A Remark on the GIBBS-Paradox of the Entropy of Mixing of Ideal Gases

1991 ◽  
Vol 95 (4) ◽  
pp. 537-537 ◽  
Author(s):  
Klaus-Dieter Wantke
Keyword(s):  
Gibbs Paradox ◽  
Entropy Of Mixing ◽  
Ideal Gases

Gibbs' paradox for entropy of mixing

1985 ◽  
Vol 62 (1) ◽  
pp. 47 ◽  
Author(s):  
H. R. Kemp
Keyword(s):  
Gibbs Paradox ◽  
Entropy Of Mixing

scholarly journals Entropy Calculation of Reversible Mixing of Ideal Gases Shows Absence of Gibbs Paradox

Entropy ◽  
1999 ◽  
Vol 1 (2) ◽  
pp. 25-36 ◽  
Author(s):  
Vasili Tatarin ◽  
Oleg Borodiouk
Keyword(s):  
Gibbs Paradox ◽  
Ideal Gases

MEMBRANE EQUILIBRIA, THE GIBBS–DALTON LAW AND THE ENTROPY OF MIXING

1949 ◽  
Vol 27b (12) ◽  
pp. 988-1014
Author(s):  
E. A. Flood ◽  
G. C. Benson
Keyword(s):  
The Other ◽  
Explicit Solutions ◽  
Classical Thermodynamic ◽  
Equilibrium Conditions ◽  
Semipermeable Membranes ◽  
Equilibrium Pressure ◽  
Entropy Of Mixing ◽  
Ideal Gases ◽  
Special Case ◽  
Thermodynamic Basis

When two pure fluids whose pressures are p1e and p2e, respectively, are separated by means of semipermeable membranes from a mixture of these fluids, and under equilibrium conditions the pressure of the mixture is P, then the net pressures sustained by the diaphragms are P − p1e and P − p2e respectively. The assumption that these net pressures are p2e and p1e, respectively, is equivalent to assuming the Gibbs–Dalton law, namely p1e + p2e = P. It is shown that the Gibbs–Dalton law when applied to fluids that are not ideal gases leads to consequences which are entirely contrary to experience and that as applied to ideal gases it has neither an experimental nor theoretical thermodynamic basis. It is shown that the Gibbs–Dalton law is only a special case of Dalton's law and that the classical thermodynamic paradox in the entropy of mixing of ideal gases is based on the erroneous assumption that the Gibbs–Dalton law necessarily holds when Dalton's law holds. It is shown that when two ideal gases obey Dalton's law of mixing, it is thermodynamically quite possible for the equilibrium pressure of one pure gas to be increased while that of the other is decreased, as well as the more familiar case of "chemical reaction", where the equilibrium pressures of both are decreased. It is shown that there is no purely thermodynamic requirement that different kinds of molecules in mixtures of ideal gases shall have the same mean translatory kinetic energy. The ideas underlying membrane equilibria are discussed in some detail. Some general condition equations which must be met are given, together with a few explicit solutions of these equations for special simple cases.

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