The specific surface area of synthesized supported nanocatalysts were measured by volumetric method, using BET isotherm model. The BET surface area of the supported nanocatalysts obtained are presented in Table 1. The specific surface area of SiO2 obtained from serpentines varies within the range of 230–280 m2/g. The specific surface area of Pt/SiO2 was 250 m2/g, 200 m2/g for Pt/Al2O3, 40 m2/g for Pt/kaolinite. After swelling with DMSO, BET analysis revealed a decrease in the surface area (from 40 m2/g to 2.05 m2/g). The increase in specific Pt surface area is probably caused to close the porosity of particle size of support material. XRD patterns of Pt/Al2O3 and Pt/SiO2 nanocatalysts and Al2O3, SiO2 catalyst supports are presented in Fig. 1(a) and 1(b), respectively. The reflections observed in the XRPD patterns indicate the existence of following components: Al2O3, SiO2, Pt. The characteristic reflections (Fig. 1(a) and Fig. 1(b)) of Pt observed at ~ 40.81, 47.14, 68.65 and 82.21o. In the XRPD pattern of γ-Al2O3 low intensity peaks at ~ 37.51, 46.6 and 67.45o are observed. SiO2 support obtained from serpentines was found to be amorphous, as a broad peak appears in the SiO2 sample (Fig. 1(a)). Figure 1(c) and Fig. 1(d) represent XRD patterns of Pt/kaolinite and Pt/kaolinite/DMSO nanocatalysts, respectively. The reflections observed in the XRD patterns are mainly consist of kaolinite, rutile impurities and small amounts of illite. Displacement of the reflections associated to the XRD basal distance d001 in kaolinite (7.18 to 11.26 Å), is coherent with a monolayer intercalation of DMSO molecules (Fig. 1(c, d)).
Table 1
BET surface area and composition of supports and nanocatalysts
Supports/nanocatalysts
|
BET surface area, m2/g
|
Pt loading, wt.%
|
SiO2
|
230–280
|
-
|
Al2O3
|
250
|
-
|
Kaolinite
|
19
|
-
|
Pt/SiO2
|
250
|
1
|
Pt/Al2O3
|
200
|
1
|
Pt/kaolinite
|
40
|
1
|
Pt/kaolinite/DMSO
|
2.05
|
1
|
To study the role of DMSO in the process of increasing the interlayer space of kaolinite the adsorption of DMSO on the surface of kaolinite and Al2O3 was studied using FTIR spectroscopy. The adsorption of the first portions of DMSO leads to decrease the intensity of the absorption band of kaolinite surface hydroxyl groups. The valence vibrations of C-H groups appear in the spectrum which indicates the presence of DMSO on the surface. To record S = O region (1100 − 1000 cm− 1) DMSO adsorption was performed on the surface of Al2O3. In the gas state the S = O region of DMSO is characterized by an absorption band at 1104 cm− 1 and a shoulder at 1040 cm− 1 (Fig. 2). In the liquid state FTIR of DMSO is characterized by an absorption band at 1054 cm− 1. It should be noted that kaolinite is identified by two absorption bands at 3695 and 3659 cm− 1 produced by vibrations of the inner-surface hydroxyl groups of kaolinite. The absorption bands observable at 3538 and 3502 cm− 1 can be assigned to the kaolinite stretching frequencies of inner-surface hydroxyls (Fig. 3a). The absorption band observable at 1121 cm− 1 corresponds to Si-O bond stretching vibrations. This fact indicates interaction between DMSO and the Si-O surface of kaolinite. The peak at 792 cm− 1 attributed to out of phase stretching of Al-OH tends to be weaken, and the peak at 687 cm− 1 describes Al-OH symmetric vibration (Fig. 3b). These IR peaks detail the bonding evolutions of hydroxyl groups at the inner surface of kaolinite upon DMSO intercalation, which leads to strong hydrogen bonds formation between the guest, DMSO molecules, and Al-OH of kaolinite host with and without hydration. Moreover, the IR spectra suggest that the Si-O band of kaolinite is only significantly impacted for DMSO intercalation in the presence of water. The vibration frequency of S = O group decreases from 1104 cm− 1 to 1060 cm− 1.
As the concentration of adsorbed DMSO increases the intensity of absorption band at 1104 cm− 1 increases as well, and the rotational deformation of oscillation frequencies of CH3 groups which is present in the liquid state (954 cm− 1 and 932 cm− 1), does not observed in the adsorbed state.
The SEM micrographs of supports and the synthesized nanocatalysts are presented in Fig. 4. The SEM micrographs of the synthesized Pt/SiO2 demonstrate some structural changes when loading on 1% platinum. According to the SEM analysis of the synthesized Pt/γ-Al2O3 nanocatalyst does not show structural changes when loading on 1% platinum.
SEM images (Fig. 4a, b, c, d) show that the sizes of Pt particles are different. Strong interaction between Pt and the γ-Al2O3 support is not observed, but in the case of Pt/SiO2 a strong interaction can take place. As the temperature increases, C1-C3 hydrocarbons are formed (Fig. 5). At 500–523 K n-heptane conversion on Pt/Al2O3 catalyst reaches about 65% (Fig. 6a). At 500–523 K n-heptane conversion on Pt/SiO2 and Pd/SiO2 catalysts are inferior in their activity to corresponding catalysts deposited on Al2O3 (Fig. 6a, b). However, the formation of isomeric products is observed on these catalysts. An increase in temperature leads to decrease in isomerization selectivity and an increase in the number of cleavage products.
The conversion of n-heptane on Pt/kaolinite and Pt/kaolinite/DMSO catalysts was studied. Increasing the temperature leads to an increase of n-heptane conversion and at 430 K n-heptane conversion on Pt/kaolinite/DMSO catalyst reaches 50% and at 480 K the highest 63% of n-heptane conversion is observed, and an increase in selectivity is observed (Fig. 7) as well. This fact is probably due to the large dispersity of Pt that occurs in the nanosized cavities of kaolinite.
The enthalpy of soaking (ΔsH) for kaolinite, Al2O3 and SiO2 with H2O, DMSO and DMSO + H2O (1:1 v/v ratio) solvents are determined using Calve type DAC-1-1 differential automatic microcalorimeter, and obtained results are presented in Table 2. The values of ΔsH for all samples in water are lower compared to H2O + DMSO binary solvent and pure DMSO. These thermal effects in the presence of DMSO could be explained by the formation and penetration of DMSO-H2O associates of different composition in the interlayer space of catalysts. When soaking with DMSO, this tendency could be probably due to the self-associated structure and penetration of DMSO associates into the interlayer space of catalysts.
Table 2
The values of enthalpy of soaking for kaolinite, Al2O3 and SiO2
Support
|
H2O
|
1H2O:1DMSO
(v/v)
ΔsH, J/g
|
DMSO
|
Kaolinite
|
-1.94
|
-3.34
|
-4.94
|
Al2O3
|
-2.86
|
-3.31
|
-5.33
|
SiO2
|
-3.14
|
-2.67
|
-4.87
|