# Oxidative Dehydrogenation of n-Butane over LaV Catalysts Supported on TiO2

Authors: Le Minh Cam; Ngo Duc Huyen; Nguyen Ngoc Ha
Journal: Journal of Chemistry
 (2013)

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## Abstract

The catalytic performance of vanadia catalysts with 15 wt% V supported on TiO2 and (15 wt% V + 4.6 wt% La) supported on TiO2 in oxidative dehydrogenation (ODH) of n-butane was investigated. The catalysts were characterized by means of TPD-NH3, TPR-H2, UV-Vis, and BET. Testing of samples showed that vanadia catalysts were active for the reaction. It was found that La doping of V/TiO2 catalyst had a negative effect on the dispersion of V species and led to formation of V2O5 clusters. This resulted in a loss of activity. Although slight improvement of selectivity was observed in comparison to undoped V/TiO2 samples due to lower acidity of La-doped –V/TiO2, this could not compensate the loss of activity and finally did not lead to higher butene yields.


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## Body

## 1. Introduction

Oxidative dehydrogenation of light alkanes has been a research topic of consistent interest from the 1980s [1–3]. The presence of oxygen raises the thermodynamic restrictions of dehydrogenation, and the exothermic character of the reaction renders it an energetically efficient process [4, 5]. The development of efficient heterogeneous catalysts for the oxidative dehydrogenation of alkanes is of great importance because of the economic benefits of using light alkanes for the production of important base chemicals [6, 7]. In order to make the process commercially feasible, the main objective is to maximize the selectivity to alkenes, a significant issue, since the deep oxidation of alkanes and alkenes (reaction products) is thermodynamically favoured [8–11]. Experimental studies have proposed that the ODH reaction of C2–C4 alkane over transition metal based catalysts occurs following a Mars-van Krevelen redox mechanism [12] in which surface catalytic sites are reduced by hydrocarbon with participation of the lattice oxygen and followed by reoxidation with adsorbed O2 from the gas phase. It is well known that the catalyst behavior depends on a number factors, such as the chemical nature of the active species, the redox properties, and the acid-base character, which in turn depend on transition metal loading, dispersion, and support effects [13].In case of butane ODH, vanadium supported catalysts are considered good catalysts, and vanadium appears to be the selective catalytic site. The coordination of vanadium in the active centres and the density of the active sites belong to the most important factors determining the catalytic performance of V catalysts. It has been postulated in the literature that tetrahedrally coordinated V centres are more selective but less active than octahedral ones [14]. However, there are discrepancies between different authors whether isolated VO4 tetrahedra are more effective than units possessing V–O–V entities. The concentration of vanadium phase on the catalyst surface depends on the method of preparation and on the nature and amounts of supports or promoters eventually added to that active phase [15–19]. Very good results for vanadium dispersion and catalytic properties have been obtained by preparing the TiO2–SiO2 support by grafting [20]. The literature provides some information on both the method of anchoring vanadium on SiO2 and TiO2–SiO2 and the properties of the obtained catalysts, but there is very little information about the vanadium alkoxide-support interaction, the relationship between dispersion and vanadium load, the amount of adsorbed vanadium corresponding to the monolayer, and the effect of calcination on surface modification. Lakshmi et al. [21] have used the sol-gel method to prepare vanadium catalysts supported on TiO2–SiO2 and Zr2O–SiO2. Murgia et al. [15] suggested that a preparation method, which causes the vanadium to be distributed homogeneously at the surface and in the bulk, was preferred over a method which deposits vanadium only at the surface. The investigation of the catalytic properties of vanadia supported catalysts in propane ODH showed that more selective catalysts were obtained on basic metal oxide supports [13]. The presence of basic sites enhances the fast desorption of the produced olefins from the catalytic surface, resulting in higher selectivities. Furthermore, Galli et al. [22] demonstrated that doping vanadia catalysts with basic promoters has a beneficial effect in n-butane ODH by increasing the olefin selectivity.It is well know that titania allows to obtain a very good dispersion of V2O5 on its surface [16]. The literature data [23, 24] reported high activity of the V2O5/TiO2 system in the oxidative conversion of propane at relatively low temperature (500–600 K). The addition of potassium to the TiO2, in particular anatase, provides an optimal chemical environment for the vanadium oxide catalytic action. Grzybowska et al. [24] suggested that the potassium hinders the formation of the electrophilic O− species responsible for total oxidation of hydrocarbon. The butane oxidation over both monolayer and multilayer vanadia on TiO2 has been reported [25, 26].In the present paper, vanadia catalysts prepared by impregnating ammonium vanadate on a titania support were investigated. We report catalytic results obtained with 15% V catalyst supported on TiO2 for the oxidative dehydrogenation (ODH) of n-butane. Our goal was to examine the effect of active metal at loadings exceeding a theoretical monolayer coverage. To study the effect of promoter on the catalytic performance, a sample of V/TiO2 with addition of 5 wt% La2O3 (equivalent to 4.6 wt% La) was prepared. The reason for choosing La is to investigate the effect of La doping on the acid-base property of the catalyst. Due to the basicity of La2O3 [27] we expect the catalytic behaviour of the La-containing V/TiO2 to be different from that of La-free V/TiO2.


## 2. Experimental

### 2.1. Catalysts Preparation and Characterization

A commercial TiO2 (anatase Aldrich) was used as a support. Vanadium oxide was deposited on the support by wet impregnation using aqueous NH4VO3 (Merck) solution. Prior to impregnation the TiO2 support was calcined at 600°C for 3 hours. An aqueous solution of ammonium metavanadate was prepared and heated slowly. Oxalic acid (Merck) was added to the solutions (NH4VO3/oxalic acid = (1/2) molar) to ensure dissolution of precursor. The nominal weight loading of V was 15 wt.%. This solution was then added to an aqueous TiO2 slurry. The resulting solution was stirred and heated until all the water was evaporated. Sample was dried overnight and calcined in air at 600°C for 4 hours. The catalyst is denoted by VT. LaV-containing TiO2 was prepared from slurries containing aqueous solutions of ammonium metavanadate and lanthanum chloride (Aldrich). The solid obtained was then heat-treated in flow oxygen at 600°C for 4 hours (named as LaVT). The nominal weight loading of La2O3 was 5 wt%.Powder X-ray diffraction (XRD) patterns were obtained using a BRUCKER D8-Advance 5005 diffractometer and Cu Kα radiation.Specific surface areas were measured by the multipoint BET analysis method using N2 adsorption isotherms at 77 K. The measurement was performed on TriStar 3000 analyser (Micromeritics).Temperature programmed reduction (TPR) experiments with H2 were carried out in a gas flow system. NH3-temperature programmed desorption (NH3-TPD) was used to determine the acid properties. The H2-TPR and NH3-TPD experiments were carried out using a Micromeritics model AutoChem II 2920. UV-Vis spectra of fresh catalysts were collected using a Cary 5000 Varian equipment.


### 2.2.  Catalytic Tests

ODH of n-butane was performed in a fixed-bed quartz tubular reactor at atmospheric pressure and under steady state conditions. The catalyst samples (0.2 g with a 0.5 to 0.7 mm particle size) and silicon carbide were packed into the reactor to maintain a constant volume in the catalytic bed. The flow rate was 32 mL/min, and the feed comprised a mixture of n-butane, oxygen, and nitrogen with a volume ratio of 3 : 1 : 6. The reaction temperature range varied between 400°C and 550°C to achieve different conversion levels. Reactants and reaction products were analyzed in line using Trace Gas Chromatograph Ultra RGA (Thermo Scientific) equipped with a thermal conductivity detector (TCD). Three columns in a series-bypass configuration were used in the analysis: BEEA, 27.5% on Chromosorb PAW, Hayesep Q, and Mol Sieve 5A. Conversions(C) and the selectivities (S) to the reaction products were defined as follows:
(1)C=(moln-butanereactedmoln-butaneinthefeed)×100,S=(moln-butaneconvertedtoimoln-butanereacted)×100,
where i = C4H8, CO, CO2, and others (CH4, C2H6, C3H8, C3H6, etc.).Blank runs carried out in the empty-volume reactor at 550°C allowed ruling out the occurrence of gas-phase reactions to a significant extent at the experimental conditions used for the activity tests. The dehydrogenation of n-butane had also been performed on the catalysts in the absence of oxygen in the feed. The obtained conversions can be negligible (<5%). Also the ODH of n-butane was tested over pristine TiO2, and the obtained results indicated a very poor catalytic activity.


## 2.1. Catalysts Preparation and Characterization

A commercial TiO2 (anatase Aldrich) was used as a support. Vanadium oxide was deposited on the support by wet impregnation using aqueous NH4VO3 (Merck) solution. Prior to impregnation the TiO2 support was calcined at 600°C for 3 hours. An aqueous solution of ammonium metavanadate was prepared and heated slowly. Oxalic acid (Merck) was added to the solutions (NH4VO3/oxalic acid = (1/2) molar) to ensure dissolution of precursor. The nominal weight loading of V was 15 wt.%. This solution was then added to an aqueous TiO2 slurry. The resulting solution was stirred and heated until all the water was evaporated. Sample was dried overnight and calcined in air at 600°C for 4 hours. The catalyst is denoted by VT. LaV-containing TiO2 was prepared from slurries containing aqueous solutions of ammonium metavanadate and lanthanum chloride (Aldrich). The solid obtained was then heat-treated in flow oxygen at 600°C for 4 hours (named as LaVT). The nominal weight loading of La2O3 was 5 wt%.Powder X-ray diffraction (XRD) patterns were obtained using a BRUCKER D8-Advance 5005 diffractometer and Cu Kα radiation.Specific surface areas were measured by the multipoint BET analysis method using N2 adsorption isotherms at 77 K. The measurement was performed on TriStar 3000 analyser (Micromeritics).Temperature programmed reduction (TPR) experiments with H2 were carried out in a gas flow system. NH3-temperature programmed desorption (NH3-TPD) was used to determine the acid properties. The H2-TPR and NH3-TPD experiments were carried out using a Micromeritics model AutoChem II 2920. UV-Vis spectra of fresh catalysts were collected using a Cary 5000 Varian equipment.


## 2.2.  Catalytic Tests

ODH of n-butane was performed in a fixed-bed quartz tubular reactor at atmospheric pressure and under steady state conditions. The catalyst samples (0.2 g with a 0.5 to 0.7 mm particle size) and silicon carbide were packed into the reactor to maintain a constant volume in the catalytic bed. The flow rate was 32 mL/min, and the feed comprised a mixture of n-butane, oxygen, and nitrogen with a volume ratio of 3 : 1 : 6. The reaction temperature range varied between 400°C and 550°C to achieve different conversion levels. Reactants and reaction products were analyzed in line using Trace Gas Chromatograph Ultra RGA (Thermo Scientific) equipped with a thermal conductivity detector (TCD). Three columns in a series-bypass configuration were used in the analysis: BEEA, 27.5% on Chromosorb PAW, Hayesep Q, and Mol Sieve 5A. Conversions(C) and the selectivities (S) to the reaction products were defined as follows:
(1)C=(moln-butanereactedmoln-butaneinthefeed)×100,S=(moln-butaneconvertedtoimoln-butanereacted)×100,
where i = C4H8, CO, CO2, and others (CH4, C2H6, C3H8, C3H6, etc.).Blank runs carried out in the empty-volume reactor at 550°C allowed ruling out the occurrence of gas-phase reactions to a significant extent at the experimental conditions used for the activity tests. The dehydrogenation of n-butane had also been performed on the catalysts in the absence of oxygen in the feed. The obtained conversions can be negligible (<5%). Also the ODH of n-butane was tested over pristine TiO2, and the obtained results indicated a very poor catalytic activity.


## 3. Results

### 3.1. Catalyst Characterization

#### 3.1.1. X-Ray Diffractions

The X-ray diffraction patterns of pure TiO2, VT, and LaVT samples were displayed in Figure 1. The solids corresponded to well-crystallized pure phase. The characteristic peak at ca. 2θ = 25.4° corresponding to (101) plane of anatase phase is clearly observed in all samples. For the pure one, no peak brookite phases of TiO2 are observed, and peak for rutile is also hardly seen. However, weak peaks for rutile are clearly detected in XRD pattern of VT and LaVT samples indicating an interaction between active phase and the support. As it can be seen, for VT and LaVT catalysts, crystalline V2O5 was detected, and an increase in the intensity of the anatase reflex, at 25.4°, can be observed. This phenomenon has already been observed [20]. That is, when vanadium is not uniformly dispersed on the surface it promoted the formation of anatase crystallites during the catalyst calcination. Sample with low lanthanum loading did not show any diffraction lines corresponding to La-containing compound suggesting that XRD analysis cannot give information about the molecular dispersion of La species.Figure 1
XRD patterns of TiO2, VT, and LaVT samples.


#### 3.1.2. BET Measurements

The characteristic properties of the catalytic materials prepared are shown in Table1. It was found that the modification of parent samples did not significantly change the structure of these materials. The changes in SBET illustrate a pronounced reduction of the surface due to the vanadium oxide impregnation. The surface area of the samples varied from 56 m2/g (parent TiO2) to 27 m2/g for VT and to 11 m2/g for LaVT. This could be explained as follows: at high calcination temperature, big crystallites of V2O5 and additional crystalline LaVO4 were formed. The formation of crystalline V2O5 as well as vanadate of La could be a reason for the drastic decrease of BET surface areas. However, the process of phase separation, being associated with a loss of specific surface area, could not be suppressed by doping with La, and thus La has no stabilising influence on the V centres.Table 1
Results of physicochemical characterization of studied samples.
Samples
S
BET (m2/g)
NH3 desorption (cm3/g)
H2 consumption
VT
27
4.33
28.67
LaVT
11
3.72
38.18


#### 3.1.3. UV-Vis Spectra

The UV-Vis spectroscopy provides information about the character and oxidation state of vanadium. The obtained UV-Vis spectra for both prepared samples are presented in Figure2. For quantitative analysis of all types of surface vanadium complexes, the spectra were deconvoluted into individual bands. The deconvolution spectra, using symmetric Gaussian curves, showed that bands related to the tetrahedral and octahedral species were observed for all solids. The octahedral species were related to V5+ ions which present characteristic absorption bands between 350 and 500 nm, while highly dispersed tetrahedral species of V5+ could be related to contributions between 280 and 340 nm [15, 16]. In present work, we suggest that the bands observed at 244.3 nm (for VT) and 246.1 nm (for LaVT) correspond to titanium ions in octahedral coordination [28]. The band at 218 nm originated from isolated VO4 tetrahedra. For VT catalyst, absorption bands around 300–350 nm can be assigned to charge transfer transitions of tetrahedrally coordinated V5+ species [15, 16]. But the position of the third band (336.4 nm) suggested that the VOx species are low oligomeric VO4 tetrahedra rather than isolated. The band at 400–430 nm pointed to the presence of V5+ in octahedral coordination. The small absorption around 480 originates most likely from some polymeric octahedrally coordinated vanadium sites. Low intensity of this band suggested that the octahedral V species play only a minor role in this material.UV-Vis spectra of VT (a) and LaVT (b).
(a)
(b)The UV-Vis spectrum of the La-doped V/TiO2 catalyst was quite similar to that of the undoped one. However the relative intensity of the band around 300–350 nm was lower than that in the undoped suggesting that tetrahedral V centres might also be polymerized lower than La-free sample. Moreover the relative intensity of the band around 450 nm, indicating the presence of higher coordinated V species, is much higher than that in undoped VOx/TiO2 sample, and its relative intensity with respect to the overall UV-vis intensity was the highest in comparison to other bands. This indicates that La does not support the dispersion of V sites.


#### 3.1.4. H2-TPR Spectra

The reducibility of the catalysts was measured by means of H2-TPR. The H2-TPR of VT and LaVT were plotted in Figure 3. For comparison, the H2-TPR profiles of parent TiO2 and pure V2O5 were also plotted. It is clear that TiO2 was hardly reduced at the temperatures lower than 800°C. In pure V2O5 the first reduction peak appeared at above 600°C. However lower reduction temperatures were observed in VT and LaVT catalyst samples indicating the interaction between active sites and the support.Figure 3
A comparison of H2-TPR spectra obtained for LaVT, VT, parent TiO2, and pure V2O5.The deconvolutions of H2-TPR profiles of VT and LaVT were shown in Figure 4. The TPR profiles of VT and LaVT consisted of several peaks. This points to the presence of different VOx species, differing in their reduction stability, and is in agreement with the results of UV-Vis and XRD. The existence of VO4 isolated species was confirmed by TPR of the studied samples. According in the literature [7] the first reduction peak is ascribable to the reduction of surface V5+ species in distorted VO4 species while the high temperature would correspond to the reduction of V5+ belonging to the bulk orthovanadate. In VT the TPR deconvolution showed reduction peaks centred at 496.4°C and 570.9°C. In LaVT these peaks shifted to higher temperatures 528°C and 608°C. In the same order, the vanadium dispersion decreased owing to a dramatic loss of surface area, which favours the formation of polymerised V species or even crystalline vanadates of La. Therefore, the TPR results indicated that less polymerised vanadium species can be move easily reduced than V centres in condensed phases. The peaks appearing at around 743°C for LaVT and 628°C for VT arose probably from the reduction of crystalline V2O5 and LaVO4 [29].H2-TPR profiles of VT (a) and LaVT (b) catalysts.
(a)
(b)


#### 3.1.5.  NH3-TPD

The surface acidic properties of VT and LaVT samples investigated by NH3-PTD were compiled in Figure 5. The NH3 desorption patterns which indicated acid sites of weak and moderate strengths were present on the catalysts. However, the presence of La decreased the moderate acid sites, and also the total NH3 desorption in LaVT sample (3.72 mL/g catalyst) was lower than that in VT sample (4.33 mL NH3/g catalyst). The obtained results suggested that the surface acidity of the LaVT sample was diminished by La doping.NH3-temperature programmed desorption profiles of the catalytic samples: (a) VT; (b) LaVT.
(a)
(b)


### 3.2. Catalytic Tests for n-Butane Oxidative Dehydrogenation

#### 3.2.1. Catalytic Activity

Table2 shows conversion of n-butane and the distribution of reaction products, obtained at each temperature over VT and LaVT catalysts. For comparison, the conversion of n-butane over pristine TiO2 and bulk V2O5 is also presented, but the obtained conversions can be negligible. Figure 6 shows the variation in n-butane conversion and total alkene’s selectivity with the reaction temperature.Table 2
Results of catalytic tests in ODH of n-butane (C4H10/O2/N2 = 30/10/60 vol. %, total flow rate 32 mL/min).
T (°C)
Catalyst
Conv. (%)
1-b
2-trans
2-cis
C4-1,3
C
O
x
400
LaVT
9.97
24.99
15.42
10.73
0
26.43
VT
10.48
27.11
13.13
7.96
0
25.02
Parent TiO2
Not observed
Bulk V2O5
Not observed
450
LaVT
14.95
19.83
14.29
10.28
0
21.15
VT
16.64
18.67
9.30
5.80
0
19.70
Parent TiO2
Not observed
Bulk V2O5
Not observed
500
LaVT
16.72
19.66
12.01
8.42
1.96
19.17
VT
18.71
17.59
9.42
6.22
1.38
19.34
Parent TiO2
Not observed
Bulk V2O5
0.94
550
LaVT
19.63
19.87
9.99
6.68
2.52
15.77
VT
21.19
17.96
8.57
5.25
0
15.72
Parent TiO2
3.73
Bulk V2O5
5.76Conversion (a) and total alkene’s selectivity (b) as functions of reaction temperature for VT and LaVT.
(a)
(b)From data reported in Table2 the major products formed under reaction conditions with 10% O2 as coreactant were 1-butene (1-b), tran-2-butene (2-trans), cis-2-butene (2-cis), butadiene, (C4-1,3) CO2, CO, and cracking products (methane, ethane, ethane, and propene). It is possible to observe an effect of the support on the activities and selectivities of vanadium based catalysts in the ODH of n-butane in agreement with the observations of many different authors reported in the literature [30]. Generally, the conversions increase with the temperature, whereas the selectivities decrease, as usual, with the conversion. Also, it was demonstrated that [20] the activity of the dispersed catalysts can be roughly related to the vanadium load. Santacesaria et al. [20] reported a conversion of 3.2% and corresponding selectivity of 51.1% obtained for the ODH of n-butane over a 5% V/TiO2 catalyst at 500°C. However, their experimental conditions differed from those in this work: the content of V was 5% (wt.), and catalyst weight was 0.05 g (meanwhile they are 15% and 0.2 g, resp., in this work); in their work, the total feed low rate was 150 mL/min, and O2/C4H10 ratio was 1.7. Therefore the differences in catalytic behaviour between our samples and theirs are quite reasonable.It can be seen that, at the same vanadium loading, although La-freeVOx/TiO2 (VT) catalyst is slightly less selective than the respective VOxLa/TiO2 (LaVT) sample in the studied temperature range (400–550°C), it is slightly more active (in terms of butane conversion) than the LaVT. It can be readily seen in Figure 7 that the intrinsic activity evidenced by surface area specific rates (R) and the corresponding turnover of the catalysts have a tendency to increase with the temperature. Moreover it can be seen that LaVT presented a lower activity compared to that of VT catalyst. This trend points to a decreasing number of ODH sites with LaVT. Since present characterizations of the materials indicated higher crystallinities in LaVT than in VT, the trend of turnover values and specific activities in Figure 7 was consistent with an inverse relationship between crystallinity and turnover and specific activity.Variation of turnover (in mol C4 h−1 (molV)−1) and the specific rate (in mol C4 h−1 m−2) with undoped and La-doped VOx/TiO2.
(a)
(b)


#### 3.2.2. Product’s Distribution

Variation of the selectivity to the main reaction products as a function of temperature on both samples was presented in Table2. Results in Table 2 showed that over both catalyst samples CO2 and CO were formed at low butane conversion. This is in agreement with the reports of Murgia et al. [15]. Products COx were slightly decreased as conversion increased. Figures 8 and 9 plot the product distrubitions against reaction temperatures. For VT sample the main reaction product was 1-butene in the whole range of studied temperatures while no measurable selectivity toward butadiene was found. Dias et al. [7] studied ODH of n-butane over Mg-V catalysts and showed that 1-butene was a main product; however for higher reaction temperatures (above 748 K) butadiene was a major product. The selectivity towards 2-butenes was always lower than selectivity towards 1-butene. Similar results were observed by Murgia et al. [15] and Jackson and Rugmini [9]. The ratio tran/cis was approximately constant and equal to 1.42. An analogous ratio for the ODH of n-butane over 5 wt.% V2O5/TiO2 was reported by Santacesaria et al. [20]. Figures 6 and 8 showed that the selectivity towards butenes decreased as conversion increased due to the consecutive reactions. Similar trends are observable for other catalysts reported in the literature [16, 20]; that is, conversion increases with the residence time, while selectivity to alkene products decreases.The distribution of alkene’s products with the reaction temperatures.
(a)
(b)Figure 9
Product selectivity over VT and LaVT catalysts at 550°C.The catalytic behaviour of LaVT sample was similar to VT sample. Taking into account the surface acidity of the samples, the LaVT exposed a higher selectivity than VT. The reaction products distribution was approximately the same: 1-butene was the main product, and the ratio trans/cis was constant and equal to 1.6. Especially, LaVT produced butadiene. Butadiene was formed by consecutive reactions, and competition due to carbon oxide formation from both butyl radicals and butenes [31].Figure9 shows the selectivities of alkenes over LaVT and VT catalysts samples at 550°C. It can be seen that the LaVT has a slightly higher selectivity of alkenes than VT.The catalytic behaviour of LaVT sample could be attributed to the following.(i)
Doping La resulted in an increase in basicity of catalyst sample (TPD-NH3 results), and it was expected that this change will affect the catalyst selectivity but not the activity. The best selectivity induced by the presence of La2O3 is a well-known phenomenon described in the literature [27]. Hoang et al. [27] studying the ODH of isobutane over chromium oxide base catalysts indicated that, when La2O3 is present in the support, the activity is low, but the selectivity was almost 100%.(ii)
The presence of La species lowers the surface area and thus also the surface vanadium dispersion due to blocking active sites (BET measurement and UV-Vis spectra) and increased reduction temperatures (TPR-H2 results). These may have a negative effect on the catalytic performance of VT catalyst.


## 3.1. Catalyst Characterization

### 3.1.1. X-Ray Diffractions

The X-ray diffraction patterns of pure TiO2, VT, and LaVT samples were displayed in Figure 1. The solids corresponded to well-crystallized pure phase. The characteristic peak at ca. 2θ = 25.4° corresponding to (101) plane of anatase phase is clearly observed in all samples. For the pure one, no peak brookite phases of TiO2 are observed, and peak for rutile is also hardly seen. However, weak peaks for rutile are clearly detected in XRD pattern of VT and LaVT samples indicating an interaction between active phase and the support. As it can be seen, for VT and LaVT catalysts, crystalline V2O5 was detected, and an increase in the intensity of the anatase reflex, at 25.4°, can be observed. This phenomenon has already been observed [20]. That is, when vanadium is not uniformly dispersed on the surface it promoted the formation of anatase crystallites during the catalyst calcination. Sample with low lanthanum loading did not show any diffraction lines corresponding to La-containing compound suggesting that XRD analysis cannot give information about the molecular dispersion of La species.Figure 1
XRD patterns of TiO2, VT, and LaVT samples.


### 3.1.2. BET Measurements

The characteristic properties of the catalytic materials prepared are shown in Table1. It was found that the modification of parent samples did not significantly change the structure of these materials. The changes in SBET illustrate a pronounced reduction of the surface due to the vanadium oxide impregnation. The surface area of the samples varied from 56 m2/g (parent TiO2) to 27 m2/g for VT and to 11 m2/g for LaVT. This could be explained as follows: at high calcination temperature, big crystallites of V2O5 and additional crystalline LaVO4 were formed. The formation of crystalline V2O5 as well as vanadate of La could be a reason for the drastic decrease of BET surface areas. However, the process of phase separation, being associated with a loss of specific surface area, could not be suppressed by doping with La, and thus La has no stabilising influence on the V centres.Table 1
Results of physicochemical characterization of studied samples.
Samples
S
BET (m2/g)
NH3 desorption (cm3/g)
H2 consumption
VT
27
4.33
28.67
LaVT
11
3.72
38.18


### 3.1.3. UV-Vis Spectra

The UV-Vis spectroscopy provides information about the character and oxidation state of vanadium. The obtained UV-Vis spectra for both prepared samples are presented in Figure2. For quantitative analysis of all types of surface vanadium complexes, the spectra were deconvoluted into individual bands. The deconvolution spectra, using symmetric Gaussian curves, showed that bands related to the tetrahedral and octahedral species were observed for all solids. The octahedral species were related to V5+ ions which present characteristic absorption bands between 350 and 500 nm, while highly dispersed tetrahedral species of V5+ could be related to contributions between 280 and 340 nm [15, 16]. In present work, we suggest that the bands observed at 244.3 nm (for VT) and 246.1 nm (for LaVT) correspond to titanium ions in octahedral coordination [28]. The band at 218 nm originated from isolated VO4 tetrahedra. For VT catalyst, absorption bands around 300–350 nm can be assigned to charge transfer transitions of tetrahedrally coordinated V5+ species [15, 16]. But the position of the third band (336.4 nm) suggested that the VOx species are low oligomeric VO4 tetrahedra rather than isolated. The band at 400–430 nm pointed to the presence of V5+ in octahedral coordination. The small absorption around 480 originates most likely from some polymeric octahedrally coordinated vanadium sites. Low intensity of this band suggested that the octahedral V species play only a minor role in this material.UV-Vis spectra of VT (a) and LaVT (b).
(a)
(b)The UV-Vis spectrum of the La-doped V/TiO2 catalyst was quite similar to that of the undoped one. However the relative intensity of the band around 300–350 nm was lower than that in the undoped suggesting that tetrahedral V centres might also be polymerized lower than La-free sample. Moreover the relative intensity of the band around 450 nm, indicating the presence of higher coordinated V species, is much higher than that in undoped VOx/TiO2 sample, and its relative intensity with respect to the overall UV-vis intensity was the highest in comparison to other bands. This indicates that La does not support the dispersion of V sites.


### 3.1.4. H2-TPR Spectra

The reducibility of the catalysts was measured by means of H2-TPR. The H2-TPR of VT and LaVT were plotted in Figure 3. For comparison, the H2-TPR profiles of parent TiO2 and pure V2O5 were also plotted. It is clear that TiO2 was hardly reduced at the temperatures lower than 800°C. In pure V2O5 the first reduction peak appeared at above 600°C. However lower reduction temperatures were observed in VT and LaVT catalyst samples indicating the interaction between active sites and the support.Figure 3
A comparison of H2-TPR spectra obtained for LaVT, VT, parent TiO2, and pure V2O5.The deconvolutions of H2-TPR profiles of VT and LaVT were shown in Figure 4. The TPR profiles of VT and LaVT consisted of several peaks. This points to the presence of different VOx species, differing in their reduction stability, and is in agreement with the results of UV-Vis and XRD. The existence of VO4 isolated species was confirmed by TPR of the studied samples. According in the literature [7] the first reduction peak is ascribable to the reduction of surface V5+ species in distorted VO4 species while the high temperature would correspond to the reduction of V5+ belonging to the bulk orthovanadate. In VT the TPR deconvolution showed reduction peaks centred at 496.4°C and 570.9°C. In LaVT these peaks shifted to higher temperatures 528°C and 608°C. In the same order, the vanadium dispersion decreased owing to a dramatic loss of surface area, which favours the formation of polymerised V species or even crystalline vanadates of La. Therefore, the TPR results indicated that less polymerised vanadium species can be move easily reduced than V centres in condensed phases. The peaks appearing at around 743°C for LaVT and 628°C for VT arose probably from the reduction of crystalline V2O5 and LaVO4 [29].H2-TPR profiles of VT (a) and LaVT (b) catalysts.
(a)
(b)


### 3.1.5.  NH3-TPD

The surface acidic properties of VT and LaVT samples investigated by NH3-PTD were compiled in Figure 5. The NH3 desorption patterns which indicated acid sites of weak and moderate strengths were present on the catalysts. However, the presence of La decreased the moderate acid sites, and also the total NH3 desorption in LaVT sample (3.72 mL/g catalyst) was lower than that in VT sample (4.33 mL NH3/g catalyst). The obtained results suggested that the surface acidity of the LaVT sample was diminished by La doping.NH3-temperature programmed desorption profiles of the catalytic samples: (a) VT; (b) LaVT.
(a)
(b)


## 3.1.1. X-Ray Diffractions

The X-ray diffraction patterns of pure TiO2, VT, and LaVT samples were displayed in Figure 1. The solids corresponded to well-crystallized pure phase. The characteristic peak at ca. 2θ = 25.4° corresponding to (101) plane of anatase phase is clearly observed in all samples. For the pure one, no peak brookite phases of TiO2 are observed, and peak for rutile is also hardly seen. However, weak peaks for rutile are clearly detected in XRD pattern of VT and LaVT samples indicating an interaction between active phase and the support. As it can be seen, for VT and LaVT catalysts, crystalline V2O5 was detected, and an increase in the intensity of the anatase reflex, at 25.4°, can be observed. This phenomenon has already been observed [20]. That is, when vanadium is not uniformly dispersed on the surface it promoted the formation of anatase crystallites during the catalyst calcination. Sample with low lanthanum loading did not show any diffraction lines corresponding to La-containing compound suggesting that XRD analysis cannot give information about the molecular dispersion of La species.Figure 1
XRD patterns of TiO2, VT, and LaVT samples.


## 3.1.2. BET Measurements

The characteristic properties of the catalytic materials prepared are shown in Table1. It was found that the modification of parent samples did not significantly change the structure of these materials. The changes in SBET illustrate a pronounced reduction of the surface due to the vanadium oxide impregnation. The surface area of the samples varied from 56 m2/g (parent TiO2) to 27 m2/g for VT and to 11 m2/g for LaVT. This could be explained as follows: at high calcination temperature, big crystallites of V2O5 and additional crystalline LaVO4 were formed. The formation of crystalline V2O5 as well as vanadate of La could be a reason for the drastic decrease of BET surface areas. However, the process of phase separation, being associated with a loss of specific surface area, could not be suppressed by doping with La, and thus La has no stabilising influence on the V centres.Table 1
Results of physicochemical characterization of studied samples.
Samples
S
BET (m2/g)
NH3 desorption (cm3/g)
H2 consumption
VT
27
4.33
28.67
LaVT
11
3.72
38.18


## 3.1.3. UV-Vis Spectra

The UV-Vis spectroscopy provides information about the character and oxidation state of vanadium. The obtained UV-Vis spectra for both prepared samples are presented in Figure2. For quantitative analysis of all types of surface vanadium complexes, the spectra were deconvoluted into individual bands. The deconvolution spectra, using symmetric Gaussian curves, showed that bands related to the tetrahedral and octahedral species were observed for all solids. The octahedral species were related to V5+ ions which present characteristic absorption bands between 350 and 500 nm, while highly dispersed tetrahedral species of V5+ could be related to contributions between 280 and 340 nm [15, 16]. In present work, we suggest that the bands observed at 244.3 nm (for VT) and 246.1 nm (for LaVT) correspond to titanium ions in octahedral coordination [28]. The band at 218 nm originated from isolated VO4 tetrahedra. For VT catalyst, absorption bands around 300–350 nm can be assigned to charge transfer transitions of tetrahedrally coordinated V5+ species [15, 16]. But the position of the third band (336.4 nm) suggested that the VOx species are low oligomeric VO4 tetrahedra rather than isolated. The band at 400–430 nm pointed to the presence of V5+ in octahedral coordination. The small absorption around 480 originates most likely from some polymeric octahedrally coordinated vanadium sites. Low intensity of this band suggested that the octahedral V species play only a minor role in this material.UV-Vis spectra of VT (a) and LaVT (b).
(a)
(b)The UV-Vis spectrum of the La-doped V/TiO2 catalyst was quite similar to that of the undoped one. However the relative intensity of the band around 300–350 nm was lower than that in the undoped suggesting that tetrahedral V centres might also be polymerized lower than La-free sample. Moreover the relative intensity of the band around 450 nm, indicating the presence of higher coordinated V species, is much higher than that in undoped VOx/TiO2 sample, and its relative intensity with respect to the overall UV-vis intensity was the highest in comparison to other bands. This indicates that La does not support the dispersion of V sites.


## 3.1.4. H2-TPR Spectra

The reducibility of the catalysts was measured by means of H2-TPR. The H2-TPR of VT and LaVT were plotted in Figure 3. For comparison, the H2-TPR profiles of parent TiO2 and pure V2O5 were also plotted. It is clear that TiO2 was hardly reduced at the temperatures lower than 800°C. In pure V2O5 the first reduction peak appeared at above 600°C. However lower reduction temperatures were observed in VT and LaVT catalyst samples indicating the interaction between active sites and the support.Figure 3
A comparison of H2-TPR spectra obtained for LaVT, VT, parent TiO2, and pure V2O5.The deconvolutions of H2-TPR profiles of VT and LaVT were shown in Figure 4. The TPR profiles of VT and LaVT consisted of several peaks. This points to the presence of different VOx species, differing in their reduction stability, and is in agreement with the results of UV-Vis and XRD. The existence of VO4 isolated species was confirmed by TPR of the studied samples. According in the literature [7] the first reduction peak is ascribable to the reduction of surface V5+ species in distorted VO4 species while the high temperature would correspond to the reduction of V5+ belonging to the bulk orthovanadate. In VT the TPR deconvolution showed reduction peaks centred at 496.4°C and 570.9°C. In LaVT these peaks shifted to higher temperatures 528°C and 608°C. In the same order, the vanadium dispersion decreased owing to a dramatic loss of surface area, which favours the formation of polymerised V species or even crystalline vanadates of La. Therefore, the TPR results indicated that less polymerised vanadium species can be move easily reduced than V centres in condensed phases. The peaks appearing at around 743°C for LaVT and 628°C for VT arose probably from the reduction of crystalline V2O5 and LaVO4 [29].H2-TPR profiles of VT (a) and LaVT (b) catalysts.
(a)
(b)


## 3.1.5.  NH3-TPD

The surface acidic properties of VT and LaVT samples investigated by NH3-PTD were compiled in Figure 5. The NH3 desorption patterns which indicated acid sites of weak and moderate strengths were present on the catalysts. However, the presence of La decreased the moderate acid sites, and also the total NH3 desorption in LaVT sample (3.72 mL/g catalyst) was lower than that in VT sample (4.33 mL NH3/g catalyst). The obtained results suggested that the surface acidity of the LaVT sample was diminished by La doping.NH3-temperature programmed desorption profiles of the catalytic samples: (a) VT; (b) LaVT.
(a)
(b)


## 3.2. Catalytic Tests for n-Butane Oxidative Dehydrogenation

### 3.2.1. Catalytic Activity

Table2 shows conversion of n-butane and the distribution of reaction products, obtained at each temperature over VT and LaVT catalysts. For comparison, the conversion of n-butane over pristine TiO2 and bulk V2O5 is also presented, but the obtained conversions can be negligible. Figure 6 shows the variation in n-butane conversion and total alkene’s selectivity with the reaction temperature.Table 2
Results of catalytic tests in ODH of n-butane (C4H10/O2/N2 = 30/10/60 vol. %, total flow rate 32 mL/min).
T (°C)
Catalyst
Conv. (%)
1-b
2-trans
2-cis
C4-1,3
C
O
x
400
LaVT
9.97
24.99
15.42
10.73
0
26.43
VT
10.48
27.11
13.13
7.96
0
25.02
Parent TiO2
Not observed
Bulk V2O5
Not observed
450
LaVT
14.95
19.83
14.29
10.28
0
21.15
VT
16.64
18.67
9.30
5.80
0
19.70
Parent TiO2
Not observed
Bulk V2O5
Not observed
500
LaVT
16.72
19.66
12.01
8.42
1.96
19.17
VT
18.71
17.59
9.42
6.22
1.38
19.34
Parent TiO2
Not observed
Bulk V2O5
0.94
550
LaVT
19.63
19.87
9.99
6.68
2.52
15.77
VT
21.19
17.96
8.57
5.25
0
15.72
Parent TiO2
3.73
Bulk V2O5
5.76Conversion (a) and total alkene’s selectivity (b) as functions of reaction temperature for VT and LaVT.
(a)
(b)From data reported in Table2 the major products formed under reaction conditions with 10% O2 as coreactant were 1-butene (1-b), tran-2-butene (2-trans), cis-2-butene (2-cis), butadiene, (C4-1,3) CO2, CO, and cracking products (methane, ethane, ethane, and propene). It is possible to observe an effect of the support on the activities and selectivities of vanadium based catalysts in the ODH of n-butane in agreement with the observations of many different authors reported in the literature [30]. Generally, the conversions increase with the temperature, whereas the selectivities decrease, as usual, with the conversion. Also, it was demonstrated that [20] the activity of the dispersed catalysts can be roughly related to the vanadium load. Santacesaria et al. [20] reported a conversion of 3.2% and corresponding selectivity of 51.1% obtained for the ODH of n-butane over a 5% V/TiO2 catalyst at 500°C. However, their experimental conditions differed from those in this work: the content of V was 5% (wt.), and catalyst weight was 0.05 g (meanwhile they are 15% and 0.2 g, resp., in this work); in their work, the total feed low rate was 150 mL/min, and O2/C4H10 ratio was 1.7. Therefore the differences in catalytic behaviour between our samples and theirs are quite reasonable.It can be seen that, at the same vanadium loading, although La-freeVOx/TiO2 (VT) catalyst is slightly less selective than the respective VOxLa/TiO2 (LaVT) sample in the studied temperature range (400–550°C), it is slightly more active (in terms of butane conversion) than the LaVT. It can be readily seen in Figure 7 that the intrinsic activity evidenced by surface area specific rates (R) and the corresponding turnover of the catalysts have a tendency to increase with the temperature. Moreover it can be seen that LaVT presented a lower activity compared to that of VT catalyst. This trend points to a decreasing number of ODH sites with LaVT. Since present characterizations of the materials indicated higher crystallinities in LaVT than in VT, the trend of turnover values and specific activities in Figure 7 was consistent with an inverse relationship between crystallinity and turnover and specific activity.Variation of turnover (in mol C4 h−1 (molV)−1) and the specific rate (in mol C4 h−1 m−2) with undoped and La-doped VOx/TiO2.
(a)
(b)


### 3.2.2. Product’s Distribution

Variation of the selectivity to the main reaction products as a function of temperature on both samples was presented in Table2. Results in Table 2 showed that over both catalyst samples CO2 and CO were formed at low butane conversion. This is in agreement with the reports of Murgia et al. [15]. Products COx were slightly decreased as conversion increased. Figures 8 and 9 plot the product distrubitions against reaction temperatures. For VT sample the main reaction product was 1-butene in the whole range of studied temperatures while no measurable selectivity toward butadiene was found. Dias et al. [7] studied ODH of n-butane over Mg-V catalysts and showed that 1-butene was a main product; however for higher reaction temperatures (above 748 K) butadiene was a major product. The selectivity towards 2-butenes was always lower than selectivity towards 1-butene. Similar results were observed by Murgia et al. [15] and Jackson and Rugmini [9]. The ratio tran/cis was approximately constant and equal to 1.42. An analogous ratio for the ODH of n-butane over 5 wt.% V2O5/TiO2 was reported by Santacesaria et al. [20]. Figures 6 and 8 showed that the selectivity towards butenes decreased as conversion increased due to the consecutive reactions. Similar trends are observable for other catalysts reported in the literature [16, 20]; that is, conversion increases with the residence time, while selectivity to alkene products decreases.The distribution of alkene’s products with the reaction temperatures.
(a)
(b)Figure 9
Product selectivity over VT and LaVT catalysts at 550°C.The catalytic behaviour of LaVT sample was similar to VT sample. Taking into account the surface acidity of the samples, the LaVT exposed a higher selectivity than VT. The reaction products distribution was approximately the same: 1-butene was the main product, and the ratio trans/cis was constant and equal to 1.6. Especially, LaVT produced butadiene. Butadiene was formed by consecutive reactions, and competition due to carbon oxide formation from both butyl radicals and butenes [31].Figure9 shows the selectivities of alkenes over LaVT and VT catalysts samples at 550°C. It can be seen that the LaVT has a slightly higher selectivity of alkenes than VT.The catalytic behaviour of LaVT sample could be attributed to the following.(i)
Doping La resulted in an increase in basicity of catalyst sample (TPD-NH3 results), and it was expected that this change will affect the catalyst selectivity but not the activity. The best selectivity induced by the presence of La2O3 is a well-known phenomenon described in the literature [27]. Hoang et al. [27] studying the ODH of isobutane over chromium oxide base catalysts indicated that, when La2O3 is present in the support, the activity is low, but the selectivity was almost 100%.(ii)
The presence of La species lowers the surface area and thus also the surface vanadium dispersion due to blocking active sites (BET measurement and UV-Vis spectra) and increased reduction temperatures (TPR-H2 results). These may have a negative effect on the catalytic performance of VT catalyst.


## 3.2.1. Catalytic Activity

Table2 shows conversion of n-butane and the distribution of reaction products, obtained at each temperature over VT and LaVT catalysts. For comparison, the conversion of n-butane over pristine TiO2 and bulk V2O5 is also presented, but the obtained conversions can be negligible. Figure 6 shows the variation in n-butane conversion and total alkene’s selectivity with the reaction temperature.Table 2
Results of catalytic tests in ODH of n-butane (C4H10/O2/N2 = 30/10/60 vol. %, total flow rate 32 mL/min).
T (°C)
Catalyst
Conv. (%)
1-b
2-trans
2-cis
C4-1,3
C
O
x
400
LaVT
9.97
24.99
15.42
10.73
0
26.43
VT
10.48
27.11
13.13
7.96
0
25.02
Parent TiO2
Not observed
Bulk V2O5
Not observed
450
LaVT
14.95
19.83
14.29
10.28
0
21.15
VT
16.64
18.67
9.30
5.80
0
19.70
Parent TiO2
Not observed
Bulk V2O5
Not observed
500
LaVT
16.72
19.66
12.01
8.42
1.96
19.17
VT
18.71
17.59
9.42
6.22
1.38
19.34
Parent TiO2
Not observed
Bulk V2O5
0.94
550
LaVT
19.63
19.87
9.99
6.68
2.52
15.77
VT
21.19
17.96
8.57
5.25
0
15.72
Parent TiO2
3.73
Bulk V2O5
5.76Conversion (a) and total alkene’s selectivity (b) as functions of reaction temperature for VT and LaVT.
(a)
(b)From data reported in Table2 the major products formed under reaction conditions with 10% O2 as coreactant were 1-butene (1-b), tran-2-butene (2-trans), cis-2-butene (2-cis), butadiene, (C4-1,3) CO2, CO, and cracking products (methane, ethane, ethane, and propene). It is possible to observe an effect of the support on the activities and selectivities of vanadium based catalysts in the ODH of n-butane in agreement with the observations of many different authors reported in the literature [30]. Generally, the conversions increase with the temperature, whereas the selectivities decrease, as usual, with the conversion. Also, it was demonstrated that [20] the activity of the dispersed catalysts can be roughly related to the vanadium load. Santacesaria et al. [20] reported a conversion of 3.2% and corresponding selectivity of 51.1% obtained for the ODH of n-butane over a 5% V/TiO2 catalyst at 500°C. However, their experimental conditions differed from those in this work: the content of V was 5% (wt.), and catalyst weight was 0.05 g (meanwhile they are 15% and 0.2 g, resp., in this work); in their work, the total feed low rate was 150 mL/min, and O2/C4H10 ratio was 1.7. Therefore the differences in catalytic behaviour between our samples and theirs are quite reasonable.It can be seen that, at the same vanadium loading, although La-freeVOx/TiO2 (VT) catalyst is slightly less selective than the respective VOxLa/TiO2 (LaVT) sample in the studied temperature range (400–550°C), it is slightly more active (in terms of butane conversion) than the LaVT. It can be readily seen in Figure 7 that the intrinsic activity evidenced by surface area specific rates (R) and the corresponding turnover of the catalysts have a tendency to increase with the temperature. Moreover it can be seen that LaVT presented a lower activity compared to that of VT catalyst. This trend points to a decreasing number of ODH sites with LaVT. Since present characterizations of the materials indicated higher crystallinities in LaVT than in VT, the trend of turnover values and specific activities in Figure 7 was consistent with an inverse relationship between crystallinity and turnover and specific activity.Variation of turnover (in mol C4 h−1 (molV)−1) and the specific rate (in mol C4 h−1 m−2) with undoped and La-doped VOx/TiO2.
(a)
(b)


## 3.2.2. Product’s Distribution

Variation of the selectivity to the main reaction products as a function of temperature on both samples was presented in Table2. Results in Table 2 showed that over both catalyst samples CO2 and CO were formed at low butane conversion. This is in agreement with the reports of Murgia et al. [15]. Products COx were slightly decreased as conversion increased. Figures 8 and 9 plot the product distrubitions against reaction temperatures. For VT sample the main reaction product was 1-butene in the whole range of studied temperatures while no measurable selectivity toward butadiene was found. Dias et al. [7] studied ODH of n-butane over Mg-V catalysts and showed that 1-butene was a main product; however for higher reaction temperatures (above 748 K) butadiene was a major product. The selectivity towards 2-butenes was always lower than selectivity towards 1-butene. Similar results were observed by Murgia et al. [15] and Jackson and Rugmini [9]. The ratio tran/cis was approximately constant and equal to 1.42. An analogous ratio for the ODH of n-butane over 5 wt.% V2O5/TiO2 was reported by Santacesaria et al. [20]. Figures 6 and 8 showed that the selectivity towards butenes decreased as conversion increased due to the consecutive reactions. Similar trends are observable for other catalysts reported in the literature [16, 20]; that is, conversion increases with the residence time, while selectivity to alkene products decreases.The distribution of alkene’s products with the reaction temperatures.
(a)
(b)Figure 9
Product selectivity over VT and LaVT catalysts at 550°C.The catalytic behaviour of LaVT sample was similar to VT sample. Taking into account the surface acidity of the samples, the LaVT exposed a higher selectivity than VT. The reaction products distribution was approximately the same: 1-butene was the main product, and the ratio trans/cis was constant and equal to 1.6. Especially, LaVT produced butadiene. Butadiene was formed by consecutive reactions, and competition due to carbon oxide formation from both butyl radicals and butenes [31].Figure9 shows the selectivities of alkenes over LaVT and VT catalysts samples at 550°C. It can be seen that the LaVT has a slightly higher selectivity of alkenes than VT.The catalytic behaviour of LaVT sample could be attributed to the following.(i)
Doping La resulted in an increase in basicity of catalyst sample (TPD-NH3 results), and it was expected that this change will affect the catalyst selectivity but not the activity. The best selectivity induced by the presence of La2O3 is a well-known phenomenon described in the literature [27]. Hoang et al. [27] studying the ODH of isobutane over chromium oxide base catalysts indicated that, when La2O3 is present in the support, the activity is low, but the selectivity was almost 100%.(ii)
The presence of La species lowers the surface area and thus also the surface vanadium dispersion due to blocking active sites (BET measurement and UV-Vis spectra) and increased reduction temperatures (TPR-H2 results). These may have a negative effect on the catalytic performance of VT catalyst.


## 4. Conclusions

V catalysts supported on titania at exceeding theoretical monolayer coverage and doping with lanthanum were tested in the oxidative dehydrogenation of n-butane. In the tested conditions 1-butene was the main reaction products. Characterization of the materials showed thatVOx surface species are well dispersed on the support surface. Acidity measurements revealed that the catalyst samples possess acid sites of weak and moderate strengths. La-containing VOx/TiO2 exhibited lower acidity than La-free VOx/TiO2 one, and doping with lanthanum did not improve the catalytic performance of VT catalyst. The low activity could be explained with the lower dispersion of VOx species in this sample since it favours the agglomeration of V sites. Despite the observation that lanthanum-doping improved slightly the butene selectivies due to lowered surface acidity, this could not improve the yields of butene. Therefore, it seems likely that improvement of the butene yields in the ODH of n-butane could be achieved using catalysts with highly dispersed, preferably tetrahedrally coordinated VOx species, supported on nonacidic materials with high surface area.



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*Source: 868906-2013-09-09.xml*