# A Simple Method of Preparation of High Silica Zeolite Y and Its Performance in the Catalytic Cracking of Cumene

Authors: Zhanjun Liu; Chenxi Shi; Dan Wu; Shixuan He; Bo Ren
Journal: Journal of Nanotechnology
 (2016)

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## Abstract

A series of high silicon zeolites Y were prepared through direct synthetic method by using silica sol as the silicon source and sodium aluminate as the aluminum source. The effects of alkalinity and crystallization time of the process of synthesis were investigated. To separately reveal the crystalline structure, element content, morphology, and surface areas, the as-synthesized zeolite Y was characterized by powder X-ray diffraction (XRD), X-ray fluorescence (XRF), scanning electron microscopy (SEM), and N2 adsorption-desorption isotherms (BET). The results show the as-synthesized zeolite Y with high relative crystallization and uniform morphology; the SiO2/Al2O3 ratio was about 4.54~6.46. For an application, the zeolite cracking activity was studied with cumene as the probe molecules.


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## Body

## 1. Introduction

Zeolites are an important class of crystalline aluminosilicates materials with open-framework structures, and they have been widely used as separations, ion exchange, and acidic catalysts for size and shape selective catalytic reactions by molecular-sized microporosity [1–3]. The synthetic zeolites microporous crystalline solids have been produced in number of industrial scale processes for many years, and the zeolite Y is highly versatile molecular sieve from the Faujasite family with the three-dimensional pore structure and the pore diameter is about 0.74 nm [4, 5]. Although many other porous materials have emerged, the zeolite Y continues to keep the most popular pyrolysis catalyst in the international field because of the inherent surface acidity and good hydrothermal stability.Faujasite zeolites are commonly separated into two classes: (1) zeolite X, which has a silicon to aluminum Si/Al ratio between 1 and 1.5, and (2) zeolite Y which has a silicon to aluminum Si/Al ratio above 1.5. The large pore openings and large cavities of zeolite X make it an attractive material for ion exchange, adsorption, and drying processes [6, 7]. Notably, the thermal and hydrothermal stabilities of zeolite Y are strongly related to its Si/Al ratio, which plays a very important role in materials intended for application as fluidized catalytic cracking (FCC) catalysts.However, conventional zeolite Y (Si/Al molar ratio below 2.5) application to petrochemical industry is limited due to the weak acidity, as well as poor hydrothermal stability. For the sake of better industrial realm application, conventional Y zeolite is replaced by a high silica ultrastable Y zeolite (USY, with Si/Al > 4) [8], prepared from various posttreatments which include steaming at elevated temperatures [9, 10], introduction of SiCl4 vapor at moderate temperatures [11], treatment with ammonium hexafluorosilicate [12], and chelating agents [13]. Unfortunately, these posttreatments methods require several posttreatments and heat treatment often leads to structure being distorted.Compared with these posttreatments, the direct synthesis method is a more convenient way to obtain the high silica Y zeolite. The direct synthesis method includes structure-directing agent (SDA) method [14, 15]; organic templates method, for example, tetramethylammonium cation (TMA+) from tetramethylammonium bromide (TMABr), or tetramethylammonium hydroxide (TMAOH), is the most typical organic template [16–20]; crown ether family [21, 22] and N-methylpyridinium iodide [5] are also occasionally used. However, the SDA has instability and bad repeatability, which limit its application in industry [15] and the organic templates method needs to consume a large amount of organic template in the synthesis process, and the high-cost and toxicity limit the broader applications in industry. Hence it is very desirable to find a low-cost approach for the synthesis of high silica zeolite Y.In the present work, we reduce the basicity of the synthesis system by adding sulfuric acid to improve the SiO2/Al2O3 ratio, and the effect of alkalinity and crystallization time is investigated to obtain a reasonable basicity. Under this basicity, we synthesized high silica zeolite Y without structure-directing agent or organic template and the crystallization time is also acceptable. Different samples are applied as a catalyst for catalytic cracking of cumene to clarify the effect of the SiO2/Al2O3 ratio on the catalytic performance, and, encouragingly, it demonstrates a strong potential in petroleum processing.


## 2. Experimental Details

### 2.1. Chemicals

All the chemicals were directly used as received with no further purification. The reactants used were aqueous colloidal silica (w(SiO2) = 30%, Sinopharm Chemical Reagent Co., Ltd.), sodium aluminate (w(Al2O3) > 45%, Sinopharm Chemical Reagent Co., Ltd.), sodium hydroxide (w(NaOH) > 96%, Sinopharm Chemical Reagent Co., Ltd.), sulfuric acid (w(H2SO4) > 98%, Sinopharm Chemical Reagent Co., Ltd.), and deionized water.


### 2.2. Preparation of Zeolite Y

Sodium aluminate, sodium hydroxide, and deionized water were placed in a beaker to ensure good mixing on a magnetic stirrer at room temperature. After the solution became transparent, the aqueous colloidal silica was added under agitation for 2 h to yield the sodium aluminate solution. At last, the sulfuric acid was added to the gel to produce a gel with the overall stoichiometry Na2O : Al2O3 : SiO2 : H2O : H2SO4 = 4.3 : 1 : 10 : 180 : a (where a = 0; 0.67; 1.34; 2.01). This gel was homogenized, and then it was transferred to a stainless-steel autoclave (50 mL PTFE lined); then the sealed autoclave was placed in the oven at 100°C for hours. After this procedure, the products were filtered, washed with deionized water, and dried. The as-synthesized zeolite Y was denoted as NaY-a-b.


### 2.3. Preparation of H-Type Zeolite Y

The sodium form of zeolite was converted to the hydrogen form by ammonium ion exchange method. The zeolite was treated with 1 M ammonium chloride solution at 80°C for 2 h. Note that the zeolite to ammonium chloride solution was 1 g : 100 mL. The residue was filtered and washed with distilled water; then the sample was dried at a temperature of 120°C for 4 h. The above cycle was repeated three times to get complete exchange of sodium. As a final step, the samples were heated at 550°C for 5 h to decompose to H-type zeolite. The zeolite HY was denoted as HY-a-b (a and b have the same meaning as those in Section 2.2).


### 2.4. H-Type Zeolite Y Activity Evaluation

The zeolite cracking activity was determined with cumene as the probe molecules, which used a flow-type apparatus equipped with a fixed-bed reactor. Nitrogen was used as carrier gas at flows of 3.0 L/h. The catalysts were pressed binder-free and crushed to a particle size of 60–80 meshes, and the catalyst amount was 0.26 g. In the case of cumene cracking, nitrogen saturated with vaporized cumene at 300°C was passed through the reactor (the flow rate of liquid state cumene = 6.0 mL/h), and the reaction temperature was 300°C as well. Reaction products were analyzed by an online gas chromatograph with flame ionization detector.


### 2.5. Sample Characterization

The powder XRD patterns were collected on the XD-3 of the Beijing Purkinje General Instrument Co., with graphite monochromatized Cu-Kα (λ = 0.154056 nm) radiation at 36 kV, 20 mA. All the samples were collected in the range of 5–50° with continuous scanning mode, and the scanning speed was set to be 2°/min. The scanning electron microscopy (SEM) images were captured on a Hitachi field-emission scanning electron microscope (S-4800) operated at an accelerating voltage of 15 kV. Elemental compositions of the samples were carried out on a Philips Magix (PW2403) X-ray fluorescence (XRF) spectrometer. The data were analyzed using an IQ + fast quantitative software package. N2 adsorption-desorption was performed at 77 K in the Bei Shi De Instrument Technology (Beijing) Co., Ltd. (3H-2000PS1), and the samples were degassed at 250°C for 6 h prior to analysis.


## 2.1. Chemicals

All the chemicals were directly used as received with no further purification. The reactants used were aqueous colloidal silica (w(SiO2) = 30%, Sinopharm Chemical Reagent Co., Ltd.), sodium aluminate (w(Al2O3) > 45%, Sinopharm Chemical Reagent Co., Ltd.), sodium hydroxide (w(NaOH) > 96%, Sinopharm Chemical Reagent Co., Ltd.), sulfuric acid (w(H2SO4) > 98%, Sinopharm Chemical Reagent Co., Ltd.), and deionized water.


## 2.2. Preparation of Zeolite Y

Sodium aluminate, sodium hydroxide, and deionized water were placed in a beaker to ensure good mixing on a magnetic stirrer at room temperature. After the solution became transparent, the aqueous colloidal silica was added under agitation for 2 h to yield the sodium aluminate solution. At last, the sulfuric acid was added to the gel to produce a gel with the overall stoichiometry Na2O : Al2O3 : SiO2 : H2O : H2SO4 = 4.3 : 1 : 10 : 180 : a (where a = 0; 0.67; 1.34; 2.01). This gel was homogenized, and then it was transferred to a stainless-steel autoclave (50 mL PTFE lined); then the sealed autoclave was placed in the oven at 100°C for hours. After this procedure, the products were filtered, washed with deionized water, and dried. The as-synthesized zeolite Y was denoted as NaY-a-b.


## 2.3. Preparation of H-Type Zeolite Y

The sodium form of zeolite was converted to the hydrogen form by ammonium ion exchange method. The zeolite was treated with 1 M ammonium chloride solution at 80°C for 2 h. Note that the zeolite to ammonium chloride solution was 1 g : 100 mL. The residue was filtered and washed with distilled water; then the sample was dried at a temperature of 120°C for 4 h. The above cycle was repeated three times to get complete exchange of sodium. As a final step, the samples were heated at 550°C for 5 h to decompose to H-type zeolite. The zeolite HY was denoted as HY-a-b (a and b have the same meaning as those in Section 2.2).


## 2.4. H-Type Zeolite Y Activity Evaluation

The zeolite cracking activity was determined with cumene as the probe molecules, which used a flow-type apparatus equipped with a fixed-bed reactor. Nitrogen was used as carrier gas at flows of 3.0 L/h. The catalysts were pressed binder-free and crushed to a particle size of 60–80 meshes, and the catalyst amount was 0.26 g. In the case of cumene cracking, nitrogen saturated with vaporized cumene at 300°C was passed through the reactor (the flow rate of liquid state cumene = 6.0 mL/h), and the reaction temperature was 300°C as well. Reaction products were analyzed by an online gas chromatograph with flame ionization detector.


## 2.5. Sample Characterization

The powder XRD patterns were collected on the XD-3 of the Beijing Purkinje General Instrument Co., with graphite monochromatized Cu-Kα (λ = 0.154056 nm) radiation at 36 kV, 20 mA. All the samples were collected in the range of 5–50° with continuous scanning mode, and the scanning speed was set to be 2°/min. The scanning electron microscopy (SEM) images were captured on a Hitachi field-emission scanning electron microscope (S-4800) operated at an accelerating voltage of 15 kV. Elemental compositions of the samples were carried out on a Philips Magix (PW2403) X-ray fluorescence (XRF) spectrometer. The data were analyzed using an IQ + fast quantitative software package. N2 adsorption-desorption was performed at 77 K in the Bei Shi De Instrument Technology (Beijing) Co., Ltd. (3H-2000PS1), and the samples were degassed at 250°C for 6 h prior to analysis.


## 3. Results and Discussion

### 3.1. Zeolite Y Crystallization with Different Alkalinity

The XRD patterns with different H2SO4/Al2O3 and different crystallization time are shown in Figure 1. Samples (A), (B), and (C) exhibited the typical diffraction peaks of zeolite Y [23], the XRD patterns correspond to gel evolution from the initial amorphous precursors (NaY-0-4), and the other XRD data can be found in detail in the supplementary information Figure S1 (see Supplementary Material available online at http://dx.doi.org/10.1155/2016/1486107). After 8 h (NaY-0-8) of crystallization XRD peaks corresponding to the Y-type zeolite structure emerged; afterward at 8–12 h of crystallization the XRD peaks become more apparent, which indicates a progressive growth of the crystallites until 12 h. Figure 1(B) shows XRD peaks corresponding to the FAU-type zeolite structure emerged after 48 h. According to the demonstrations, the alkalinity of the synthesis system directly affects the crystallization time. The crystallization time of a high crystalline zeolite Y increased from 8 h to 48 h when the H2SO4/Al2O3 changed from 0 to 0.67, and it extends to 312 h when H2SO4/Al2O3 = 1.34 (Figure 1(C)). At last, when H2SO4/Al2O3 = 2.01 (Figure 1(D)), the transformation process from the initial amorphous precursors to zeolite could not emerge.Figure 1
XRD patterns for NaY zeolite samples with different H2SO4/Al2O3 and different crystallization time. (A) NaY-0-12, (B) NaY-0.67-48, (C) NaY-1.34-312, and (D) NaY-2.01-720.Figure2 shows the relation of relative crystallinity and crystallization time with different H2SO4/Al2O3. In order to calculate relative crystallinity of the samples, a modified procedure described in [24] was used. After a background correction, the peak intensity sum of (111) (2θ = 6.2), (331) (2θ = 15.6), and (533) (2θ = 22.1) is an evaluation criterion; the maximum peak intensity (sample NaY-0-24) is designated as 100%. Figure 2 reflects the relations between the alkalinity of the synthesis system and the crystallization times. In this study, the sulfuric acid works as an additive to reduce the basicity of the synthesis system and the solubility of the aluminosilicate, which led to the decreased crystallization rate.Figure 2
The relation of relative crystallinity and crystallization time with different H2SO4/Al2O3.


### 3.2. XRF

The detailed SiO2/Al2O3 ratio data are listed in Table 1. It reveals that the alkalinity of the synthesis system has important impacts on SiO2/Al2O3 ratio of zeolite NaY. The SiO2/Al2O3 ratio of samples increases from 4.54 to 6.45 with the H2SO4/Al2O3 in the gel changing from 0 to 1.34.Table 1
The element content and SiO2/Al2O3 measured by XRF.
Sample
SiO2  (w%)
Al2O3  (w%)
Na2O (w%)
SiO2/Al2O3  (n/n)
NaY-0-12
62.8
23.5
13.5
4.54
NaY-0.67-48
66.2
21.4
12.3
5.26
NaY-0.67-144
66.1
21.4
12.3
5.25
NaY-1.34-312
70.3
18.5
10.9
6.46


### 3.3. SEM

SEM images of the samples collected at different H2SO4/Al2O3 and different crystallization time are presented in Figure 3. Sample (a) showed relatively uniform spherical particles in the size range of 0.8–1.0 μm. Under the lower alkalinity of the synthesis system, the particles size of sample (c) increased to 1.5 μm, and sample (e) particles size was about 4.0 μm; this law of variation about particle size has been reported in the literature [25]. It is worth mentioning that these particles’ surface was rough and angular; the characteristics of morphologies facilitated differentiating the crystal and the amorphous.Figure 3
The SEM images of the samples with different H2SO4/Al2O3 and different crystallization time. (a) NaY-0-12; (b) NaY-0.67-24; (c) NaY-0.67-48; (d) NaY-0.67-144; (e) NaY-1.34-312.
(a)
(b)
(c)
(d)
(e)


### 3.4. BET

Figure4 shows the N2 adsorption-desorption isotherms of the samples obtained at different alkalinity of gel, and the detailed data are in Table 2. All the samples exhibited a sharp uptake of N2 at very low relative pressures (P
/
P
0
<
0.001), implying the presence of micropores. On the other hand, samples (A) and (B) exhibited another uptake appeared at high relative pressure (0.85
<
P
/
P
0
<
1.0), which originated from intraparticle macropores [23] because of the uneven grain sizes of sample (C) (Figure 3(e)); it could not form intraparticle macropores. Particularly, sample (A) presented higher N2 adsorption capacity (about 240 cm3/g) at low pressures than sample (B) (about 220 cm3/g) and sample (C) (about 100 cm3/g), suggesting that the zeolite NaY synthesized in H2SO4/Al2O3 = 0 had larger surface area than other alkalinity. As shown in Table 2, the micropore surface area was decreased from 944.1 m2/g for sample (A), to 845.6 m2/g for sample (B), to 357.8 m2/g for sample (C). The micropore volume revealed the same decline tendencies in the following order: sample (C) < sample (B) < sample (A). Based on the above results, our study suggests that the textural parameters are related to the crystallinity of the samples, when the H2SO4/Al2O3 = 1.34; the product had low degree of crystallization and BET surface area.Table 2
Textural parameters of the samples obtained at different H2SO4/Al2O3.
Sample
Relative crystallinity %
BET surface area [m2g−1]
Micropore surface area [m2g−1]
Micropore volume [cm3g−1]
(A)
NaY-0-12
100
986.6
944.1
0.37
(B)
NaY-0.67-48
91
911.4
845.6
0.33
(C)
NaY-1.34-312
36
401.8
357.8
0.14Figure 4
N2 adsorption-desorption isotherms of the samples obtained at different H2SO4/Al2O3. (A) NaY-0-12; (B) NaY-0.67-48; (C) NaY-1.34-312.The XRD patterns of the samples transformed into H-type zeolite are illustrated in Figure5. Following ion exchange and calcinations, the XRD features of sample (A) weaken obviously except for (111) peak, but the positions of (111), (331), and (533) peaks change, indicating the part of the HY structure collapsed, whereas samples (B), (C), (D), and (E) show only a diminution of the original XRD intensity, but the peaks positions do not change clearly. The temperature of NH4Y structural collapse is strongly associated with the ammonium ion exchange degree and the SiO2/Al2O3 molar ratio. Hence the partial collapse of sample (A) should be the result from the low SiO2/Al2O3. Because the temperature of structural collapse was lower than the ammonia decomposition, NH4X and the low silica NH4Y zeolite could not be transformed to H-form zeolite by calcination method.Figure 5
XRD patterns of the H-type zeolite samples. (A) HY-0-12; (B) HY-0.67-24; (C) HY-0.67-48; (D) HY-0.67-144; (E) HY-1.34-312.


### 3.5. Catalytic Cracking of Cumene

The catalytic activity of the samples is shown in Figure6. The sample HY-0-12 had the lowest activity, the conversion of decomposition was only 12.7%, and the catalytic activity disappeared when the reaction lasted for about 70 min. It should be caused by the low content of zeolite; the sample HY-0-12 was mainly composed of amorphous silica-alumina material. However, samples HY-0.67-48, HY-0.67-72, and HY-0.67-144 had better performance; in particular the conversion of HY-0.67-48 could reach as high as 88.3% at the beginning of the reaction and 20.0% when the reaction lasted for about 390 min; the conversions of HY-0.67-72 and HY-0.67-144 were slightly lower than HY-0.67-48, 72% and 75%, respectively. The catalytic activity is related to the relative crystallinity, under the same SiO2/Al2O3 ratio condition; the higher the relative crystallinity, the higher the catalytic activity.Figure 6
The cumene catalytic reaction performance of the samples and the thermal cracking without catalyst (insert). (A) HY-0-12, (B) HY-0.67-48, and (C) HY-1.34-312.In addition, we found the activity reduces with the increasing reaction time. This is mainly caused by the coke deposit on catalysts; the coke deposition can block the zeolite pores and prevent active sites contact with cumene.


## 3.1. Zeolite Y Crystallization with Different Alkalinity

The XRD patterns with different H2SO4/Al2O3 and different crystallization time are shown in Figure 1. Samples (A), (B), and (C) exhibited the typical diffraction peaks of zeolite Y [23], the XRD patterns correspond to gel evolution from the initial amorphous precursors (NaY-0-4), and the other XRD data can be found in detail in the supplementary information Figure S1 (see Supplementary Material available online at http://dx.doi.org/10.1155/2016/1486107). After 8 h (NaY-0-8) of crystallization XRD peaks corresponding to the Y-type zeolite structure emerged; afterward at 8–12 h of crystallization the XRD peaks become more apparent, which indicates a progressive growth of the crystallites until 12 h. Figure 1(B) shows XRD peaks corresponding to the FAU-type zeolite structure emerged after 48 h. According to the demonstrations, the alkalinity of the synthesis system directly affects the crystallization time. The crystallization time of a high crystalline zeolite Y increased from 8 h to 48 h when the H2SO4/Al2O3 changed from 0 to 0.67, and it extends to 312 h when H2SO4/Al2O3 = 1.34 (Figure 1(C)). At last, when H2SO4/Al2O3 = 2.01 (Figure 1(D)), the transformation process from the initial amorphous precursors to zeolite could not emerge.Figure 1
XRD patterns for NaY zeolite samples with different H2SO4/Al2O3 and different crystallization time. (A) NaY-0-12, (B) NaY-0.67-48, (C) NaY-1.34-312, and (D) NaY-2.01-720.Figure2 shows the relation of relative crystallinity and crystallization time with different H2SO4/Al2O3. In order to calculate relative crystallinity of the samples, a modified procedure described in [24] was used. After a background correction, the peak intensity sum of (111) (2θ = 6.2), (331) (2θ = 15.6), and (533) (2θ = 22.1) is an evaluation criterion; the maximum peak intensity (sample NaY-0-24) is designated as 100%. Figure 2 reflects the relations between the alkalinity of the synthesis system and the crystallization times. In this study, the sulfuric acid works as an additive to reduce the basicity of the synthesis system and the solubility of the aluminosilicate, which led to the decreased crystallization rate.Figure 2
The relation of relative crystallinity and crystallization time with different H2SO4/Al2O3.


## 3.2. XRF

The detailed SiO2/Al2O3 ratio data are listed in Table 1. It reveals that the alkalinity of the synthesis system has important impacts on SiO2/Al2O3 ratio of zeolite NaY. The SiO2/Al2O3 ratio of samples increases from 4.54 to 6.45 with the H2SO4/Al2O3 in the gel changing from 0 to 1.34.Table 1
The element content and SiO2/Al2O3 measured by XRF.
Sample
SiO2  (w%)
Al2O3  (w%)
Na2O (w%)
SiO2/Al2O3  (n/n)
NaY-0-12
62.8
23.5
13.5
4.54
NaY-0.67-48
66.2
21.4
12.3
5.26
NaY-0.67-144
66.1
21.4
12.3
5.25
NaY-1.34-312
70.3
18.5
10.9
6.46


## 3.3. SEM

SEM images of the samples collected at different H2SO4/Al2O3 and different crystallization time are presented in Figure 3. Sample (a) showed relatively uniform spherical particles in the size range of 0.8–1.0 μm. Under the lower alkalinity of the synthesis system, the particles size of sample (c) increased to 1.5 μm, and sample (e) particles size was about 4.0 μm; this law of variation about particle size has been reported in the literature [25]. It is worth mentioning that these particles’ surface was rough and angular; the characteristics of morphologies facilitated differentiating the crystal and the amorphous.Figure 3
The SEM images of the samples with different H2SO4/Al2O3 and different crystallization time. (a) NaY-0-12; (b) NaY-0.67-24; (c) NaY-0.67-48; (d) NaY-0.67-144; (e) NaY-1.34-312.
(a)
(b)
(c)
(d)
(e)


## 3.4. BET

Figure4 shows the N2 adsorption-desorption isotherms of the samples obtained at different alkalinity of gel, and the detailed data are in Table 2. All the samples exhibited a sharp uptake of N2 at very low relative pressures (P
/
P
0
<
0.001), implying the presence of micropores. On the other hand, samples (A) and (B) exhibited another uptake appeared at high relative pressure (0.85
<
P
/
P
0
<
1.0), which originated from intraparticle macropores [23] because of the uneven grain sizes of sample (C) (Figure 3(e)); it could not form intraparticle macropores. Particularly, sample (A) presented higher N2 adsorption capacity (about 240 cm3/g) at low pressures than sample (B) (about 220 cm3/g) and sample (C) (about 100 cm3/g), suggesting that the zeolite NaY synthesized in H2SO4/Al2O3 = 0 had larger surface area than other alkalinity. As shown in Table 2, the micropore surface area was decreased from 944.1 m2/g for sample (A), to 845.6 m2/g for sample (B), to 357.8 m2/g for sample (C). The micropore volume revealed the same decline tendencies in the following order: sample (C) < sample (B) < sample (A). Based on the above results, our study suggests that the textural parameters are related to the crystallinity of the samples, when the H2SO4/Al2O3 = 1.34; the product had low degree of crystallization and BET surface area.Table 2
Textural parameters of the samples obtained at different H2SO4/Al2O3.
Sample
Relative crystallinity %
BET surface area [m2g−1]
Micropore surface area [m2g−1]
Micropore volume [cm3g−1]
(A)
NaY-0-12
100
986.6
944.1
0.37
(B)
NaY-0.67-48
91
911.4
845.6
0.33
(C)
NaY-1.34-312
36
401.8
357.8
0.14Figure 4
N2 adsorption-desorption isotherms of the samples obtained at different H2SO4/Al2O3. (A) NaY-0-12; (B) NaY-0.67-48; (C) NaY-1.34-312.The XRD patterns of the samples transformed into H-type zeolite are illustrated in Figure5. Following ion exchange and calcinations, the XRD features of sample (A) weaken obviously except for (111) peak, but the positions of (111), (331), and (533) peaks change, indicating the part of the HY structure collapsed, whereas samples (B), (C), (D), and (E) show only a diminution of the original XRD intensity, but the peaks positions do not change clearly. The temperature of NH4Y structural collapse is strongly associated with the ammonium ion exchange degree and the SiO2/Al2O3 molar ratio. Hence the partial collapse of sample (A) should be the result from the low SiO2/Al2O3. Because the temperature of structural collapse was lower than the ammonia decomposition, NH4X and the low silica NH4Y zeolite could not be transformed to H-form zeolite by calcination method.Figure 5
XRD patterns of the H-type zeolite samples. (A) HY-0-12; (B) HY-0.67-24; (C) HY-0.67-48; (D) HY-0.67-144; (E) HY-1.34-312.


## 3.5. Catalytic Cracking of Cumene

The catalytic activity of the samples is shown in Figure6. The sample HY-0-12 had the lowest activity, the conversion of decomposition was only 12.7%, and the catalytic activity disappeared when the reaction lasted for about 70 min. It should be caused by the low content of zeolite; the sample HY-0-12 was mainly composed of amorphous silica-alumina material. However, samples HY-0.67-48, HY-0.67-72, and HY-0.67-144 had better performance; in particular the conversion of HY-0.67-48 could reach as high as 88.3% at the beginning of the reaction and 20.0% when the reaction lasted for about 390 min; the conversions of HY-0.67-72 and HY-0.67-144 were slightly lower than HY-0.67-48, 72% and 75%, respectively. The catalytic activity is related to the relative crystallinity, under the same SiO2/Al2O3 ratio condition; the higher the relative crystallinity, the higher the catalytic activity.Figure 6
The cumene catalytic reaction performance of the samples and the thermal cracking without catalyst (insert). (A) HY-0-12, (B) HY-0.67-48, and (C) HY-1.34-312.In addition, we found the activity reduces with the increasing reaction time. This is mainly caused by the coke deposit on catalysts; the coke deposition can block the zeolite pores and prevent active sites contact with cumene.


## 4. Conclusions

We have demonstrated that high silica Y zeolite can be synthesized using direct synthesis method without adding any organic additive or SDA. The relative crystallinity and crystallization time of zeolite NaY particles can be controlled by the H2SO4/Al2O3 ratio of the synthesis gel. The crystallization time was also acceptable when the synthesis gel Na2O : Al2O3 : SiO2 : H2O : H2SO4 = 4.3 : 1 : 10 : 180 : 0.67. XRD and XRF show that the zeolite Y nanocrystals obtained are highly crystalline and high SiO2/Al2O3 ratio. The as-synthesized zeolite Y nanocrystals show high N2 adsorption and BET surface area and micropore volume are determined to be 911.4 m2/g and 0.33 cm3/g, respectively. In addition, compared with lower silica Y zeolite, the as-synthesized high silica Y zeolite shows excellent cracking performance.



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