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dual-site Toth model for Beta-1,-2,-3 are smaller than b derived from the Toth model for Beta-0 and both b1 and b2 decrease with the increase of mesoporosity. Moreover, the b1-values are much greater than b2, which is similar to the result of mesoporous ZSM-5 [8], reflecting a weaker adsorbate-adsorbent interaction in mesopores than in micropores. With regard to the saturate adsorption capacities (qm and qm1, qm2) of three xylene isomers, the order is: o-xylene > p-xylene > m-xylene. The reason why o-xylene has a greater adsorption amount can be divided into two characters. On the one hand, the packing configuration of o-xylene molecules, called “face-to-face” packing orientation, can pack much more closely in the channel of Beta zeolite samples than p-xylene molecules which have a “shoulder to shoulder” packing orientation [25,26]. This may contribute to the higher saturation capacities of o-xylene than p-xylene. On the other hand, the higher ortho adsorption also corresponds to the bigger b-values, which reflect the interaction between adsorbate and adsorbent. As listed in Tables 2 and 3, the values of b for Beta-0 and b1, b2 for Beta-1,-2,-3 follow the same order of o-xylene > m-xylene > p-xylene. The result shows that o-xylene with a dipole moment interacts more strongly with the electric field of Beta zeolite than p-xylene without dipole moment. Thus, the ortho adsorption is further enhanced by electrostatic effects [27]. However, as to m-xylene, the electrostatic interaction seems to be only of secondary importance in the adsorption. The smallest adsorption capacity of m-xylene, which is inconsistent with the order of interactions, indicates that molecular configuration and size become the dominant factors in the adsorption of m-xylene on Beta zeolites. Apparently, there is only a slight difference in adsorption amounts between p-xylene and m-xylene, reflecting the combined effects of molecular configuration and electrostatic interaction. 2.2.3. Henry’s Constants and Initial Heats of Adsorption Henry’s constants (KH) and the initial heats of adsorption, which are the characterizations of interaction force between the adsorbate and adsorbent at very low adsorption pressure, were calculated from the isotherm data in this work. According to the Virial equation: ln(p/q) = −ln(KH) + A1q + A2q2 + A3q3 + ... (3) where A1, A2, A3, . . . are the virial coefficients. The plot of ln(p/q) as a function of q should approach a line while the adsorption amount q approximates to zero. The Henry’s constant (KH) could be directly calculated from the intercept –ln(KH) [28,29]. 246PDF Image | Zeolite Catalysis
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