Abstract
The Gibbs paradox results from analyzing mixing entropy as if it was a type of thermodynamic entropy. It begins with an adiabatic box divided in half by an adiabatic removable partition. There are two ideal gases, at equal temperatures and pressures, distinguishable as gas A and gas B, each separately contained in separate halves of the box. The partition is removed, the two gases mix. Mixing entropy theory predicts a significant change in temperature for the gases due to mixing. However, experimental results show that the mixing process produces no detectable change in temperature. The solution presented in this essay introduces new explanations for both thermodynamic entropy and mixing entropy. It is shown that the paradox is not real. The prediction of mixing entropy is illusory due to an incorrect assumption: The mixing entropy is not like Clausius’ thermodynamic entropy. The subject of this essay was chosen to demonstrate the negative consequences of theorists bypassing an understanding of what is Clausius’ thermodynamic entropy.
James A Putnam