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=====Lecture: Heat Capacity (10 minutes)=====

  * This lecture should bring in points that were previously covered in a discussion of the Dulong and Petit Rule. 
  * It should be noted that although the heat capacity depends on many different factors, the values should all be reasonably close to the value given by Dulong and Petit











=====Lecture notes from Dr. Roundy's 2014 course website:=====
As we learned last week, **heat capacity** is amount of energy required to raise the temperature of an object by a small amount.
$$C \sim \frac{đ Q}{\partial T}$$
$$đ Q = C dT \text{   At constant what?}$$
If we hold the volume constant, then we can see from the first law that
$$dU = đQ - pdV$$
since $dV=0$ for a constant-volume process,
$\newcommand\myderiv[3]{\left(\frac{\partial #1}{\partial #2}\right)_{#3}}$
$$C_V = \myderiv{U}{T}{V}$$
But we didn't measure $C_V$ on Monday, since we didn't hold the volume of the water constant. Instead we measured $C_p$, but what is that? To distinguish between different sorts of heat capacities, we need to specify the sort of path used. So, for instance, we could write
$$đQ=Tds$$
$$đQ=C_αdT+?dα$$
$$TdS=C_αdT+?dα$$
$$dS= \frac{C_\alpha}{T} dT + \frac{?}{T}d\alpha$$
$$C_\alpha = T \myderiv{S}{T}{\alpha}$$

This may look like an overly-tricky derivative, so let's go through the first law and check that we got it right in a few cases. I'll do the $C_V$ case. We already know that
$$dU=đQ-pdV$$
$$C_V= \myderiv{U}{T}{V}$$
$$= \myderiv{U}{S}{V} \myderiv{S}{T}{V}$$
$$= T \myderiv{S}{T}{V}$$
where the second step just uses the ordinary chain rule.


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