Relation between heat capacity and internal energy

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The discussion centers on deriving the heat capacity at constant volume (Cv) and its relationship to temperature. The initial formula for internal energy is presented, but confusion arises during differentiation, leading to incorrect conclusions about the temperature dependence. Participants debate the correct application of differentiation techniques, particularly the quotient and chain rules, to achieve the desired expression. It is clarified that at high temperatures, the heat capacity should be inversely proportional to the square of the temperature. The conversation highlights the importance of accurate mathematical methods in deriving physical relationships.
trelek2
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The task is to derive an expression for the heat capacity of a system at constant volume and show that at high temperatures it is inversely proportional to the square of temperature.

As far as I'm concerned the relation between internal energy and heat capacity is:
Cv=dE/dT
However with with i cannot get a reasonable answer.

The expression for the total internal energy of a system is given by:
E= \frac{N \Delta E}{exp( \Delta E/kT) +1 } }

Where N is the total number of particles, T is the temperature, k is the Boltzmann constant.

When i differentiate it I get an expression which is negative and inversely proportional to the temperature, not to the square temperature...
 
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I do not think you are differentiating correctly. I took the partial in a big T limit and got a positive inverse T relationship. What are your steps?
 
But it is clearly supposed to be proportional to inverse square T...
I use the quotient rule E'=(u'v-uv')/v^2
and take u=NdeltaE, u'=0
v=exp(deltaE/kT)+1 v'=(deltaE/kT)exp(deltaE/kT).
This clearly gives a negative inverse T proportional.
Show me what I am supposed to do.
 
Sorry, typo. I meant to say positive inverse square T. Your v' is incorrect. Use the chain rule.
 
oh ****, you're right. How stupid I am.
 
No worries :approve:
 

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