Question

Derive the relation between Cp and Cv for an ideal gas.

Answer 1

Answer:

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 in internal energy,

that is,

qV = n CV∆T = ∆U

We know that for one mole (n=1) of an 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

CP = CV + R

CP – CV = R

Answer 2

Answer:

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Explanation:

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