N 2 and CO 2 Adsorption by Soils with High Kaolinite Content from San Juan Amecac , Puebla , México

Carbon dioxide (CO2) is considered one of the most important greenhouse gases in the study of climate change. CO2 adsorption was studied using the gas chromatography technique, while the Freundlich and Langmuir adsorption models were employed for processing isotherm data in the temperature range of 473–573 K. The isosteric heat of adsorption was calculated from the Clausius–Clapeyron equation. Moreover, the thermodynamic properties ∆G, ∆U, and ∆S were evaluated from the adsorption isotherms of Langmuir using the Van’t Hoff Equation. The four soil samples were recollected from San Juan Amecac, Puebla, Mexico, and their morphologies were investigated through X-ray diffraction (XRD) and N2 adsorption at 77 K. The SJA4 soil has a crystalline Kaolinite phase, which is one of its non-metallic raw materials, and N2 isotherms allowed for the determination of pore size distributions and specific surface areas of soil samples. The Barrett–Joyner–Halenda (BJH) distribution of pore diameters was bimodal with peaks at 1.04 and 3.7 nm, respectively. CO2 adsorption showed that the SJA1 soil afforded a higher amount of adsorbed CO2 in the temperature range from 453 to 573 K followed by SJA4 and finally SJA2, classifying this process as exothermic physisorption.


Introduction
Nowadays.one problem that affects our society is the treatment of greenhouse gases, namely, the enforcement of a separation, capture, and storage that is environmentally friendly and economically viable [1], particularly CO 2 given that this gas is becoming increasingly important in the future of the world economy [2].Carbon dioxide (CO 2 ) is considered one of the main greenhouse gases producing global warming.Hence, the adsorption processes require the development of new technologies for the effective adsorption and storage of large amounts of CO 2 [3].Carbon sequestration means capturing CO 2 from the atmosphere or from anthropogenically produced large-scale mixtures of effluent gases exhausted from industries.On the other hand, carbon capture involves the separation of this compound from a gas mixture and to adsorb (concentrate) it on the surface of assorted substrates.CO 2 is particularly important for its effect on the climate conditions of the planet, since it is a long-standing gas that remains active in the atmosphere for a long time.Once the CO 2 reaches the atmosphere, it reacts immediately with the short-lived gases of the biosphere and surface ocean, and the remaining CO 2 remains for hundreds of years to be captured and converted amid the deep ocean and the terrestrial biosphere [4].Between 2000 and 2006, CO 2 sink by land accounted for about 0.30 of the total airborne fraction; while the ocean sink accounted for 0.24 and the atmospheric accumulation of the gas amounted to 0.45 [5].
A special feature of contaminant sorption by soils is that it is a multiple reaction phenomenon.Most natural soils are inherently heterogeneous, including the microscopic-scale soils, due to the fact that their composition and framework are variable at interparticle and intraparticle scale [6].The ideal adsorption of molecules in pore systems depends on the pore character in relation to its shape, size, and chemical nature [7].Any solid can fix or adsorb on the surface, molecules, atoms, or ions.In the area of gas-solid interfaces, the use of sorption isotherms is widely spread to determine the adsorption capacity of the substrate [8].
Soils are considered complex systems, a mixture primarily composed of organic matter and mineral material such as quartz and clay; quartz is completely inert, organic matter, and clays expand when exposed to water and other fluids, thereby increasing the surface area and adsorption capacity.Carbon dioxide capture and storing (CCS) occur in three steps: CO 2 is separated from other industrial mixture gases when it is captured at its source, CO 2 is stored away in the atmosphere in a compressed form to a suitable storage location, i.e., underground, the deep ocean, or in some mineral compounds.During the last few years, certain commercial projects have already been developed for CO 2 storage in underground geological formations, such as oil and gas recovery and abstraction projects [9].
The presence of kaolinite clays in earth soils can strongly affect the mass-transfer processes occurring in natural environments [10].Kaolinite is a mineral solid that consists of tetrahedral silicate sheets and octahedral hydroxide sheets in a 1:1 proportion [11].The mass transfer that takes place in the environment process can be significantly affected by the presence of kaolinite clays in soils.Usually, if pollutants are originated in different sources such as domestic sewage, sludge, and other solid waste, and these are poured on the earth surface, the mineral particles of soils react with them.In this way, the presence of clay minerals in soils acts as pollutant collectors improving the environment [12].
The amount of CO 2 adsorbed by adsorbents is dependent on temperature, CO 2 partial pressure, and the potential interaction between CO 2 and the adsorbent itself [13], as well as the topography of the adsorbent surface.Adsorption is considered one of the most promising physical processes used by new technologies to efficiently capture CO 2 from flue gases [3].Adsorption occurs from interactions among the individual atoms, ions, and molecules of an adsorbate and those present on the adsorbent surface.The process involves the separation of a substance from one phase and its accumulation at the surface of another [14].
Adsorption occurs from interactions between the accumulation of individual atoms and molecules of the adsorbate and the surface of the adsorbent.It must separate and accumulate a fluid phase on a solid surface.It is necessary to know the porous system of solids to understand most processes that are carried out on them, such as nutrient dynamics and adsorption phenomena.Environmental chemistry has been of significant importance since organic and inorganic adsorption includes the transport and activity of pollutants in soils, sediments, and water; consequently, it affects the bioavailability, biodegradability, and ultimate destination of organic waste [15,16].
Several adsorption processes are frequently used in the industry, e.g., pressure swing adsorption (PSA) and thermal or temperature swing adsorption (TSA) [16].The main contrast concerning these processes is that, in PSA, the pressure of the adsorption bed is reduced; on the other hand, in TSA processes, the temperature increases while pressure remains fairly constant.Zeolites are the most common materials used as adsorbents in the study of CO 2 capture by PSA and TSA technologies [17].
The purpose of this work consisted in the evaluation of the total amount of CO 2 adsorbed on four kinds of kaolinite clay soils [18].This determination can help to establish the efficacy toward CO 2 capture by actual soils.In this respect, kaolinite soils were chosen for this CO 2 adsorption study [19] by virtue of its being the most widespread clay mineral in earth, since entire clay deposits can be composed of this mineral.This kind of soil contains a high amount of colloidal particles and becomes viscous when wet.As a result, the capture of CO 2 by kaolinitic soils should be an interesting subject of research, since, for instance, once captured, CO 2 can remain in storage conditions [20], awaiting further transformation into other compounds.CO 2 adsorption is one of the best methods for measuring the microporosity of a given material.However, the fact that micropores are the smallest of voids, with pore widths less than 2 nm, makes the desorption process of the adsorbate difficult.On the one hand, zeolites are one of the best known microporous substrates and are very useful for performing CO 2 capture.On the other hand, mesoporous solids (soils included) are sometimes preferred since the transport properties are better qualified for a faster uptake and liberation of gases (CO 2 included).

Materials and Methods
Four soil samples were collected in the locality of San Juan Amecac, Puebla, Mexico.The geographical location of these soils is 18 ˝50 1 24 11 N and 98 ˝39 1 23 11 W.In each sampling site, of an area of approximately 550 m 2 , 5 simple samples of about 1.5 kg were taken and mixed together to form a compound specimen of 7.5 kg in total, of which 1 kg was taken for characterization purposes.This same sampling process was repeated for each soil, and every 1 kg specimen was then dried under sunlight and sieved at a mesh size of 0.3-0.18mm.Samples were labeled as SJA1, SJA2, SJA3 and SJA4, respectively.

X-Ray Diffraction (XRD) and Energy-Dispersive X-Ray Spectroscopy (EDS)
XRD patterns were determined through a Bruker D8 diffractometer using nickel-filtered Cu Kα (λ = 0.154 nm) radiation operated at 40 kV and 30 mA [8].The crystalline phases were identified by comparing the diffraction patterns obtained with the database of the International Centre for Diffraction Data (ICDD) (JCPDS-ICDD, 2000).The samples were scanned within the range of 5 ˝-60 2θ with a step size of 0.03 2θ and a counting time of 2 s.In turn, EDS (Energy-Dispersive X-Ray Spectroscopy) analyses were performed in a JEOL JSM-6610LV instrument (Jeol Ltd., Tokyo, Japan) equipped with a tungsten filament electron detector operated at 30 kV.This allowed for the obtainment of the elemental composition at the nanoscopic level.

N 2 Adsorption
N 2 adsorption isotherms were carried out at the boiling point of liquid nitrogen (76 K) at an altitude of 2200 m in Puebla City, México (2200 m above mean sea level AMSL), using an automatic volumetric adsorption instrument (Quantachrome AutoSorb-1C, Quantachrome Instruments, Boynton Beach, FL, USA).This equipment includes, in addition to the mechanical pump, a turbomolecular pump and a low-pressure transducer, which is located close to the measuring adsorption cell.N 2 adsorption isotherms were evaluated at the relative pressure range (p/p 0 ) of 10 ´6-1.
Where p is the adsorption pressure and p 0 is the saturation pressure at 76 K of N 2 .A specific mesh size of 0.250 mm was used for all samples.Before carrying out the experimental run, the samples were degassed via thermal treatments at 623 K for 20 h under a vacuum of 10 ´5 Torr [21].Pore size distribution (PSD) was calculated by the Barrett-Joyner-Halenda (BJH) method, applied to the N 2 adsorption boundary isotherm.

CO 2 Adsorption
The adsorption properties of the soils were further evaluated by means of a GOW-MAC 350 gas chromatograph (GOW-MAC Instrument Co., Bethlehem, PA, USA) provided with a thermal conductivity detector (TCD).Soil samples were packed into the stainless steel columns with a diameter of 5 mm and a length of 50 cm.Soils were outgassed in situ with a helium flow as carrier gas for 3 h at 573 K. Retention times were measured within the temperature range of 573-453 K, and from these the adsorption isotherms were determined through the chromatographic technique (i.e., the GC peak maxima method) [22].
Structural changes of the soil specimens begin with their endothermic dehydroxylation to metastable metakaolinite phases, occurring from 723 to 973 K [23].

Data Analysis
Mathematical models of Freundlich and Langmuir were using for the analysis of the CO 2 isotherm data.
Freundlich's isotherm linear form is as follows: where a is the amount of CO 2 adsorbed by the soil samples expressed in mmoles at pressure p, followed by K F , which is the Freundlich adsorption constant; and n is an exponential factor.In this approach, the Henry constant (K H ) were evaluated for the soils under study according to the following expression: Langmuir equation in its linear form is given as where a m is the monolayer capacity, and K L is the Langmuir adsorption constant.

Crystalline Phases and Chemical Composition
The XRD (X-ray diffraction) patterns are shown in Figure 1, in which the presence of three crystalline phases has been noted: quartz (Joint Committee on Powder Diffraction Standards, JCPDS card 03-065-0466), albite (JCPDS card 01-071-1150), and kaolinite (JCPDS card 00-001-0527).The sample SJA4 showed a large presence of mineral phases followed by the SJA3, SJA1 and SJA2 materials.The characteristic signals of kaolinite are located at 2θ: 12.04 ˝, 20.09 ˝, 23.7 ˝and 35.65 ˝.This behavior of the obtained XRD patterns are similar to those previously reported [24].
The chemical composition of kaolinite indicates Al 2 Si 2 O 5 (OH) 4 structural formula with the following weight contents of 46% SiO 2 , 39.5% AlO 3 , and 14.0% H 2 O [25].Nevertheless, in natural kaolinites proceeding from soils, this composition is rarely found due to the relatively high amount of impurities, generally present as mixtures of minerals, metal oxides, and organic materials.The chemical compositions of the soil samples studied are shown in Table 1.

N2 Adsorption
The textural parameters of the samples were determined from the N2 adsorption isotherms of at 76 K (Figure 2).

N 2 Adsorption
The textural parameters of the samples were determined from the N 2 adsorption isotherms of at 76 K (Figure 2).

N2 Adsorption
The textural parameters of the samples were determined from the N2 adsorption isotherms of at 76 K (Figure 2).
The initial part (p/p 0 = 0.1-0.4) of these isotherms can be attributed to the formation of multilayer formation, since it follows the course corresponding to the IUPAC Type II isotherm.Therefore, when N 2 molecules are deposited on mesoporous soils, there surges a competition among the fluids invading the substrate; on the other hand, the intensity of this invasion will be a function of the amount of pores of given sizes and of their surface heterogeneity [21].In these isotherms, the adsorption is carried out on the pore walls and is similar to the classic way observed in real porous solids with structures in which mesopores dominate.
Based on the shape of the isotherms (IUPAC Type IV and IUPAC type H3 hysteresis loops) that present this type of soil, the Brunauer-Emmet-Teller equation (BET) was satisfactorily applied.The values obtained of the BET constants (C BET ) are similar for SJA1, SJA2, and SJA4, whereas the C BET for the SJA3 soil is the smallest of all since the corresponding isotherm shows no definite knee (i.e., the monolayer adsorption is not as definite as with the other samples and the specific surface area is also the smallest of all).Additionally, a negative C BET value indicates a low adsorption energy for the same reason for which the transition from the monolayer adsorption to the multilayer formation is not sharp.All C BET values are higher than unity, something that confirms the absence of micropores.In the same table, by comparison, the values of the pore total volumes, V Σ , are listed and evaluated according to the Gurvitsch rule at p/p 0 = 0.95.The highest values of the specific surface, the total volume, and the diameter are obtained in the sample SJA4 (Table 2).PSD was calculated from the N 2 adsorption isotherms through BJH analysis (Figure 3), and the results indicated that Sample SJA4 produces bimodal distributions with pore sizes of around 1.043 and 3.790 nm, and SJA3 also shows bimodal distribution but with 3.3-and 5.2-nm values.However, the intensity of these signals depends on the content of kaolinite in soils.In the case of SJA1 and SJA2, unimodal distributions («3.6 nm) are produced.According to the size, they are called mesopores that exist in the external area of the soils studied.
The SJA3 sample was found to be poorly consolidated because, at temperatures from 523 to 573 K, it is compacted, and gases such as He and CO 2 cannot pass through the chromatography column, impeding the obtainment of any results.Thus, it was not adapted to the experimental conditions of adsorption of 523-573 K and 517-1034 mm Hg, and, therefore, only the chromatography results of Samples SJA1, SJA2 and SJA4 are shown.The initial part (p/p 0 = 0.1-0.4) of these isotherms can be attributed to the formation of multilayer formation, since it follows the course corresponding to the IUPAC Type II isotherm.Therefore, when N2 molecules are deposited on mesoporous soils, there surges a competition among the fluids invading the substrate; on the other hand, the intensity of this invasion will be a function of the amount of pores of given sizes and of their surface heterogeneity [21].In these isotherms, the adsorption is carried out on the pore walls and is similar to the classic way observed in real porous solids with structures in which mesopores dominate.
Based on the shape of the isotherms (IUPAC Type IV and IUPAC type H3 hysteresis loops) that present this type of soil, the Brunauer-Emmet-Teller equation (BET) was satisfactorily applied.The values obtained of the BET constants (CBET) are similar for SJA1, SJA2, and SJA4, whereas the CBET for the SJA3 soil is the smallest of all since the corresponding isotherm shows no definite knee (i.e., the monolayer adsorption is not as definite as with the other samples and the specific surface area is also the smallest of all).Additionally, a negative CBET value indicates a low adsorption energy for the same reason for which the transition from the monolayer adsorption to the multilayer formation is not sharp.All CBET values are higher than unity, something that confirms the absence of micropores.In the same table, by comparison, the values of the pore total volumes, VΣ, are listed and evaluated according to the Gurvitsch rule at p/p 0 = 0.95.The highest values of the specific surface, the total volume, and the diameter are obtained in the sample SJA4 (Table 2).PSD was calculated from the N2 adsorption isotherms through BJH analysis (Figure 3), and the results indicated that Sample SJA4 produces bimodal distributions with pore sizes of around 1.043 and 3.790 nm, and SJA3 also shows bimodal distribution but with 3.3-and 5.2-nm values.However, the intensity of these signals depends on the content of kaolinite in soils.In the case of SJA1 and SJA2, unimodal distributions (≈3.6 nm) are produced.According to the size, they are called mesopores that exist in the external area of the soils studied.
The SJA3 sample was found to be poorly consolidated because, at temperatures from 523 to 573 K, it is compacted, and gases such as He and CO2 cannot pass through the chromatography column, impeding the obtainment of any results.Thus, it was not adapted to the experimental conditions of adsorption of 523-573 K and 517-1034 mm Hg, and, therefore, only the chromatography results of Samples SJA1, SJA2 and SJA4 are shown.

CO2 Adsorption
The adsorptions isotherms of CO2 are presented in Figure 4.The nonlinear shape of CO2 isotherms is more likely to be associated with interactions of CO2 with high-energy adsorption sites on mineral surfaces [5].Sample SJA2 presents the lowest adsorption capacity with maximum values of 0.055 mmol/g at higher pressures in comparison with the other soil samples, while Sample SJA1 presents the highest quantity of substance adsorbed with 0.106 mmol/g.These results are higher than those obtained either for natural clinoptilolites (zeolites) or for similar specimens treated chemically, with values of the total adsorbed CO2 mass amounting to 0.06-0.09mmol/g [21].The CO2 retention at 298 K in HDP-montmorillonite (clay) (0.038-0.06 mmol/g) [26] and Skardon River kaolinite (0.056 mmol/g) [27] also have different operation conditions from those proposed in the present research.At the same time, these are all lower than those previously reported in activated carbons [16,28], zeolites [2], and synthetic materials [29].Pore diameter (nm)

CO 2 Adsorption
The adsorptions isotherms of CO 2 are presented in Figure 4.The nonlinear shape of CO 2 isotherms is more likely to be associated with interactions of CO 2 with high-energy adsorption sites on mineral surfaces [5].Sample SJA2 presents the lowest adsorption capacity with maximum values of 0.055 mmol/g at higher pressures in comparison with the other soil samples, while Sample SJA1 presents the highest quantity of substance adsorbed with 0.106 mmol/g.These results are higher than those obtained either for natural clinoptilolites (zeolites) or for similar specimens treated chemically, with values of the total adsorbed CO 2 mass amounting to 0.06-0.09mmol/g [21].The CO 2 retention at 298 K in HDP-montmorillonite (clay) (0.038-0.06 mmol/g) [26] and Skardon River kaolinite (0.056 mmol/g) [27] also have different operation conditions from those proposed in the present research.At the same time, these are all lower than those previously reported in activated carbons [16,28], zeolites [2], and synthetic materials [29].

CO2 Adsorption
The adsorptions isotherms of CO2 are presented in Figure 4.The nonlinear shape of CO2 isotherms is more likely to be associated with interactions of CO2 with high-energy adsorption sites on mineral surfaces [5].Sample SJA2 presents the lowest adsorption capacity with maximum values of 0.055 mmol/g at higher pressures in comparison with the other soil samples, while Sample SJA1 presents the highest quantity of substance adsorbed with 0.106 mmol/g.These results are higher than those obtained either for natural clinoptilolites (zeolites) or for similar specimens treated chemically, with values of the total adsorbed CO2 mass amounting to 0.06-0.09mmol/g [21].The CO2 retention at 298 K in HDP-montmorillonite (clay) (0.038-0.06 mmol/g) [26] and Skardon River kaolinite (0.056 mmol/g) [27] also have different operation conditions from those proposed in the present research.At the same time, these are all lower than those previously reported in activated carbons [16,28], zeolites [2], and synthetic materials [29].The experimental points of the CO 2 isotherms estimated in the interval of 573 to 473 K were evaluated and favorably described for the Freundlich equation in their linear coordinates.It is shown in Figure 5a, with the determination pertinent to the adsorption parameters indicating the heterogeneity in the adsorption sites [30], with correlated coefficients of 0.996 to 0.999.This effect was not observed when the Langmuir equation was applied in these conditions.
The experimental points of the CO2 isotherms estimated in the interval of 573 to 473 K were evaluated and favorably described for the Freundlich equation in their linear coordinates.It is shown in Figure 5a, with the determination pertinent to the adsorption parameters indicating the heterogeneity in the adsorption sites [30], with correlated coefficients of 0.996 to 0.999.This effect was not observed when the Langmuir equation was applied in these conditions.The values of the Freundlich constants (KF) and n, the monolayer adsorption capacity (am), are reported in Table 2.The Langmuir equation considers the interaction of unimolecular unions, and the Freundlich equation is an interactive equation of the adsorbed substance with the adsorbent, which can be related to the element disposition in the soil [22].The monolayer adsorption capacity (am) and the Langmuir constant (KL) depend on temperature, deriving from the Langmuir plots (Figure 5b), as shown in Table 3.The isosteric adsorption heat qst (kJ•mol −1 ) in low quantities of an adsorbed substance was evaluated from the data of the adsorption isotherms through the Clausius-Clapeyron equation: where T and p are the temperature and pressure at equilibrium.In this study, the CO2 isosteric heats were calculated from the analysis of the linear regression of the graphic p vs. 1/T using the original equilibrium isotherms data [28].This technique is used at relatively high temperatures as well as for very short times of contact [31] due to the presence of an inactivated diffusion process.The diffusion of CO2 is hindered by the presence of steric barriers across mesoporous channels; therefore, higher The values of the Freundlich constants (K F ) and n, the monolayer adsorption capacity (am), are reported in Table 2.The Langmuir equation considers the interaction of unimolecular unions, and the Freundlich equation is an interactive equation of the adsorbed substance with the adsorbent, which can be related to the element disposition in the soil [22].The monolayer adsorption capacity (am) and the Langmuir constant (K L ) depend on temperature, deriving from the Langmuir plots (Figure 5b), as shown in Table 3.The isosteric adsorption heat q st (kJ¨mol ´1) in low quantities of an adsorbed substance was evaluated from the data of the adsorption isotherms through the Clausius-Clapeyron equation: where T and p are the temperature and pressure at equilibrium.In this study, the CO 2 isosteric heats were calculated from the analysis of the linear regression of the graphic p vs. 1/T using the original equilibrium isotherms data [28].This technique is used at relatively high temperatures as well as for very short times of contact [31] due to the presence of an inactivated diffusion process.The diffusion of CO 2 is hindered by the presence of steric barriers across mesoporous channels; therefore, higher temperatures are required to further permeate these capillaries into the pores beyond [32].The adsorption isosteric heat shows the energy of interaction among the adsorbate-adsorbent and the adsorbate-adsorbate that take place in the adsorption system.The behavior of the isosteric systems in the studied soils are shown in Figure 6 in which the decline in the isotherm heat of adsorption, in a width interval of the cover surface, can be observed.temperatures are required to further permeate these capillaries into the pores beyond [32].The adsorption isosteric heat shows the energy of interaction among the adsorbate-adsorbent and the adsorbate-adsorbate that take place in the adsorption system.The behavior of the isosteric systems in the studied soils are shown in Figure 6 in which the decline in the isotherm heat of adsorption, in a width interval of the cover surface, can be observed.This behavior is frequent on non-uniform surfaces, even when there exist specific adsorbentadsorbate interactions.In general, in low adsorbed quantities, the isosteric heat magnitude decreases with the addition of adsorbed substance.This behavior is common in adsorbents that have heterogeneous adsorption sites, as in the case of the soil [8].
The thermodynamics parameters in the CO2 adsorption were evaluated from the data of the adsorption isotherms of Langmuir using the Van't Hoff Equation [33] using the following relations: where ∆G is the free energy change of Gibbs, that is, the same as the isosteric heat under isothermal conditions, leaving behind the gas imperfections, ∆H is the enthalpy change, and ∆S is the entropy change of the adsorption process.The values of the thermodynamic parameters for the adsorption of CO2 are presented in Table 4. There, negative values of ∆G are observed, confirming the viability and spontaneous nature of the adsorption process, while the negative values in ∆H indicate that the adsorption phenomenon is exothermic and the positive value of ∆S confirms the affinity [17] of the kaolinite soils toward CO2.This behavior is frequent on non-uniform surfaces, even when there exist specific adsorbent-adsorbate interactions.In general, in low adsorbed quantities, the isosteric heat magnitude decreases with the addition of adsorbed substance.This behavior is common in adsorbents that have heterogeneous adsorption sites, as in the case of the soil [8].
The thermodynamics parameters in the CO 2 adsorption were evaluated from the data of the adsorption isotherms of Langmuir using the Van't Hoff Equation [33] using the following relations: ∆G " ´RTln p 0 p ; (5) where ∆G is the free energy change of Gibbs, that is, the same as the isosteric heat under isothermal conditions, leaving behind the gas imperfections, ∆H is the enthalpy change, and ∆S is the entropy change of the adsorption process.The values of the thermodynamic parameters for the adsorption of CO 2 are presented in Table 4. There, negative values of ∆G are observed, confirming the viability and spontaneous nature of the adsorption process, while the negative values in ∆H indicate that the adsorption phenomenon is exothermic and the positive value of ∆S confirms the affinity [17] of the kaolinite soils toward CO 2 .

Conclusions
The characterization of soils with high kaolinite content was satisfactorily performed through several experimental techniques; the XRD results show that the SJA4 soil contains the crystalline kaolinite phase, while, according to N 2 adsorption, this same sample attained the highest specific surface area and the widest pore size distribution.
The characterization by N 2 adsorption demonstrated the structural heterogeneity of the soil samples studied.For this, it is convenient to conduct studies on pore size distribution.It is necessary not to consider a specific mechanism, but to illustrate the difference between the filling of meso-and macropore surfaces in adsorption processes.
According to the adsorption parameters calculated in this work, CO 2 was favorably adsorbed mainly on the SJA1 sample, which attained the highest values of CO 2 adsorption.This process is physisorption, which can be confirmed by the obtained values of the isosteric heat of adsorption.The adsorption isotherms obtained experimentally were adjusted to the adsorption model of Freundlich, which confirmed the soil heterogeneity and CO 2 multilayer filling for all samples.
However, the transformation of trapped CO 2 into other compounds, such as alcohols, ketones, acids, and aldehydes, seems to have a better end result.After secondary oil recovery, CO 2 can remain buried in the tiny spaces between grains of sand where oil was previously held.CO 2 capture by soils is an important option because of the availability of these substrates.

Figure 3 .
Figure 3. Pore size distribution of soils samples.

Figure 3 .
Figure 3. Pore size distribution of soils samples.

Figure 3 .
Figure 3. Pore size distribution of soils samples.

Figure 5 .
Figure 5. Linear fit of (a) the Freundlich model and (b) the Langmuir model for the CO2 adsorption in soils.

Figure 5 .
Figure 5. Linear fit of (a) the Freundlich model and (b) the Langmuir model for the CO 2 adsorption in soils.

Table 1 .
Chemical composition of soil samples.

Table 1 .
Chemical composition of soil samples.

Table 1 .
Chemical composition of soil samples.

Table 3 .
Freundlich and Langmuir parameters for the adsorption of CO2 in soils samples with correlation coefficients.

Table 3 .
Freundlich and Langmuir parameters for the adsorption of CO 2 in soils samples with correlation coefficients.