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cations in the SII locations, similarly, have little effect on the adsorptive properties, again, because of the shielding provided by framework oxygen (Ag-Y zeolites have very low N2 adsorptive capacity despite having a full occupancy of SII). However, silver in SII*, are very active (Hutson et al., 2000). This helps to explain the increase in the adsorptive capacity of Li94.2Ag1.1Na0.7-LSX after vacuum dehydration at 450 C over that of both the Li94.2Ag1.1Na0.7-LSX after vacuum dehydration at 350 C and the Li94.5Na1.5- LSX. From the structural determinations, only the Li94.2Ag1.1Na0.7-LSX zeolite, after vacuum dehydration at 450 C, contain silver in the SII* location. This is supported by the fact that this is the only one of these two samples that showed the enhancement in adsorptive capacity over the near-fully Li+-exchanged LSX sample. The same sample, vacuum dehydrated at 350 C, did not show an enhancement in the adsorptive capacity, because the silver is located in the inaccessible SII' location. This boost in the adsorption capacity is a result of an increase in the number of SII* cations. This increase in SII* cations is a result of thermally induced silver migration from the SII′ location. This thermally induced silver migration is likely the result of a partial breakdown of the framework from autoreduction of silver with framework oxygen as shown in Eq. 2 (Hutson et al., 2000). 2 ( A g + − Z − O − ) → 2 A g 0 + ( 12 ) O 2 + Z − O − + Z + (2) The breakdown is not significant enough to destroy the crystallinity of the zeolite, and it is random enough to prevent its detection using X-ray or neutron diffraction. However, the breakdown likely creates an energetically unfavorable environment for the silver. As a result, silver in the SII' then moves to the SII or SII* location. Repulsive forces (probably from silver in the SII' location) then push the Ag into the adsorbate 102PDF Image | PSA USING SUPERIOR ADSORBENTS
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