# Preparation of Ti Material Supported SBA-15 Functionalized with Sulfonic Acid Environmental Friendly Catalyst: Application for Esterification Process

Authors: Raju Kalakuntala; Mallaiah Mekala; Suman Chirra; Venkatathri Narayanan; Vighneswara Rao Kakara; Srinath Suranani
Journal: Journal of Nanomaterials
 (2022)

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## Abstract

Kinetics of catalytic esterification between propionic acid and n-butanol has been studied in a batch reactor by using a Ti-supported SBA-15 catalyst with sulfonic acid. The synthesized catalyst is used to test the efficacy of catalyst for esterification reaction. The SBA-15 acidity is tied to incorporation of Ti and -SO3H groups through and the use of Si/Ti with Si/S molar ratios. The results are mesoporous materials with a typical hexagonal structure of the Ti SBA-15 and wide areas and high pore diameters that are operated with sulfonic groups. The addition of SBA to Ti leads mainly to catalytic materials with Bronsted and Lewis acid sites. Ti SBA-15 is the most effective catalyst for sulfonic acid, with the highest consents of Lewis acid sites and deactivation resistance and low hydrophilicity. The effect of temperature, catalyst amount, and molar ratio on reaction kinetics has been studied. The conversion of propionic acid is found to be 91% at 115°C at a 2 : 1 ratio of n-butanol to propionic acid molars with 2% of sulfonic acid supported Ti SBA-15. The Eley-Rideal kinetic model is used to fit the experimental data. The activation energy and kinetic factor are found to be 29.63 kJ mol–1 and ko 0.549 L2 g-1 mol-1, respectively.


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## Body

## 1. Introduction

Catalysis was first introduced as part of the growth of industrial technology in the 1960s, with a focus on refinery and petrochemical operations. Catalysis has advanced at a rapid rate over the last two decades, and it is now recognized as a multidisciplinary discipline requiring synergistic interactions among a diverse spectrum of professionals, including materials, electrical, and mechanical engineers, physicists, biologists, and physicians. Catalysis provides and develops new, efficient, and cost-effective strategies and tools, as a leading technology toward a sustainable future and a clean environment, thereby improving people’s quality of life [1].
(1)Propionicacid+Butanol↔Butylpropionate+WaterIn a multitude of goods, carboxylic acid esters are essential, from fragrances to biofuels. The latter would be of specific importance because of increasing crude oil prices and environmental issues. There are several hybrid routes for the production of organic esters [2]. The widely used technique for ester synthesis is an esterification reaction between carboxylic acids and alcohol. The reaction could be performed conventionally in batch reactors in a liquid state using powerful liquid nutrient acids like H2SO4, HI, and HCl as the catalyst [3, 4]. However, the handling strategy needs extra measures of catalyst removal and segregation with the substrate being disposed of salts, which usually adds to the processing cost. Alternatively, it is easy to separate strong catalysts from response products that can be used for various reaction cycles in most instances [4]. Furthermore, strong catalysts are used more readily in ongoing processing activities, enhancing the ester manufacturing economy. For these reasons, the development of strong acid catalysts for esterification applications is of considerable concern [5]. The mathematical model and response mechanism for alkene esterification using homogeneous catalysts were well documented during a protonated methyl ester which was assaulted by a molecule of nucleophile alcohol, resulting in ester and water. With strong acid precursors containing mainly Bronsted acid clusters, esterification reaction could be expected with an analogous process to the homogeneous regime that mediates conversion [6, 7]. The results were uncertain in the literature on a basic strong acid-catalyzed esterification reaction. Two processes were suggested mainly for the esterification of heterogeneous catalysts. One is a single site mechanism, and the other one is a double site mechanism. Acetic acid esterification reaction with methanol by using SAC-13 was carried out with Bronsted acid sites as a single-site system. It is a gas stage with a range of temperatures of 90-140°C or within a condensed stage with temperature of 660°C, based on mainly the outcomes of studies with pyridine poisoning. An Eley-Rideal kinetic equation was developed to predict the experimental results with an accuracy of 8% for 1-octanol and hexanoic acid esterification utilizing zeolite and SAC-13 as catalysts [8].The objective of the present research is the preparation and characterizations of an environmental catalyst for the esterification of propionic acid after the integration of Ti and sulfonic groups in SBA-15. The kinetics studies at different parameters have been carried out to find the conversion of propionic acid under various parameters. The Eley-Rideal model fitted with experimental data.


## 2. Experimental

### 2.1. Catalyst Preparation

Pluronic P123 is a discreet, linear substitute, triblock copolymer made up of polyethylene oxide (PEO) and polypropylene oxide (PPO). In an experiment 5 g of triblock copolymer (i.e., P123), structured mesoporous components such as SBA-15 are used as a backbone to be dispersed into distilled water of 116.25 g, and 29.13 g hydrochloric acid is inputted into the solution. Final 11 g of tetra-ethyl-ortho-silicate as a drug additive of silica was applied to tetraisopropoxide titanium (Si/Ti=100) during steady 24-hour temperature mixing. The resulting slurry was accompanied by N-butanol and washed with distilled water. The material dried at 110°C for 12 hours and then calcined at 500°C for 8 hours [9].


### 2.2. Characterization

The pattern in the Ultima IV diffractometer is the powder X-ray diffraction (XRD). The following statistical figures are obtained within the range of 0.1-5° with a phase of 0.008° and a scanning speed of 0.5° per minute, using the nonfiltered Cu Kα radiation source, in the form of a Ţ=0.54178Å with 30 mA and 40 kV. TESCAN and VEGA 3 LMU, Australia, used for surface morphology study a scanning electron microscope (SEM). The photos of the samples were analysed with a 200 kv acceleration voltage using a tool JEOL Australia. Sample pores and surface area are specified in liquid nitrogen (77 K) and the Chinese surface inspection system, Quanta Chrome Nova-1000, and also the de Boert map, BET, and pore size. Samples were obtained at 1 : 10 KBr room temperature with 10 scans from FTIR, PerkinElmer, Spectrum 100, USA. A Fourier transform spectra registered the samples [10]. On Evolution 300 Thermo Science, the sample spectrum was recorded with UV-visible spectrometer, USA, and BaSO4 as reference, diffuse UV-visible spectrum (UV-Vis-DRS).


### 2.3. Reaction Kinetics Study

The reactor was filled with one mole of propionic acid and one mole of n-butanol. The heat input is supplied by rotating the heating knob to a desired temperature. The stirrer is adjusted to 480 rpm to mix the catalyst with reactants. When there is no temperature, the recalculated amount of catalyst is transferred into the reaction mixture. This time onwards the actual reaction time counted. The samples have been withdrawn in the regular intervals and analysed for propionic acid conversion by titration with standard NaOH solution. The reaction is continued till there is no change in the concentration of propionic acid concentration with time. This indicates the reaction reached chemical equilibrium.


## 2.1. Catalyst Preparation

Pluronic P123 is a discreet, linear substitute, triblock copolymer made up of polyethylene oxide (PEO) and polypropylene oxide (PPO). In an experiment 5 g of triblock copolymer (i.e., P123), structured mesoporous components such as SBA-15 are used as a backbone to be dispersed into distilled water of 116.25 g, and 29.13 g hydrochloric acid is inputted into the solution. Final 11 g of tetra-ethyl-ortho-silicate as a drug additive of silica was applied to tetraisopropoxide titanium (Si/Ti=100) during steady 24-hour temperature mixing. The resulting slurry was accompanied by N-butanol and washed with distilled water. The material dried at 110°C for 12 hours and then calcined at 500°C for 8 hours [9].


## 2.2. Characterization

The pattern in the Ultima IV diffractometer is the powder X-ray diffraction (XRD). The following statistical figures are obtained within the range of 0.1-5° with a phase of 0.008° and a scanning speed of 0.5° per minute, using the nonfiltered Cu Kα radiation source, in the form of a Ţ=0.54178Å with 30 mA and 40 kV. TESCAN and VEGA 3 LMU, Australia, used for surface morphology study a scanning electron microscope (SEM). The photos of the samples were analysed with a 200 kv acceleration voltage using a tool JEOL Australia. Sample pores and surface area are specified in liquid nitrogen (77 K) and the Chinese surface inspection system, Quanta Chrome Nova-1000, and also the de Boert map, BET, and pore size. Samples were obtained at 1 : 10 KBr room temperature with 10 scans from FTIR, PerkinElmer, Spectrum 100, USA. A Fourier transform spectra registered the samples [10]. On Evolution 300 Thermo Science, the sample spectrum was recorded with UV-visible spectrometer, USA, and BaSO4 as reference, diffuse UV-visible spectrum (UV-Vis-DRS).


## 2.3. Reaction Kinetics Study

The reactor was filled with one mole of propionic acid and one mole of n-butanol. The heat input is supplied by rotating the heating knob to a desired temperature. The stirrer is adjusted to 480 rpm to mix the catalyst with reactants. When there is no temperature, the recalculated amount of catalyst is transferred into the reaction mixture. This time onwards the actual reaction time counted. The samples have been withdrawn in the regular intervals and analysed for propionic acid conversion by titration with standard NaOH solution. The reaction is continued till there is no change in the concentration of propionic acid concentration with time. This indicates the reaction reached chemical equilibrium.


## 3. Results and Discussions

The synthesized sulfonic acid-functionalized Ti SBA-15 catalyst is analysed for its characterization and used for kinetic investigations for reaction temperature of 85°C to 115°C, catalyst loading of 1 wt% to 3 wt%, and mole ratio of acid to alcohol 1 : 1 to 1 : 4.


### 3.1. Transmission Electron Micrograph Analysis (TEM)

Figure1 shows Ti-supported SBA-15 functionalized with sulfonic acid, revealing a hexagonally well-organized mesoporous catalyst with severe parallel channels, close to porous configuration. Ti-supported SBA-15 functionalized with sulfonic acid; TEM images functionalized with sulfonic acid [11]. In the long-range mesoporous ordering determined as opposed to the Ti-supported SBA-15 functionalized with sulfonic acid, there were uniform morphologies of the macrostructure of silica materials sulfonated.Figure 1
TEM images of Ti-supported SBA-15 functionalized with sulfonic acid.


### 3.2. Diffuse Reflectance Ultraviolet-Visible Spectroscopic Analysis

The Ti-supported SBA-15 functionalized with sulfonic acid spectrum of UV-Vis-DRS is shown in Figure2. Two large peaks of ~210-230 nm and 330-350 nm were observed confined to the presence and integration of the tetrahedral environment and the homogeneous distribution of Ti ions in the Ti-supported SBA-15 functionalized with sulfonic acid matrix [12].Figure 2
Ti-supported SBA-15 functionalized with sulfonic acid UV-Vis-DRS study.


### 3.3. Fourier Transform Infrared Spectroscopic Analysis (FTIR)

Figure3 displays the Ti-supported SBA-15 functionalized with sulfonic acid composite FTIR spectrum of sulfonic acid. The 1088 cm-1 peak suggests the Si-O-Si bond in a Ti SBA-15 fused sulfonated binding. The vibrations of Si–O–Si symmetrically stretching were 802 cm–1 and 466 cm–1, respectively. Due to Ti-O-infrastructure Si’s vibration, peaks 910 and 960 cm–1 resulted, which means that Ti is strongly indicated in the SBA-15 matrix [13]. The exact location of the pictures was found to contribute both to the chemical composition and the calibration and resolution of the instrument used in the studies. In the Ti-supported SBA-15 functionalized with sulfonic acid catalyst, the maximum strength of the band is 960 cm-1. Due to hydrogen interaction, breaks between the silanol groups and the water molecules adsorbed were seen at 1630 and 3400 cm-1 (SI-OH). The peaks of 1052 and 1140 cm-1 confirm that the functional groups -SO4H have symmetrical and asymmetrical vibrations.Figure 3
FT-IR analysis of Ti-supported SBA-15 functionalized with sulfonic acid.


### 3.4. Powder X-Ray Diffraction (XRD)

Synthesized sulfonic acid pattern of powder X-ray diffraction (XRD) composites functionalized by Ti-supported SBA-15 shown in Figure4. In the X-ray diffraction study, two weak peaks and a strong, extreme peak were noted [14]. The weak peaks found by 2θ were 1.4 and 1.7, and the sharp peak by 2θ was 0.8, which specify the periodicity of the high structures as a result of higher condensation between the silanol and titanium groups.Figure 4
Small-angle XRD pattern of Ti-supported SBA-15 functionalized with sulfonic acid.


### 3.5. Thermogravimetry/Differential Thermal Analysis

Figures5 and 6 display the Ti-supported SBA-15 functionalized with sulfonic acid materials from the TG-DTA analysis of sulfonic acid. It explains preliminary weight loss from 0°C to 300°C (4.31%) by loss in mesoporous composite of water adsorbed and ethanol molecules [15]. Therefore, the decomposition of the pattern that is trapped within the Ti-supported SBA-15 functionalized with sulfonic acid and its remainder shown to be steep weight loss between 350°C and 600°C is 29.86% to 58.75%.Figure 5
TGA analysis of Ti-supported SBA-15 functionalized with sulfonic acid.Figure 6
DTA analysis of Ti-supported SBA-15 functionalized with sulfonic acid.The DTA plot proposed that the patterns of the mesoporous material should be heated. A weight loss of initial 0°C to 300°C of 0°C is observed in the data track of the sulfonic acid functionalized composite Ti-SBA-15 (4.06%). A further weight loss in sulfonic acid pores of Ti-SBA-15 (42.89%) was found to be 52.3% due to the oxidative decomposition of obstructed patterns, and residual mass was 52.3%. A large exothermic peak at 308.7°C has been reported. The Ti-supported SBA-15 functionalized with sulfonic acid composite has no weight loss observed in 500-700°C. These Ti-SBA-15 composites with sulfonic acid function are also thermally stable up to 700°C.


### 3.6. N2 Adsorption-Desorption Studies

Information on the surface area, the pores of composites Ti-supported SBA-15 functionalized with sulfonic acid have been provided through adsorption isothermal studies and is shown in Figure7. Subsequently, it was noted that the silicon composites were shown to indicate their mesoporosity as the type IV nitrogen isotherms with the deposal H1 hysteresis loop [16]. The distribution of mesoporous sizes extends when the Ti is incorporated in the SBA-15 framework. These results have been validated using the distribution curve for pore size. The results show that when the Ti was integrated into the SBA-15 functionalized with sulfonic acid framework, the consistency of the mesoporous size distribution has declined. It was also noted that the pore volume, surface area, pore diameter, and also peak intensities were decreased sharply with increased incorporation of Ti into the SBA-15 functionalized with sulfonic acid samples [17]. This could be due to the blocking by titanium-based mesoporous canals. In order to define the texture properties of the mesoporous catalysts, the BJH pore size distribution approach and the BET surface analysis are employed in Table 1.Figure 7
Ti-supported SBA-15 functionalized with sulfonic acid with N2 adsorption/desorption isotherms, pore diameter, and pore volume distribution.Table 1
BET–isothermic adsorption and porosity data.
Mesoporous materialPore volume (cc/g)Average pore diameter (Å)Surface area (m2/g)Ti-supported SBA-15 functionalized with sulfonic acid1.0231.78457


## 3.1. Transmission Electron Micrograph Analysis (TEM)

Figure1 shows Ti-supported SBA-15 functionalized with sulfonic acid, revealing a hexagonally well-organized mesoporous catalyst with severe parallel channels, close to porous configuration. Ti-supported SBA-15 functionalized with sulfonic acid; TEM images functionalized with sulfonic acid [11]. In the long-range mesoporous ordering determined as opposed to the Ti-supported SBA-15 functionalized with sulfonic acid, there were uniform morphologies of the macrostructure of silica materials sulfonated.Figure 1
TEM images of Ti-supported SBA-15 functionalized with sulfonic acid.


## 3.2. Diffuse Reflectance Ultraviolet-Visible Spectroscopic Analysis

The Ti-supported SBA-15 functionalized with sulfonic acid spectrum of UV-Vis-DRS is shown in Figure2. Two large peaks of ~210-230 nm and 330-350 nm were observed confined to the presence and integration of the tetrahedral environment and the homogeneous distribution of Ti ions in the Ti-supported SBA-15 functionalized with sulfonic acid matrix [12].Figure 2
Ti-supported SBA-15 functionalized with sulfonic acid UV-Vis-DRS study.


## 3.3. Fourier Transform Infrared Spectroscopic Analysis (FTIR)

Figure3 displays the Ti-supported SBA-15 functionalized with sulfonic acid composite FTIR spectrum of sulfonic acid. The 1088 cm-1 peak suggests the Si-O-Si bond in a Ti SBA-15 fused sulfonated binding. The vibrations of Si–O–Si symmetrically stretching were 802 cm–1 and 466 cm–1, respectively. Due to Ti-O-infrastructure Si’s vibration, peaks 910 and 960 cm–1 resulted, which means that Ti is strongly indicated in the SBA-15 matrix [13]. The exact location of the pictures was found to contribute both to the chemical composition and the calibration and resolution of the instrument used in the studies. In the Ti-supported SBA-15 functionalized with sulfonic acid catalyst, the maximum strength of the band is 960 cm-1. Due to hydrogen interaction, breaks between the silanol groups and the water molecules adsorbed were seen at 1630 and 3400 cm-1 (SI-OH). The peaks of 1052 and 1140 cm-1 confirm that the functional groups -SO4H have symmetrical and asymmetrical vibrations.Figure 3
FT-IR analysis of Ti-supported SBA-15 functionalized with sulfonic acid.


## 3.4. Powder X-Ray Diffraction (XRD)

Synthesized sulfonic acid pattern of powder X-ray diffraction (XRD) composites functionalized by Ti-supported SBA-15 shown in Figure4. In the X-ray diffraction study, two weak peaks and a strong, extreme peak were noted [14]. The weak peaks found by 2θ were 1.4 and 1.7, and the sharp peak by 2θ was 0.8, which specify the periodicity of the high structures as a result of higher condensation between the silanol and titanium groups.Figure 4
Small-angle XRD pattern of Ti-supported SBA-15 functionalized with sulfonic acid.


## 3.5. Thermogravimetry/Differential Thermal Analysis

Figures5 and 6 display the Ti-supported SBA-15 functionalized with sulfonic acid materials from the TG-DTA analysis of sulfonic acid. It explains preliminary weight loss from 0°C to 300°C (4.31%) by loss in mesoporous composite of water adsorbed and ethanol molecules [15]. Therefore, the decomposition of the pattern that is trapped within the Ti-supported SBA-15 functionalized with sulfonic acid and its remainder shown to be steep weight loss between 350°C and 600°C is 29.86% to 58.75%.Figure 5
TGA analysis of Ti-supported SBA-15 functionalized with sulfonic acid.Figure 6
DTA analysis of Ti-supported SBA-15 functionalized with sulfonic acid.The DTA plot proposed that the patterns of the mesoporous material should be heated. A weight loss of initial 0°C to 300°C of 0°C is observed in the data track of the sulfonic acid functionalized composite Ti-SBA-15 (4.06%). A further weight loss in sulfonic acid pores of Ti-SBA-15 (42.89%) was found to be 52.3% due to the oxidative decomposition of obstructed patterns, and residual mass was 52.3%. A large exothermic peak at 308.7°C has been reported. The Ti-supported SBA-15 functionalized with sulfonic acid composite has no weight loss observed in 500-700°C. These Ti-SBA-15 composites with sulfonic acid function are also thermally stable up to 700°C.


## 3.6. N2 Adsorption-Desorption Studies

Information on the surface area, the pores of composites Ti-supported SBA-15 functionalized with sulfonic acid have been provided through adsorption isothermal studies and is shown in Figure7. Subsequently, it was noted that the silicon composites were shown to indicate their mesoporosity as the type IV nitrogen isotherms with the deposal H1 hysteresis loop [16]. The distribution of mesoporous sizes extends when the Ti is incorporated in the SBA-15 framework. These results have been validated using the distribution curve for pore size. The results show that when the Ti was integrated into the SBA-15 functionalized with sulfonic acid framework, the consistency of the mesoporous size distribution has declined. It was also noted that the pore volume, surface area, pore diameter, and also peak intensities were decreased sharply with increased incorporation of Ti into the SBA-15 functionalized with sulfonic acid samples [17]. This could be due to the blocking by titanium-based mesoporous canals. In order to define the texture properties of the mesoporous catalysts, the BJH pore size distribution approach and the BET surface analysis are employed in Table 1.Figure 7
Ti-supported SBA-15 functionalized with sulfonic acid with N2 adsorption/desorption isotherms, pore diameter, and pore volume distribution.Table 1
BET–isothermic adsorption and porosity data.
Mesoporous materialPore volume (cc/g)Average pore diameter (Å)Surface area (m2/g)Ti-supported SBA-15 functionalized with sulfonic acid1.0231.78457


## 4. Catalytic Performance (Sulfonic Acid Functionalized Ti SBA-15)

### 4.1. Effect of Reactant Molar Ratio

The mole ratio of propionic acid with n-butanol varied from 1 : 1 to 1 : 4 at a temperature of 115°C and a speed of 240 rpm for conversion of propionic acid with Ti-supported SBA-15 functionalized with sulfonic acid [18]. The conversion of propionic acid as function of molar ratio is shown in Figure 8. The propionic acid conversion increases as the molar ratio increases due to excess n-butanol. From the figure, it could be observed as 79.90%.Figure 8
Conversion versus time for different molar ratios. Other conditions are catalyst loading: 2%, temperature: 115°C, and speed: 240 rpm.


### 4.2. Effect of Temperature

The effect temperature on the conversion of propionic acid at 2% by wt catalyst loading and at 1 : 1 mole ratio is shown in Figure9. The conversion of propionic acid is increased as temperature increases. Higher the temperatures, the time required to reach equilibrium is lesser [19]. It shows that the reaction is kinetically controlled.Figure 9
Conversion versus time for different temperatures. Other conditions are catalyst loading: 2%, mole ratio: 1 : 1, and speed: 240 rpm.


### 4.3. Effect of Catalyst Amount

The effect of catalyst amount on the propionic acid conversion kinetics is shown in Figure10 at a temperature of and mole ratio of 1 : 1. The experiments employ separate catalyst concentrations of 1, 2, and 3 wt%. The conversion of propionic acid increases as the catalyst loading increases [20]. When the catalyst quantity increased in the reaction mixture, the reaction rate increases due to availability of H+ ions which in turn provide more catalyst surface area. The experiments were conducted for 4 runs with the same catalyst. The propionic acid conversion is the same under 1% error.Figure 10
Conversion vs. time (min) for different catalyst loadings. Other conditions are mole ratio: 1 : 1, temperature: 115°C, and speed: 240 rpm.


### 4.4. The Ti-Supported SBA-15 Functionalized with Sulfonic Acid for the Kinetic Analysis

The initial reaction rate of propionic acid with n-butanol has been carried out under different catalyst loadingsrAo=∆CAo/∆t for this catalyst [21]. The general kinetic expression for the catalyzed heterogeneous esterification reaction can be written as
(2)−rA=kfwcatCACB−CRCw/Keq1+KACA+KBCB+KECE+KwCwn,whererA is the reaction rate and wcat is the catalyst weight on dry basis. A, B, E, and W represent propionic acid, n-butanol, butyl propionate, and water. K is the adsorption constant, Ke is the equilibrium constant, and kf is the forward reaction rate constant. In equation (2), when n=0, it is a PH model; when n=1, it is ER model; and when n=2, it is a LHHW model.As can be seen in Figure11, the starting reaction rate instead of the plated one is a linear feature, which means the adsorption of propionic acid on the Ti-supported SBA-15 functionalized with sulfonic acid catalyst surface is not possible, and at the same time, the initial rate of reaction increases in line with n-butanol concentrations. Therefore, we can infer that at low concentrations of n-butanol, it adsorbed n-butanol extremely low and almost continuously increases the concentration. This study concludes that the reaction mechanism is defined in the Eley-Rideal model, i.e., reaction between adsorbed butanol molecules and propionic acid molecules in the bulk solution. In the single site, only one reactant is adsorbed on the catalyst and the remaining reactant is in the bulk reaction. In the double site, two reactants are at the catalyst surface and reaction proceed at this place and formed products desorbed from the catalyst surface. The literature found the solvent (dioxane) and ester adsorption to be insignificant. The rate determination step is to specifically take the stoichiometric and corresponding reaction rate as the Eley-Rideal (ER) model of a surface-reaction equation. After excluding terms of adsorption of acid and ester, ER form can be written as
(3)−rA=kfwcatCACB−CRCw/Keq1+KBCB+KwCw.Figure 11
The effect on the initial reaction rate of (−rAo) at different temperatures on the charging of catalyst.The Arrhenius law expresses the dependence of temperature on reaction rate as given in the following.Equation (3) behavior is used for speed expression rather than concentration, because the predictions of models adapted to the measured film data result in improved prediction [22]. Relocation of equation (4) can be described as equation for the initial reaction rate without a product present, shown in
(4)CAoCBo−rAo=1kfwcat+KBkfwcatCBo.Figure12 shows the plot of CAoCBo/−rAo versus CB,o results in a direct slope line KB/kfwcat and intercept 1/kfwcat as shown in the figure.Figure 12
CAoCBo/−rAo versus CB0 at different temperatures.Slopes and intercepts in these figures indicate the constants in rates and adsorption constantskF, KB, KW, and their estimated values at three temperatures as shown in Table 2.Table 2
Kinetics and adsorption constants.
Temperature (°C)kf/L2 mol-1 h-1KB/L mol-1KW/L mol-1850.78×10−40.180.19950.81×10−40.200.491050.78×10−40.190.511150.90×10−40.090.56


### 4.5. Activation Energy and Rate Constants

The Arrhenius law expresses the dependence of temperature on reaction rate as given in the following:(5)ki=kioexp−Ei/RT,wherekf is the activation energy for forward reaction and kio is the frequency factor [23]. Equation (5), a plot of lnKF, lnKB, and lnKW versus 1/T plot, lists a slope straight of (E/R) and, as shown in Figure 13, lnkio intercept opposed to 1/T. In the presence of sulfonic acid functionalized Ti SBA-15, the activation energy was found to be 39.5 kJ mol–1. The adsorption constants as function of temperature have arrived from Figure 13 as given in equations (7)–(9).
(6)KFL2g−1mol−1h−1=exp232–1109/T,(7)KBLmol−1=exp3125/T–17.83,(8)KwLmol−1=exp4856/T–54.9.Figure 13
Arrhenius plot forlnKb, lnkf, and lnKW vs. T.


### 4.6. Model Prediction

Model predictions with ER model have been compared with experimental results as shown in Figure14, for esterification of propionic acid with butanol over an entire range of expected parameters [24].Figure 14
Parity plot for rate of reaction from experimental data and model prediction.The following equation (9) is used to determine the experimental reaction rate for different time steps for various acid conversions.
(9)−rA,experimental=∆CA∆t=CAo∆X∆t.Figure14 shows the parity plot between the experimental value and the calculated values. It can be observed that the findings fall within ±5 percent error.


## 4.1. Effect of Reactant Molar Ratio

The mole ratio of propionic acid with n-butanol varied from 1 : 1 to 1 : 4 at a temperature of 115°C and a speed of 240 rpm for conversion of propionic acid with Ti-supported SBA-15 functionalized with sulfonic acid [18]. The conversion of propionic acid as function of molar ratio is shown in Figure 8. The propionic acid conversion increases as the molar ratio increases due to excess n-butanol. From the figure, it could be observed as 79.90%.Figure 8
Conversion versus time for different molar ratios. Other conditions are catalyst loading: 2%, temperature: 115°C, and speed: 240 rpm.


## 4.2. Effect of Temperature

The effect temperature on the conversion of propionic acid at 2% by wt catalyst loading and at 1 : 1 mole ratio is shown in Figure9. The conversion of propionic acid is increased as temperature increases. Higher the temperatures, the time required to reach equilibrium is lesser [19]. It shows that the reaction is kinetically controlled.Figure 9
Conversion versus time for different temperatures. Other conditions are catalyst loading: 2%, mole ratio: 1 : 1, and speed: 240 rpm.


## 4.3. Effect of Catalyst Amount

The effect of catalyst amount on the propionic acid conversion kinetics is shown in Figure10 at a temperature of and mole ratio of 1 : 1. The experiments employ separate catalyst concentrations of 1, 2, and 3 wt%. The conversion of propionic acid increases as the catalyst loading increases [20]. When the catalyst quantity increased in the reaction mixture, the reaction rate increases due to availability of H+ ions which in turn provide more catalyst surface area. The experiments were conducted for 4 runs with the same catalyst. The propionic acid conversion is the same under 1% error.Figure 10
Conversion vs. time (min) for different catalyst loadings. Other conditions are mole ratio: 1 : 1, temperature: 115°C, and speed: 240 rpm.


## 4.4. The Ti-Supported SBA-15 Functionalized with Sulfonic Acid for the Kinetic Analysis

The initial reaction rate of propionic acid with n-butanol has been carried out under different catalyst loadingsrAo=∆CAo/∆t for this catalyst [21]. The general kinetic expression for the catalyzed heterogeneous esterification reaction can be written as
(2)−rA=kfwcatCACB−CRCw/Keq1+KACA+KBCB+KECE+KwCwn,whererA is the reaction rate and wcat is the catalyst weight on dry basis. A, B, E, and W represent propionic acid, n-butanol, butyl propionate, and water. K is the adsorption constant, Ke is the equilibrium constant, and kf is the forward reaction rate constant. In equation (2), when n=0, it is a PH model; when n=1, it is ER model; and when n=2, it is a LHHW model.As can be seen in Figure11, the starting reaction rate instead of the plated one is a linear feature, which means the adsorption of propionic acid on the Ti-supported SBA-15 functionalized with sulfonic acid catalyst surface is not possible, and at the same time, the initial rate of reaction increases in line with n-butanol concentrations. Therefore, we can infer that at low concentrations of n-butanol, it adsorbed n-butanol extremely low and almost continuously increases the concentration. This study concludes that the reaction mechanism is defined in the Eley-Rideal model, i.e., reaction between adsorbed butanol molecules and propionic acid molecules in the bulk solution. In the single site, only one reactant is adsorbed on the catalyst and the remaining reactant is in the bulk reaction. In the double site, two reactants are at the catalyst surface and reaction proceed at this place and formed products desorbed from the catalyst surface. The literature found the solvent (dioxane) and ester adsorption to be insignificant. The rate determination step is to specifically take the stoichiometric and corresponding reaction rate as the Eley-Rideal (ER) model of a surface-reaction equation. After excluding terms of adsorption of acid and ester, ER form can be written as
(3)−rA=kfwcatCACB−CRCw/Keq1+KBCB+KwCw.Figure 11
The effect on the initial reaction rate of (−rAo) at different temperatures on the charging of catalyst.The Arrhenius law expresses the dependence of temperature on reaction rate as given in the following.Equation (3) behavior is used for speed expression rather than concentration, because the predictions of models adapted to the measured film data result in improved prediction [22]. Relocation of equation (4) can be described as equation for the initial reaction rate without a product present, shown in
(4)CAoCBo−rAo=1kfwcat+KBkfwcatCBo.Figure12 shows the plot of CAoCBo/−rAo versus CB,o results in a direct slope line KB/kfwcat and intercept 1/kfwcat as shown in the figure.Figure 12
CAoCBo/−rAo versus CB0 at different temperatures.Slopes and intercepts in these figures indicate the constants in rates and adsorption constantskF, KB, KW, and their estimated values at three temperatures as shown in Table 2.Table 2
Kinetics and adsorption constants.
Temperature (°C)kf/L2 mol-1 h-1KB/L mol-1KW/L mol-1850.78×10−40.180.19950.81×10−40.200.491050.78×10−40.190.511150.90×10−40.090.56


## 4.5. Activation Energy and Rate Constants

The Arrhenius law expresses the dependence of temperature on reaction rate as given in the following:(5)ki=kioexp−Ei/RT,wherekf is the activation energy for forward reaction and kio is the frequency factor [23]. Equation (5), a plot of lnKF, lnKB, and lnKW versus 1/T plot, lists a slope straight of (E/R) and, as shown in Figure 13, lnkio intercept opposed to 1/T. In the presence of sulfonic acid functionalized Ti SBA-15, the activation energy was found to be 39.5 kJ mol–1. The adsorption constants as function of temperature have arrived from Figure 13 as given in equations (7)–(9).
(6)KFL2g−1mol−1h−1=exp232–1109/T,(7)KBLmol−1=exp3125/T–17.83,(8)KwLmol−1=exp4856/T–54.9.Figure 13
Arrhenius plot forlnKb, lnkf, and lnKW vs. T.


## 4.6. Model Prediction

Model predictions with ER model have been compared with experimental results as shown in Figure14, for esterification of propionic acid with butanol over an entire range of expected parameters [24].Figure 14
Parity plot for rate of reaction from experimental data and model prediction.The following equation (9) is used to determine the experimental reaction rate for different time steps for various acid conversions.
(9)−rA,experimental=∆CA∆t=CAo∆X∆t.Figure14 shows the parity plot between the experimental value and the calculated values. It can be observed that the findings fall within ±5 percent error.


## 5. Conclusions

SBA-15, Ti, and -SO3H were successfully incorporated with a sol-gel process. It is found that final Ti-and-S contents were less than anticipated in samples. Moreover, the presence of sulphur decreases titanium’s inclusion in the SBA-15. Propionic acid reaction kinetics with n-butanol has been investigated with this catalyst. Experimental results indicate that the reaction is kinetic controlled instead of mass transfer controlled. Eley-Rideal (ER) was developed based on an adsorption analysis to interpret kinetic data. The kinetic model was well prepared with experimental results. The EA 29.63 kJ/mol activation energy and kinetic factor ko 0.549 L2/g-mol-h were found.



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