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between the charged Ag-clusters (Ag+ at SII) and the quadrupole moment of the O2 molecule (whereas, the Ar has no quadrupole moment). The N2 adsorption isotherms, measured at 25 C, for LixAgy-LSX zeolites after vacuum dehydration at 450 C for a minimum of 4 hours are shown in Figure 8 where the amount adsorbed is given in both mmol/g (top) and molec/uc (bottom). These zeolites contained varying amounts of Ag per unit cell ranging from zero (i.e., the near-fully exchanged Li94.5Na1.5-LSX sample) to 21 (the Li73.8Ag21Na1.2-LSX sample). This plot reveals that the incorporation of only a small amount of silver changes the adsorptive properties of the near-fully exchanged Li94.5Na1.5-LSX zeolite. With increasing additions of Ag+ (and corresponding removal of Li+ and Na+) the adsorption isotherms begin to take on more of the characteristics of the near-fully exchanged Ag95.3Na0.3-LSX material (i.e., the high “knee” at low pressures). Heats of Adsorption Heterogeneity in zeolites may result from a number of causes including a mixed population of charge compensating cations. If the intracrystalline cation composition is mixed, sites in the vicinity of a cation will differ for each cation whether or not they occupy equivalent crystallographic positions. Further, in a mixed cation population the proportion of one cation to another may vary from one cavity to another so that the behavior of the cavities as multiple sorption sites may vary throughout the crystal (Barrer, 1978). The presence of energetic heterogeneity of a system can be determined by plotting the isosteric heat of adsorption versus the amount adsorbed. Energetic heterogeneity of the system will result in a decrease in the isosteric heat of adsorption as the amount 99PDF Image | PSA USING SUPERIOR ADSORBENTS
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