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2.2.2 Adsorption Thermodynamics Adsorption equilibrium determines how much of a fluid molecule is trapped in an adsorbent at a defined pressure, temperature, and composition. Adsorption causes a gas molecule to lose at least one of its translational degrees of freedom because it restricts the gas molecule to move along the adsorbent surface. This causes a decrease in entropy (ΔS) and since adsorption is a spontaneous process, Gibbs free energy (ΔG) is reduced as well. According to the thermodynamic expression in equation 2.2, ΔH (enthalpy) also must decrease (heat is released), making adsorption an exothermic process. Isotherms are a typical method of representing equilibrium for single component adsorption. Isotherms are measured at a constant temperature while the pressure is varied and the amount of adsorbate is measured. They form different shapes as shown in Figure 2.5. Type I isotherms are most relevant to this study and represent adsorbents that have pores similar in size to the adsorbate molecules and fill up as a saturation limit is approached. The other types of isotherms have larger pores compared to the adsorbate and hence do not experience this saturation limit, except for type IV and V isotherms near Ps. Type III isotherms represent systems where an adsorbate interacts more strongly with other adsorbates than with the adsorbent. Type II isotherms can have multiple adsorbed layers because of their larger pore size distribution and represents the other type of isotherm sometimes used in a PSA process. 15PDF Image | LIMITS OF SMALL SCALE PRESSURE SWING ADSORPTION
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