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SAI = m o l a r e n t r o p y o f s p e c i e s A a t s t a t e ( 1 ) 0 / m o l K } SAO= molar entropy of species A at state (0) {J/mol K} The variables for species B are defined similarly. As enthalpy is only a function of temperature for ideal gases, the first term in the above equations is zero, so the above formulas reduce to: VAI =-T O(S AI -S AO) (2.9) WB\ ~ -^o(SBl S Bo) (2.10) As gases are separated, they move from a disordered, or more probable state to a more ordered, or less probable state. This implies a decrease in entropy and an increase in availability (Equations (2.9) and (2.10) have positive values). As the gases in state (1) have positive availability relative to state (0), a reversible change from state (1) to (0) is capable of producing work. The opposite of this work is the reversible work of separation. The isothermal change in entropy of an ideal gas species A is: (P } P\ (2.11) = -RM( _o_ {PA J The change in entropy of species B is defined analogously: fp\ fp\ -Rln (2.12) 11PDF Image | Energy Efficiency of Gas Separation Pressure Swing Adsorption
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