (ie compared to the size of one nucleus). This gives the diatomic molecule a moment of inertia about two axes (the 2 axes perpendicular to the axis joining the nuclei). It has virtually no moment of inertia about the third axis joining the nuclei because the mass is all on that axis. That gives it 2 additional degrees of freedom for a total of 5, each with NkT/2 energy (according to the equipartition law).

For reasons that I am not quite clear on myself, light nuclei such as H2 lack a vibrational mode at least at lower temperatures so they only have 5 degrees of freedom, 3 translational and 2 rotational each carrying NkT/2 of energy.

AM
 
  • #5
gomunkul51
275
0
@WolfeSieben: I am sure your tutor didn't asked you to solve that question without teaching you the theory/concept behind it. I advise you to go back to your class notes/course book and study the chapter dealing with kinetic energy (or internal energy) of non monoatomic (or polyatomic) gases.
Andrew Mason gave a good explanation, but you need study material and also examples.

good luck !
 

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