Internal energy and thermal energy

  • #1
138
2
I'm watching a lecture introduction internal energy and in it, the lecturer states the following for some system:

[tex] E_{internal} = E_{translational} + E_{vibrational} + E_{rotational} + E_{other} [/tex]

where ## E_{other} ## could be chemical energy, magnetic energy, electrostatic energy etc.

Then he circles ## E_{translational} + E_{vibrational} + E_{rotational} ## and states that the RANDOM portions of these energy contributions represents the thermal energy. He says there is an ordered contribution from these terms and an unordered contribution and that this unordered (or random) contribution is the thermal energy.

What does the ordered vs. random contributions mean? I have no idea what that means.
 

Answers and Replies

  • #2
DrClaude
Mentor
7,428
3,702
What does the ordered vs. random contributions mean? I have no idea what that means.
Me neither! Can you post a link to the lecture?

[tex] E_{internal} = E_{translational} + E_{vibrational} + E_{rotational} + E_{other} [/tex]
This doesn't bode well. Translational energy is definitely not a form of internal energy.
 
  • #3
mjc123
Science Advisor
Homework Helper
1,005
478
I think it's talking about the motion of a body as a whole, i.e. the coordinated motion of the atoms that make it up. For example, if you throw a ball, the translational motion of the ball is not internal energy - if you throw it faster it is not hotter - but the random motions of the atoms (superimposed on their ordered motion with the ball) do constitute internal energy - if the ball is hotter these random motions are more energetic.
 
  • #4
sophiecentaur
Science Advisor
Gold Member
25,069
4,759
Translational energy is definitely not a form of internal energy.
Is he not referring to the translational Energy of the individual molecule within the gas? After all, in elementary kinetic theory of gases, that is the only form of internal energy that's considered. The Rotational Energy that is also in the expression would normally be assumed the molecular rotation and not the coordinated rotation of the whole.
We would need to see the lecture to get the exact context of the expression. @mjc123 and I have both managed to get totally opposite messages from this; that speaks volumes. :smile:
 
  • #5
20,517
4,395
I support mjc123's description of this very standard development. An example is an ideal monatomic gas. If ##\mathbf{v_i}## is the velocity of the i'th atom, then the average velocity of the gas is $$\bar{\mathbf v}=\frac{\sum_1^N{\mathbf{v_i}}}{N}$$If ##\mathbf{v'_i}## represents the deviations from the average velocity, then $$\mathbf{v_i}=\bar{\mathbf{v}}+\mathbf{v'_i}$$The total energy of the gas is the sum of the kinetic energies its particles: $$E=\sum_1^N\frac{m}{2}(\bar{\mathbf{v}}+\mathbf{v'_i})^2=N\frac{m}{2}\bar{v}^2+\frac{m}{2}\sum_1^Nv_i^2$$where the square on the left hand side of this equation symbolically represents the dot product of the vector velocity with itself. The first term on the right hand side of this equation is the "coordinated" kinetic energy of the gas, and the second term is the "random" kinetic energy, also called the internal energy of the gas. Thus,
$$E=(KE)+U$$U is typically calculated from the Boltzmann velocity distribution.
 
  • Like
Likes Lord Jestocost
  • #7
138
2
Hey all!

Here is the lecture:
I set it to start at 1:25 but it's over the first few minutes that he discusses this.

In terms of the translational component to the internal energy, I think he is referring to the individual motions of the particles, as seen in the center of mass and as noted by @sophiecentaur.

I'll take a look at what you wrote @Chestermiller and respond soon!
 

Related Threads on Internal energy and thermal energy

  • Last Post
Replies
4
Views
1K
  • Last Post
Replies
12
Views
3K
  • Last Post
Replies
1
Views
1K
  • Last Post
Replies
7
Views
2K
  • Last Post
Replies
23
Views
44K
  • Last Post
Replies
7
Views
719
  • Last Post
Replies
9
Views
3K
Replies
11
Views
1K
Replies
20
Views
4K
  • Last Post
Replies
12
Views
2K
Top