Differential heats, isotherms, the differential entropies and thermokinetics of benzene adsorption in the zeolite LiY at 303K have been measured using the method of adsorption calorimetry. Differential molar entropy and free energy of adsorption were calculated. The isotherms of adsorption were quantitatively reproduced on the basis of three-term VOM theory. These data formed the basis for identifying the detaled mechanism of benzene adsorption in LiY zeolite.

Анотація наукової статті за медичними технологіями, автор наукової роботи - Abdurakhmonov Eldor, Rakhmatkariev Gairat, Rakhmatkarieva Feruza, Ergashev Oybek

Область наук:
  • Медичні технології
  • Рік видавництва: 2018
    Журнал: Austrian Journal of Technical and Natural Sciences



    ?Abdurakhmonov Eldor, Junior researcher, Laboratory of Elemental Analysis of Institute of General and Inorganic Chemistry of Uzbekistan Academy of Sciences

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    Rakhmatkariev Gairat,

    Dr in chemistry, Prof., Head of Laboratory of Elemental Analysis of Institute of General and Inorganic Chemistry of Uzbekistan Academy of Sciences;

    Rakhmatkarieva Feruza, Ph D., Researcher, Head of Laboratory of Elemental Analysis of Institute of General and Inorganic Chemistry of Uzbekistan Academy of Sciences

    Ergashev Oybek,

    Ph D., Teacher, Namangan Engineering-Technological Institute Ministry of the higher and secondary special education of the republic of Uzbekistan


    Abstract: Differential heats, isotherms, the differential entropies and thermokinetics ofbenzene adsorption in the zeolite LiY at 303K have been measured using the method of adsorption calo-rimetry. Differential molar entropy and free energy of adsorption were calculated. The isotherms of adsorption were quantitatively reproduced on the basis of three-term VOM theory. These data formed the basis for identifying the detaled mechanism of benzene adsorption in LiY zeolite.

    Keywords: Ion-molecular complexes, LiY zeolite, benzene, differential heats, isotherms, the differential entropies, thermokinetics, adsorption calorimetry.

    Introduction mechanism of adsorption of benzene in zeolite ofY

    Zeolite [1] is microporous crystals possessing wide type with exchangeable Li + cations. application in chemical and petrochemical industries Subjects and Methods. Adsorption studies

    as catalysts and sorbates [2; 3]. Method of adsorptive were carried out with zeolite Li Y. As adsorptives of

    calorimetry is widely used in our practice ensuring de- benzene molecule were selected. Adsorption-calo-

    tailed researches host-guest interaction in the systems rimetric method used in this paper provides a high-

    adsorbent-adsorbate in wide space equilibrium pres- precision molar thermodynamic characteristics of

    sure. The results these studies were confirmed such adsorption systems and through them to reveal the

    complementary methods as powder X-ray diffraction, mechanism of adsorption processes occurring in the

    NMR spectroscopy and computer modeling [4]. Be- adsorbent. As a calorimeter the microcalorimeter

    fore benzene adsorption was mainly studied in Na Tian-Calvet-type, with high accuracy and stability

    form zeolites type X and Y [5-7]. We were set a goal was used [11; 12].

    to reveal detailed mechanism ofbenzene adsorption in Results and discussion. Changing the dif-

    the zeolite LiY based on results energy investigations. ferential heat of adsorption (Qd) benzene in the

    Objective: to study isotherms and main ther- zeolite LiY depending on the amount of adsorp-

    modynamic characteristics of adsorption and the tion ^ -amount of benzene per 1/8 of the unit cell

    (C6H6 / (1/8) unit cell) or one supercages) shown in Fig. 1. The dashed line in the figure shows the heat of condensation of benzene AHv. The adsorption heats in ~ 2.3 times exceed the heat of benzene condensation. Change of the differential heats of adsorption is singular as well.

    Heats begin from 108 kJ / mol and reduced sharply to 73.5 kJ / mol at 0.21 C6H6 / (l / 8) unit cell, then double pass through a maximum, more pronounced in the range of adsorption, a 0,21-0.49 C6H6 / (1/8) unit cell and less pronounced 0,49-0,78 C6H6 / (1/8) unit cell. Further the heat are reduced wavy to 75.21 kJ / mol at ~ 2 C6H6 / (1/8) unit cell, then grow to a maximum of 82.28 kJ / mol at 4 ~ C6H6 / (1/8) unit cell.

    Entering into the cavity of the third and fourth molecules leads to an increase of the heat of adsorption due to the contribution to the total energy, the energy of interaction between adsorbate-adsorbate. Location four C6H6 / Li + complexes is close to the tet-rahedral and a cluster fills almost all the space supercages. The fifth entry of the molecule leads to a wavelike decrease ofheat at first insignificant, then sharply in the range of4.36-4.85 C6H6 / (1/8) unit cell.

    In accordance with the wavelike Qd it can be divided into the following sections: 0,78-1,41; 1,41-1,92; 1,92-2,44; 2,44-3,08, 3,08-3,73, 3,734,36 and 4,36-5,00 C6H6 / (1/8) unit cell, which complete curve and small segment in the range of 5,00 -5,18 C6H6 / (1/8) unit cell.Total LiY zeolite adsorbs 5.18 of benzene molecules per 1/8 unit cell or one supercages.

    On 1/8 unit cell investigated by us the zeolite there is an average of 6.87 cations of Li +. All of them, in accordance with [7; 8; 9], should be distributed HN on sodalite (SI position ', adjacent to the hexagonal ring that separates the sodalite cavity from the hexagonal prism) and supercages (SII position adjacent to the undivided surface of sodalite cavity). If the position SII, whose number is 4, fully settled by cations, the remaining 2.87 cations are distributed on positions SI ', whose number is also 4.

    So far sodalite cavity with diameter of the input six -membered oxygen window ~ 0.25 nm have not been available for a relatively large molecule of benzene. Therefore, we exclude from consideration of adsorption centers in these cavities. Consequently, adsorption mainly proceeds in Supercages. High-energy area (up to a = 0.21 C6H6 / (l / 8) unit cell) refers to adsorption on the cations of Li +, are in supercagess in SIII position '. These open positions are more accessible to the adsorbed molecules and therefore have the greatest energy of a specific interaction, reaching to llOkJ / mol.

    The ability of the adsorbed molecules in supercages to extract small size of the cations of Li + from sodalite cells, was shown by us in the adsorption of polar H2O and quadrupole CO2 molecules [10]. Two sec2ions 0,21-0,49 and 0,49-0,78C6H6 / (l / 8) unit cell at ~ 77 kJ / mol, we refer to benzene adsorption on the lithium cations are in the 4-membered oxygen rings ( SIII).

    A cation of Li +, located in SII positions due to the small size is immersed in the 6-membered oxygen ring. Therefore, the benzene molecule adsorbed on the cation of lithium in the SII position, can not be focused more favorably as cation and a negatively charged oxygen atoms forming 6-membered oxygen ring. After the adsorption of benzene on the Li + in the SIII 'position has begun its adsorption on the Li + in SIII position. The further mixed adsorption of C6H6 0.63 / (1/8) unit cell benzene occurs on lithium cations in the positions of the SII and SIII (0,78-1,41C6H6 / (1/8) unit cell).

    It is only two sections 1,41-1,92 1,92-2,44 and C6H6 / (1/8) unit cell by 0.5 C6H6 / (1/8) unit cell are responsible for the benzene adsorption exclusively on SII lithium cations. The rest of the section is per 0.64 C6H6 / (1/8) unit cell each reflects adsorption on the SIII and SII. If each of these sections to subtract a portion of responsible for adsorption on SII, 0,50 C6H6 / (1/8) unit cell, the residue corresponding to adsorption SIII, equals 0.144 C6H6 / (1/8) unit cell. Such sections are 5, therefore, within

    these sections adsorbed 0.72 C6H6 / (l / 8) unit cell (5 x 0.144 = 0.72). And 0.72 + 0.57 = 1.29 C6H6 / (1/8) unit cell is adsorbed just taking into account SIII on the second and third sections. With reference to adsorption on SII, 2.5 C6H6 / (1/8) unit

    cell (5 x 0.5 = 2.5) are adsorbed in accordance with the five sections in these centers and plus 1 C6H6 / (1/8) unit cell (2 by 0,5C6H6 / (l / 8) unit cell of5 and 6 sections) . A total of 33.5 C6H6 / (l / 8) unit cell adsorbed in the SII.

    Figure 1. The differential heat of benzene adsorption in the zeolite LiY at 303K. The horizontal dashed line is heat benzene condensation at 303K

    Figure 2. Benzene adsorption isotherm in the zeolite LiY at 303K

    Thus, at saturation of LiY zeolite cavities by 0.21C6H6 / (1/8) unit cell adsorbed on cations in the SIII ', 1,296 C6H6 / (1/8) unit cell adsorbed on SIII and 3,5 SII. From 6.87 of lithium cations per 1.8 unit cell in the adsorption process involved 5. In the last section, after adsorption of 4.36 C6H6 / (1/8) unit cell heat begins to decreas from 82.1 to 77.1 kJ / mol, as is usual at the end of the adsorption process. However, the redistribution of the adsorbed molecules to create more densely packed adsorbate molecules allow to decreased more 0,64 C6H6 / (1/8) unit cell, adsorption which leads to a sharp rise of heat of adsorption to the level of81.3 kJ / mol. Redistribution ofbenzene begins after adsorption of 4 C6H6 / (1/8) unit cell. In the issue of the redistribution, the fifth molecule of benzene per 1/8 unit cell is displaced to a new the center of W in the 12 -membered oxygen rings. The small "tail" on the curve Qd at culminating stage of

    A - experimental data A - estimating data by VOM

    benzene adsorption (a from 5 and 5.18 C6H6 / (1/8) unit cell with a heat falling from 61 to 40 kJ / mole) is determined by adsorption in mesopores.

    The adsorption isotherm was determined by volumetric method at a temperature of 303K. Control of adsorption equilibrium carefully performed with the thermo-kinetic curves. Figure 2 shows the adsorption isotherm (a) of benzene in the zeolite Li Y. Isotherm was built in semilogarithmic coordinates, allowing you to visually present the adsorption of a in the entire range of equilibrium pressures.

    There are identified the adsorption point, the blackout point processed VOM equation in Fig. 2. It is observed that a satisfactory agreement between the experimental and calculated points in the initial and final adsorption areas.

    The molar differential entropy of adsorption (ASd) of benzene in the zeolite LiY calculated by the

    Gibbs-Helmholtz equation of the isotherms and differential heats of adsorption [11-12] and is shown in Figure 3.The initial part of the curve rises from area of ​​the low and negative entropy (-125kJ / mol * K), pointing to a strong localization of benzene adsorbed on Li + cations in the open position of SIII ', then passes through a maximum (-30kJ / mol * K)


    a -10


    1 "40 1" 70


    * LOO -130

    Figure 3. The differential entropy of the benzene adsorption in the zeolite LiY at 303K. Entropy of liquid benzene is taken as zero. The horizontal

    dashed line - mean molar integral entropy

    It is interesting that, when N = 4,26 C6H6 / (1/8) unit cell entropy decrease sharply interrupted and the curve forms a step with a length of 0.4 C6H6 / (1/8) unit cell in the range of 4.26- 4.66 C6H6 / (1 / '8) unit cell at 92.6 J / mol * K. However, further the entropy decreases sharply up to 123.1J / mol * K at 4.9 C6H6 (/ 1/8) unit cell. The adsorption entropy confirms the data heats of adsorption indicating that in this area there is a redistribution of the benzene molecules benzene and formation of densely packed ofbenzene molecules. The curve sharply rises in the direction of liquid benzene entropy passing through a minimum. Mean molar integral of the entropy of adsorption close to entropy of solid benzene and is equal to -61.4 J / mol * K, which generally indicates the solidlike state of benzene molecules in the zeolite matrix.

    After two adsorption of C6H6 / (1/8) unit cell t is accelerated and equilibrium is established in av-

    and at first slowly up to N = 2 C6H6 / (1/8) unit cell, then decreases sharply and at 4.9 C6H6 / (1/8) unit cell it becomes two times lower than the solid benzene entropy, is123 J / mol * K), which demonstrates the growing inhibition of translational and rotational motions of benzene molecules with the gradual filling of the adsorption space.

    0 1 2 3 4 5 N, C6H6 / (l / 8) u.c.

    Figure 4. The set-time of the adsorption equilibrium, depending on the size of the adsorption of benzene in the zeolite LiY at 303K

    erage for 2-2.5 hours. Accelerate of the adsorption smoothes the waves, but if the rest of the curve divided into sections from the maximum to the maximum, that is got a section with length of 1.0 C6H6 / (1/8) unit cell and three at 0.63 C6H6 / ( 1/8) unit cell. The first section corresponds to the adsorption of benzene on the Li + in the SII positions (2 by 0.50 C6H6 / (1/8) unit cell) and three sections reflect adsorption on mixed positions of SIII and SII (at 0.63 C6H6 / (1 / 8) unit cell). Reducing heat in the adsorption is more than 4 C6H6 / (1/8) unit cell. It leads to accelerate the process, but benzene redistribution and the appearance of new centers dramatically slows down and the curve t passes through maximum at 4.9 and 4.98 unit cell.

    The study shows that, along with the isotherm and differential heats of adsorption, entropy and thermo kinetics of adsorption reflects the specifics

    of the formation of the ion / molecular complexes in the zeolite matrix are strongly localized and their

    in the zeolite matrix. The mechanism of adsorption, state closes to solidlike. The migration of cations

    established on the basis of the heats of adsorption from the sodalite cavities in the supercages flows

    and isotherms, fully confirmed. Benzene molecules with a strong slowdown in the adsorption process.


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