When heat is absorbed by a body, temperature of the body increases. And when heat is lost, the temperature decreases. Temperature of any object is the measure of the total kinetic energy of the particles that make up that object. So when heat is absorbed by an object this heat gets translated into the kinetic energy of the particles and as a result the temperature increases. Thus, the change in temperature is proportional to the heat transferred. The formula q = n C ∆T represents the heat q required to bring about ∆T difference in temperature of one mole of any matter. The constant C here is called the molar heat capacity of the body. Thus, molar heat capacity of any substance is defined as the amount of heat energy required to change the temperature of 1 mole of that substance by 1 unit. It depends on the nature, size and composition of the system. In this article we will discuss two types of molar heat capacity – CP and CV and derive a relationship between them.
What are Heat Capacity C, CP and CV?
- The molar heat capacity C, at constant pressure, is represented by CP.
- At constant volume, the molar heat capacity C is represented by CV.
In the following section, we will find how CP and CV are related, for an ideal gas.
Relationship between CP and CV for an Ideal Gas
From the equation q = n C ∆T, we can say:
At constant pressure P, we have qP = n CP∆T
This value is equal to the change in enthalpy, that is, qP = n CP∆T = ∆H
Similarly, at constant volume V, we have qV = n CV∆T
This value is equal to the change internal energy, that is, qV = n CV∆T= ∆U
We know that for one mole (n=1) of ideal gas,
∆H = ∆U + ∆(pV )
= ∆U + ∆(RT )
= ∆U + R∆T
Therefore, ∆H = ∆U + R ∆T
Substituting the values of ∆H and ∆U from above in the former equation,
CP∆T = CV∆T + R ∆T
Or CP = CV + R
Or CP – CV= R
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