FLUIDIZABLE ALKANE DEHYDROGENATION CATALYST

Abstract

Fluidizable catalysts for oxygen-free oxidative dehydrogenation of alkanes to corresponding olefins. The catalysts contain 10-20% (by weight per total catalyst weight) of one or more vanadium oxides as the catalytic material, which are mounted upon an alumina support that is modified with zirconia at alumina/zirconia ratios of 5:1 up to 1:2. Various methods of preparing and characterizing the fluidizable catalysts are also provided.

Claims

1. A fluidizable alkane dehydrogenation catalyst comprising: a zirconia-modified alumina -Al.sub.2O.sub.3 support material; and 10-20% of one or more vanadium oxides by weight based on a total weight of the alkane dehydrogenation fluidizable catalyst, the one or more vanadium oxides being adsorbed onto the support material; wherein the support material comprises an -Al.sub.2O.sub.3/zirconia weight ratio of 1-5:1-3; and wherein the alkane dehydrogenation fluidizable catalyst has an average particle size of 40-120 m.

2. The fluidizable alkane dehydrogenation catalyst of claim 1, wherein the one or more vanadium oxides are selected from the group consisting of V.sub.2O.sub.5, VO.sub.2 and V.sub.2O.sub.3.

3. The fluidizable alkane dehydrogenation catalyst of claim 2, comprising at least 50% of V.sub.2O.sub.5 based on total weight of the one or more vanadium oxides.

4. The fluidizable alkane dehydrogenation catalyst of claim 1, wherein the -Al.sub.2O.sub.3/zirconia weight ratio is 1-2:1.

5. The fluidizable alkane dehydrogenation catalyst of claim 1, wherein the one or more vanadium oxides form a crystalline phase on the surface of the zirconia-modified -Al.sub.2O.sub.3 support material.

6. (canceled)

7. A fluidizable alkane dehydrogenation catalyst of claim 1, comprising: a zirconia-modified -Al.sub.2O.sub.3 support material; and 10-20% of one or more vanadium oxides by weight based on a total weight of the alkane dehydrogenation fluidizable catalyst, the one or more vanadium oxides being adsorbed onto the support material: wherein the support material comprises an -Al.sub.2O.sub.3/zirconia weight ratio of 1-5:1-3; and wherein the alkane dehydrogenation fluidizable catalyst is in the form of a plurality of particles and more than 75% of the particles have a particle size of 40-120 m.

8. The fluidizable alkane dehydrogenation catalyst of claim 1, having an apparent particle density of 1.5-3.5 g/cm.sup.3.

9. The fluidizable alkane dehydrogenation catalyst of claim 1, having Class B powder properties in accordance with Geldart particle classification.

10. A fluidizable alkane dehydrogenation catalyst, comprising: a zirconia-modified -Al.sub.2O.sub.3 support material; and 10-20% of one or more vanadium oxides by weight based on a total weight of the alkane dehydrogenation fluidizable catalyst, the one or more vanadium oxides being adsorbed onto the support material; wherein the support material comprises an -Al.sub.2O.sub.3/zirconia weight ratio of 1-5:1-3; and wherein the alkane dehydrogenation fluidizable catalyst has a BET surface area of 10-50 m.sup.2/g.

11. The fluidizable alkane dehydrogenation catalyst of claim 1, wherein the zirconia present in the -Al.sub.2O.sub.3/zirconia ratio depresses the surface acidity of the alkane dehydrogenation fluidizable catalyst.

12. The fluidizable alkane dehydrogenation catalyst of claim 1, wherein the zirconia present in the -Al.sub.2O.sub.3/zirconia ratio enhances the interaction between the one or more vanadium oxides and the support material.

13. The fluidizable alkane dehydrogenation catalyst of claim 1, wherein the zirconia present in the -Al.sub.2O.sub.3/zirconia ratio enhances the reducibility of the one or more vanadium oxides.

14-18. (canceled)

Description

BRIEF DESCRIPTION OF THE DRAWINGS

[0035] A more complete appreciation of the disclosure and many of the attendant advantages thereof will be readily obtained as the same becomes better understood by reference to the following derailed description when considered in connection with the accompanying drawings, wherein:

[0036] FIG. 1 is the Geldart diagram for classification of particle fluidization.

[0037] FIG. 2 is a curve showing N2 adsorption/desorption isotherms of 15% VO.sub.x/Al2O.sub.3-ZrO.sub.2 (2:1) catalyst sample.

[0038] FIG. 3 shows the XRD patterns of various Al.sub.2O.sub.3-ZrO.sub.2 catalysts, with the arrows indicating the peaks for V.sub.2O.sub.5.

[0039] FIG. 4A shows the TPR profiles for various Al.sub.2O.sub.3-ZrO.sub.2 catalysts.

[0040] FIG. 4B shows the H.sub.2 consumption of various Al.sub.2O.sub.3-ZrO.sub.2 catalysts with various-ZrO.sub.2 loadings.

[0041] FIG. 5 shows H.sub.2 consumption of TPR/TPO cycles of 15% VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2 (2:1) catalyst.

[0042] FIG. 6A is an SEM image of a fresh sample of the 15% VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2 (2:1) catalyst (50 kx magnification).

[0043] FIG. 6B is an SEM image of a TPR-reduced sample of the 15% VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2(2:1) catalyst (50 kx magnification).

[0044] FIG. 7 shows the NH.sub.3-TPD profiles of Al.sub.2O.sub.3-ZrO.sub.2 support with various ZrO.sub.2 loadings and 15% VO.sub.x.

[0045] FIG 8A is a schematic diagram of the CREC Riser Simulator experimental set-up.

[0046] FIG. 8B is a schematic diagram providing an overview of the CREC Riser Simulator reactor body.

[0047] FIG. 9 shows the effect ZrO.sub.2 on ethane conversion and product selectivity defined per gram VO.sub.x with reaction conditions: Reaction time=40 s, T=600 C., W=0.4, Ethane Feed=1 ml STP).

[0048] FIG. 10 shows ethane conversion and ethylene selectivity over redox cycles for the VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2 (2:1) catalyst, defined per gram VO.sub.x with reaction conditions: Reaction time=40 s, T=600 C., W=0.4, Ethane Feed=1 ml STP).

[0049] FIG. 11 shows the effect of temperature on ethane conversion, defined per gram VO.sub.x with reaction conditions: Reaction time=40 s, Ethane Feed=1 ml STP).

[0050] FIG. 12 shows the effect of temperature on product selectivity, defined per gram VO.sub.x with reaction conditions: Reaction time=40 s, Ethane Feed=1 ml STP).

[0051] FIG. 13A shows the effect of reaction time on ethane conversion and product selectivity, defined per gram VO.sub.x loaded on Al.sub.2O.sub.3-ZrO.sub.2 (2:1) with reaction conditions: T=550 C., Ethane Feed=1 ml STP).

[0052] FIG. 13B shows the effect of reaction time on ethane conversion and product selectivity defined per gram VO.sub.x loaded on Al.sub.2O.sub.3, with reaction conditions: T=550 C., Ethane Feed=1 ml STP).

DETAILED DESCRIPTION OF THE EMBODIMENTS

[0053] Referring now to the drawings, wherein like reference numerals designate identical or corresponding parts throughout the several views.

[0054] In the present disclosure, there are provided catalysts for oxidative dehydrogenation (ODH) of alkanes in reactors having a fluidized bed design. These catalysts contain one or more oxides of vanadium (VO.sub.x) as catalytic material, which are adsorbed and mounted upon zirconia or ZrO.sub.2-modified alumina support material.

[0055] In a fluidized bed reactor, before the reactor is started, the catalyst pellets lie on a grate at the bottom of the reactor. Reactants are continuously pumped into the reactor through a distributor causing the bed to become fluidized. During the fluidization, the catalyst pellets are converted from a static solid-like state to a dynamic fluid-like state. The bed's behavior after initial fluidization depends on the state of the reactant. If it is a liquid the bed expands uniformly with increased upward flow of the reactant, resulting in a homogenous fluidization. If the reactant is a gas, the bed will be non-uniform because the gas forms bubbles in the bed, resulting in aggregative fluidization. In the present disclosure, the reactant or feed is a light alkane such as but not limited to ethane, propane and butane (including n-butane and isobutane), all of which are gases and hence, an aggregative fluidization may be more probable.

[0056] Properties or parameters for determining the fluidizability of a catalyst include but are not limited to average particle size, and particle size distribution. The average particle size and the particle size distribution can be measured, for example, using a Mastersizer 2000 from Malvern Instruments. The apparent particle, density can be assessed using a CREC-established method. In the method, a known amount of catalyst is introduced to a flask. The flask is filled with isopropanol and the apparent particle density, AD, is calculated using the following equation:

[00001]$\begin{array}{cc}\mathrm{AD}=\frac{W_{\mathrm{eat}}}{V_T-V_{\mathrm{isopropanol}}}& \left(\mathrm{Eq}..Math.1\right)\end{array}$

where AD is the apparent panicle density (g/cm.sup.3) W.sub.cat is the catalyst weight, V.sub.x is the flask volume and V.sub.isopropanol is the volume of isopropanol calculated as the ratio of the weight of isopropanol needed to fill the flask and the density of isopropanol.

[0057] A catalyst in accordance with the present disclosure has an average particle size (diameter) of 40-120 m, preferably 50-100 m, more preferably 60-80 m. The particle size distribution is 20-180 m where more than 75% of the particles are 40-120 m, preferably more than 80%, more preferably more than 85%, even more preferably more than 90%. The apparent particle density of the catalyst is 1.0-4.0 g/cm.sup.3, preferably 1.5-3.5 g/cm.sup.3, more preferably 1.8-3.2 g/cm.sup.3.

[0058] In some embodiments, with the calculated average particle size and particle apparent density values, the fluidization regime of the vanadia-zirconia-alumina catalyst particles of the present disclosure can be determined using Geldart's powder classification chart of FIG. 1 [Geldart, D. (1973). Types of Gas Fluidization. Powder Technology, 7, 285-292incorporated herein by reference in its entirety]. In at least one embodiment, the catalyst particles display a Geldart Class B powder property, which is highly fluidizable under ODH conditions. Large particles, such as those under Geldart Class D, may limit the gas phase reactant access to the inner layers of the catalyst. As a result, using smaller particles can minimize the diffusional resistance and reduction/oxidation rates can be maximized. On the other hand, very small particles, such as those under Geldart's Class C, can cause fluidization problems, channeling and loss of fines. In addition, these very fine particles fluidize under very difficult to attain conditions, and may require the application of an external force, such as mechanical agitation.

[0059] In certain embodiments, the fluidizability of the catalysts is demonstrated in a Plexiglas unit with dimensions matching the one of a CREC riser simulator.

[0060] Accordingly, the fluidizable catalysts of the present disclosure contain 10-20% of one or more vanadium oxides as catalytic material by weight based on the total catalyst weight, preferably 12-18%, more preferably 12.5-17.5%. The vanadium oxides are of formula V.sub.xO.sub.y wherein x=1-2 and y=2-5, preferably selected from the group consisting of V.sub.2O.sub.5, VO.sub.2 and V.sub.2O.sub.3. In certain embodiments, the catalysts are substantially free of V.sub.2O.sub.3 and contain a mixture of at least 50% V.sub.2O.sub.5 based on total weight of vanadium oxides, with the rest being VO.sub.2, preferably 75-80% V.sub.2O.sub.5, more preferably 85-90% V.sub.2O.sub.5, even more preferably at least 90-95% V.sub.2O.sub.5, most preferably 95-99.9% V.sub.2O.sub.5. In some embodiments, the catalysts consist essentially of V.sub.2O.sub.5 and are substantially free of V.sub.2O.sub.3 and VO.sub.2.

[0061] The vanadinm oxide catalytic material is loaded on a zirconia-alumina inert support. The zirconia-alumina support comprises zirconia (ZrO.sub.2) and alumina (Al.sub.2O.sub.3) at different alumina/zirconia weight ratios: 5:3, 5:2, 5:1, 4:3, 4:1, 3:2, 3:1, 2:1, 1:1 or 1:2, preferably 4:1, 3:2, 3:1, 2:1 or 1:1, more preferably 2:1 or 1:1 or any range, fractional or whole, between the aforementioned ranges. In one embodiment, the alumina/zirconia weight ratio in the support material is 2:1. The alumina-based support material may be comprised of a plurality of different crystallographic phases. Examples of alumina-based inert material include but are not limited to aluminum oxide, alumina, alumina monohydrate, alumina trihydrate, alumina-silica, bauxite, calcined aluminum hydroxides such as gibbsite, bayerite and boelimite, -alumina, transition aluminas such as -alumina, -alumina and -alumina, and calcined hydrotalcite. In at least one embodiment, the support material is -alumina-based (-Al.sub.2O.sub.3).

[0062] To modify the alumina support with zirconia (ZrO.sub.2), an alumina support can be initially calcined to remove moisture and other volatile compounds then immersed in a solution containing a zirconium precursor salt (e.g. zirconium tetrachloride) and an organic solvent such as toluene, for 12-24 h and preferably with stirring to achieve a homogeneous mixture. The soaked alumina support can then be dried by calcination again. In general, the zirconia modification is found to have the effect of reducing the BET (Brunauer-Emmett-Teller) surface area of the alumina. The zirconia-modified alumina support has a BET surface area of 10-50 m.sup.2/g, preferably 15-40 m.sup.2/g, more preferably 20-30 m.sup.2/g.

[0063] To deposit and adsorb the catalytic material onto the zirconia-modified alumina support, a similar soaking impregnation method as described above may be used, with a vanadium(IV) or a vanadium(V) precursor salt such as vanadyl acetylacetonate, vanadyl sulfate, vanadium pentoxide, vanadium oxytripropoxide, tetrakis(diethylamido)vanadium. The vanadium precursor is preferably phosphorus-free. It is during the post-soaking calcination that the vanadium salt is converted into one or more vanadium oxides.

[0064] In addition to the effect on surface area, the zirconia modification also depresses the surface acidity and metal-support interaction of the catalyst, thereby enhancing olefin selectivity in ODH reactions and reducing coke (CO.sub.x) formation. Catalyst acidity plays a major role in metal support interaction affecting VO.sub.x reducibility. Reducibility may control catalyst activity and selectivity by providing O.sub.2 for oxidation, with high acidity not favoring able selective oxidation.

[0065] The effects of the zirconia modification can be established by at least NH.sub.3 desorption kinetics analysis, and the vanadia-zirconia-alumina catalysts provided herein have an estimated energy of NH.sub.3 desorption of 70-90 kJ/g, preferably 72-85 kJ/g, more preferably 75-82 kJ/g. Furthermore, as evaluated by X-ray diffraction, the vanadia catalytic material (comprising one or more vanadium oxides as described herein) forms a crystalline phase on the zirconia-alumina support surface. In the absence of the zirconia modification of the alumina support, the catalyst would display an amorphous phase.

[0066] The present disclosure also relates to a process of converting an alkane to a corresponding olefin by oxidative dehydrogenation in the presence of a fluidizable catalyst described herein.

[0067] Alkane oxidative, dehydrogenation (ODH) reactions incorporating a vanadia-zirconia-alumina fluidizable catalyst provided herein are preferably operated in an oxygen-free environment or atmosphere at temperatures ranging 525-675 C. preferably 550-625 C., more preferably 575-600 C., at standard pressure (100 kPa/1 bar/14.5 psi 0.9869 atm) and a minimum catalyst-alkane feed contact time of 15 s to 1 min, preferably 20-50 s, more preferably 30-45 s. The amount of catalyst present in an ODH reaction is 0.05-0.5 g/ml per ml of alkane feed injected, preferably 0.1-0.4 g/ml, more preferably 0.15-0.3 g/ml. Under these operating conditions, an alkane is converted to a corresponding olefin in accordance with the equation below:

C.sub.yH.sub.2y+2+V.sub.2O.sub.5.fwdarw.C.sub.yH.sub.2y+H.sub.2O+V.sub.2O.sub.3 (2)

where y is 2, 3 or 4.
In some embodiments, the alkane-olefin conversion may be accompanied by the following complete oxidation of the alkane or the olefin as side, secondary reactions:

C.sub.yH.sub.2y+2+V.sub.2O.sub.5.fwdarw.aCO.sub.2+bCO+(2y2)/2H.sub.2O+V.sub.2O.sub.3 (3)

C.sub.yH.sub.2y+V.sub.2O.sub.5.fwdarw.aCO.sub.2+bCO+2y/2H.sub.2O+V.sub.2O.sub.3 (4)

where y is 2, 3 or 4 and y=a+b.

[0068] With the use of the vanadia-zirconia-alumina fluidizable catalyst, an ODH reaction has an alkane conversion rate, as defined with the equation below, of up to 50%, preferably 15-45%, more preferably 17-40%. In at least one embodiment, the alkane converted is ethane and the corresponding olefin is ethylene.

[00002]$\begin{array}{cc}\mathrm{Conversion}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}=\frac{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}.Math..Math.\mathrm{converted}}{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}.Math..Math.\mathrm{fed}}100.Math.\%& \left(\mathrm{Eq}..Math.5\right)\end{array}$

The selectivity to the corresponding olefin or CO.sub.x is calculated as:

[00003]$\begin{array}{cc}\mathrm{Selectivity}.Math..Math.\mathrm{to}.Math..Math.\mathrm{product}=\frac{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{product}}{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}.Math..Math.\mathrm{reacted}-\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{product}}100.Math.\%& \left(\mathrm{Eq}..Math.6\right)\end{array}$

The olefin selectivity is at least 75%, preferably 80-90%, more preferably 85-90%.

EXAMPLES

[0069] In the following examples, the effects of ZrO.sub.2 modification on the fluidizable VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 catalysts for oxidative dehydrogenation (ODH) of ethane to ethylene were investigated. These examples are provided to further illustrate the numerous embodiments of the present disclosure, and are not intended to limit the scope of the appended claims. The synthesized catalysts were characterized using different physiochemical techniques. The gas phase, oxygen-free ODH (of ethane) experiments were established in a CREC-Riser Simulator under various reaction conditions. The main findings of these examples are provided in the following paragraphs:

[0070] From the XRD analysis, it is shown that both V.sub.2O.sub.5 and ZrO.sub.2 species are present on the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 catalysts. XRD patterns also demonstrate that VO.sub.x is present in the prepared catalyst in a crystalline phase, with the formation of this crystalline phase being promoted by the ZrO.sub.2. Samples of VO.sub.x/-Al.sub.2O.sub.3 catalyst display an amorphous phase only.

[0071] From the temperature-programmed reduction (TPR) experiments. It is demonstrated that good V.sub.2O.sub.5 reduction activity occurs at low ZrO.sub.2 content (2:1 ratios). TPR/TPO oxidation-reduction cycles show good catalyst stability, increasing ZrO.sub.2 content decreases the percent of metal reduction.

[0072] NH.sub.3-TPD measurements confirm the existence of weak acid sites on the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2. The desorption kinetics suggests a medium range of interaction energies involved between VO.sub.x, and the support, with this likely enhancing metal reducibility.

[0073] ODH of ethane in the presence of VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 and under free oxygen atmosphere shows that ethylene, CO and CO.sub.2 are the major products.

[0074] Among the three samples prepared, the catalyst with -Al.sub.2O.sub.3:ZrO.sub.2=2:1 ratio gives the highest ethane conversion (37.9%). This result is in agreement with TPR analysis which shows best reducibility (highest consumption) for this catalyst.

[0075] The VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 fluidizable catalyst (-Al.sub.2O.sub.3:ZrO.sub.2=2:1) displays ethylene selectivity up to 90% (at 600 C.) while the unmodified VO.sub.x/-Al.sub.2O.sub.3 catalyst gives 42% ethylene selectivity under same reaction conditions.

[0076] ZrO.sub.2 addition alters the acidity and structure of the alumina support which influences the formation of VO.sub.x (mono or poly). The ZrO.sub.2 also affects the metal support interaction and plays a critical role in lowering VO.sub.x reducibility, therefore allowing an increased ethylene selectivity due to a promoted oxygen controlled release rate.

Example 1

Catalyst Preparation

[0077] Impregnation by a soaking (excess of solvent) technique was used to prepare catalyst samples [M. A. Baares, M. V Mart, X. Gao, J. L. G. Fierro, and I. E. Wachs, Dynamic behavior of supported vanadia catalysts in the selective oxidation of ethane in situ Raman, UV-Vis DRS and reactivity studies, vol. 61, pp. 295-301, 2000incorporated herein by reference in its entirety]. Before metal loading, the alumina support was calcined under pure N.sub.2 flow at 500 C. for 4 h, to remove moisture and volatile compounds. The calcined sample was placed in a beaker and toluene was added. Zirconium tetrachloride was then added to the beaker, and the mixture was left under stirring for 12 h. The sample was filtered from the solvent and dried at ambient conditions. After complete drying, the sample was calcined again at 500 C. for 5 h to remove the solvent. Three support samples were prepared with -Al.sub.2O.sub.3/ZrO.sub.2 weight ratios of 2:1, 1:1 and 1:2.

[0078] Accordingly, three catalyst samples were prepared by dispersing 15 wt % of V on each of the above -Al.sub.2O.sub.3-ZrO.sub.2 supports. Vanadyl acetylacetonate (Aldrich, 97%) was used as precursor for vanadium loading. The V loading was also accomplished using the same approach as ZrO.sub.2 loading. The ZrO.sub.2 modified Al.sub.2O.sub.3 support and vanadyl acetylacetonate, were added to a beaker containing toluene. The mixture was stirred for 24 h, to obtain a homogeneous mixture which facilitated better metal dispersion. The solid sample was separated by vacuum nitration and dried at ambient temperature. The dried sample was then reduced with hydrogen (10% H.sub.2 and 90 Ar) at 500 C. in a fluidized bed reactor. Finally, the reduced sample was calcined under air at 500 C. for 4 h to obtain the oxide for of the catalyst. After this treatment, catalyst color became yellow indicating the presence of V.sub.2O.sub.5 on the support surface.

Example 2

Elemental and BET Surface Area Analyses of Catalysts

[0079] XRF analysis was used to determine elements and compound ratios in each sample after synthesis. A Bruker Tornado M4 Micro-XRF Analyzer, equipped with a single High Performance XFlash Detector and a 25 m diameter spot size, was employed for XRF analysis.

[0080] The nitrogen adsorption and BET surface area of the VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2 catalyst samples were determined in a Quantachrome ASIQwin. The nitrogen adsorption was carried out at 77 K. For each experiment, 0.40-0.50 g of catalyst sample was degassed at 350 C. for 2 h. The adsorption isotherms were measured in the 0.04 to 1 kcal/mol relative pressure range.

[0081] The XRF results as shown in Table 1, indicate that compound percentages are equal to what was targeted, with a slight deviation. The nitrogen isotherm analysis was conducted to understand the adsorption/desorption characteristics of the catalyst sample. FIG. 2 shows the adsorption/desorption isotherms of a ZrO.sub.2 modified VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 sample synthesized for this study. The sample shows a Type-V isotherm indicating narrow size mesoporosity [X. Lin, R. R. Poeppelmeier, and E. Weitz, Oxidative dehydrogenation of ethane with oxygen catalyzed by K-Y zeolite supported first-row transition metals, Appl. Catal. A Gen., vol. 381, no. 1-2, pp. 114-120, June 2010incorporated herein by reference in its entirety]. The isotherm data was further processed to determine the BET surface of the sample. The calculated BET surface area and the monolayer volume are also presented in Table 1. The BET surface area of the ZrO.sub.2 modified sample is lower than the surface of the bare -Al.sub.2O.sub.3 support (141 m.sup.2/g). The dispersed ZrO.sub.2 and the vanadium species occupied the support pores, which contributed to the decrease of the surface area.

[0082] The monolayer volume of the adsorbed nitrogen can be calculated by Eq. 7:

[00004]$\begin{array}{cc}{n}_m=\frac{s_{\mathrm{BET}}}{A_{m}N}& \left(\mathrm{Eq}..Math.7\right)\end{array}$

where, (1) S.sub.BET is the BET surface area m.sup.2, (2) N represents Avogadro's constant and molecule/mol, (3) A.sub.m stands for the volume occupied by one N.sub.2 gas molecule (0.162 m.sup.2), and (4) n.sub.m denotes the monolayer volume per gram catalyst. The monolayer coverage occurs after 0.75 relative pressure indicates good dispersion of active sites, and their availability for adsorption. This was expected as the catalyst was synthesized by soaking impregnation which provided good metal dispersion and thus, a satisfactory monolayer volume.

TABLE-US-00001 TABLE 1 XRF.sup.a and BET surface area characterization results. BET Surface Monolayer area volume Sample VO.sub.x % Al.sub.2O.sub.3 % ZrO.sub.2 % (m.sup.2/g .Math. cat) (cm.sup.3/g) 15% VO.sub.x/Al.sub.2O.sub.3ZrO.sub.2(2:1) 14.4 57.2 28.4 24.1 2.4 10.sup.4 .sup.aCatalyst elements percentages are within 2% accuracy.

Example 3

X-ray Diffraction Analysis of Catalysts

[0083] X-ray diffraction (XRD) analysis was conducted to identify the crystallographic structure of catalyst samples, XRD patterns of all catalysts reported in this study, were recorded on a Rigaku MiniFlex Diffractometer with monochromatic Cu K radiation (=0.15406 nm, 30 kV, 15 mA) using the normal scan rate of 4/min. X-rays were collected using a 1.25 divergent scattering slit, and a 0.13 mm receiving slit. Samples were scanned within the 2 range of 20-80 with a step size of 0.005.

[0084] FIG. 3 shows the XRD patterns of the various -Al.sub.2O.sub.3/ZrO.sub.2 containing support samples and the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 catalyst after VO.sub.x loading. The V.sub.2O.sub.5 was detected in the range of 2 from 10 to 40 [F. Klose, T. Wolff, H. Lorenz, a Seidelmorgenstern. Y. Suchorski, M. Pierkowska, and H. Weiss, Active species on -alumina-supported vanadia catalysts: Nature and reducibility, J. Catal., vol. 247, no. 2, pp. 170-193, April 2007incorporated herein by reference in its entirety]. Peaks of t-ZrO.sub.2 can also be found at 2 of 30, 48 and 65 while -Al.sub.2O.sub.3 peaks appeared at 2 of 45 and 60.

[0085] It can be seen in FIG. 3 that the V.sub.2O.sub.5 peak intensity was sharply decreased with decreasing the -Al.sub.2O.sub.3 to ZrO.sub.2 ratios (increasing in ZrO.sub.2 contents). Only VO.sub.2 was obtained on the support surface in -Al.sub.2O.sub.3-ZrO.sub.2 (1:2), which resulted in lower oxygen-carrying capacity and therefore lowers catalyst activity.

[0086] Furthermore, ZrO.sub.2 introduced a crystal phase to the catalyst, in comparison with the catalyst sample without ZrO.sub.2 [S. Al-Ghamdi, M. Volpe, M. M. Hossain, and H. de Lasa, VO.sub.x/c-Al.sub.2O.sub.3 catalyst for oxidative dehydrogenation of ethane to ethylene: Desorption kinetics and catalytic activity, Appl. Catal. A Gen., vol. 450, pp. 120-130, January 2013incorporated herein by reference in its entirety]. This crystal phase is not detected by XRD and may reduce the oxygen-carrying capacity and the catalyst activity by increasing active site agglomeration.

Example 4

Temperature Programmed Reduction-Oxidation (TPR/TPO) Experiments

[0087] The TPR/TPO experiments were conducted using a Micromeritics AutoChemII 2920 Analyzer. The purpose of the TPR/TPO cycles was to determine catalyst reduction temperature, maximum temperature and catalyst stability during reduction-oxidation cycles. It is reported that during reduction/oxidation at high temperatures, vanadium dispersion changes [E. Lpez, E. Heracleous, A. a . Lemonidou, and D. O. Borio, Study of a multitubular fixed-bed reactor for ethylene production via ethane oxidative dehydrogenation, Chem. Eng. J., vol. 145, no. 2, pp. 308-315, December 2008incorporated herein by reference in its entirety] when VO.sub.x phase interact on the support surface [M. Argyle, Effect of Catalyst Structure on Oxidative Dehydrogenation of Ethane and Propane on Alumina-Supported Vanadia, J. Catal., vol. 208, no. 1, pp. 139-149, May 2002.incorporated herein by reference in its entirety]. As a result, the catalyst activity and stability changes significantly [S. Al-Ghamdi, M. Volpe, M. M. Hossain, and H. de Lasa, VO.sub.x/c-Al.sub.2O.sub.3 catalyst for oxidative dehydrogenation of ethane to ethylene: Desorption kinetics and catalytic activity, Appl. Catal. A Gen., vol. 450, pp. 120-130, January 2013incorporated herein by reference in its entirety].

[0088] At the beginning of each experiment, argon (99.9%) was introduced at rate of 50 ml/min while the temperature was increased to 300 C. for a period of 3 h. The system was cooled to ambient temperature and H.sub.2/Ar gas mixture (10% H.sub.2) was circulated at a rate of 50 ml/min. At after the gas flow reached to steady state, the catalyst bed temperature was raised to 750 C. at a heating rate of 10 C./min. The H.sub.2 concentration of the gas leaving the catalyst bed was measured using a thermal conductivity detector (TCD). The detector signal was calibrated to a volume of H.sub.2 consumed cc/g catalyst. A plot of the volume of H.sub.2 consumption versus time/temperature represents the reduction profile of the catalyst sample. The area under the TPS profiles represents the total hydrogen consumption of the catalyst samples.

[0089] TPR/TPO characterization is an important technique for oxygen free ODH catalyst characterization. TPR simulates the ODH reaction as shown in Eq. 2 and Eq. 3:

Reduction of the ODH catalyst during TPR with hydrogen:

V.sub.2O.sub.5+2 H.sub.2.fwdarw.V.sub.2O.sub.3+2 H.sub.2O (8)

Reduction of the ODH catalyst with ethane:

2CH.sub.3CH.sub.3+V.sub.2O.sub.5.fwdarw.V.sub.2O.sub.3+2CH.sub.2CH.sub.2+2H.sub.2O (9)

[0090] It can be seen in both Eq. 8 and Eq. 9 cases, by using hydrogen or ethane, ODH reduces the V.sub.2O.sub.5 into V.sub.2O.sub.3. Consequently, the TPR evaluation of the catalyst sample can be correlated to the activity (reactivity) of the catalyst at various temperature ranges. The TPR/TPO test also determines the oxygen-carrying capacity and the redox properties of the catalysts. The oxygen-carrying capacity eventually determines the circulation rate of the catalyst between the twins fluidized bed reactors: ODH reactor and the catalyst regenerator. FIGS. 4A and 4B show the TPR profiles and the H.sub.2 consumption, for different ZrO.sub.2 containing catalysts. In all samples, the V loading is kept at a 15 wt % of the catalyst. Thus, the presence of multiple peaks indicates that the reduction proceeds in several steps [F. Klose, T. Wolff, H. Lorenz, a Seidelmorgenstern, Y. Suchorski, M. Piorkowska, and H. Weiss, Active species on -alumina-supported vanadia catalysts: Nature and reducibility, J. Catal., vol. 247, no. 2, pp. 176-193, April 2007; Y, H. Kim and H. Lee, Redox Property of Vanadium Oxide and Its Behavior in Catalytic Oxidation, vol. 20, no. 12, 1999each incorporated herein by reference in its entirety]. The introduction of the ZrO.sub.2, reduced the support surface acidity, and as a result, this enhances the formation of isolated mono-vanadate species on the support surfaces [I. E. Wachs, Catalysis science of supported vanadium oxide catalysts, Dalton Trans., vol. 42, no. 33, pp. 11762-9, September 2013; J. R. Sohn, S. G. Cho, Y. Il Pae, and. S. Hayashi, Characterization of Vanadium OxideZirconia Catalyst, vol. 177, no. 0076, pp. 170-177, 1996each incorporated herein by reference in its entirety]. During vanadium oxide reduction, oxygen vacancies are formed at the surface. As the reduction proceeds, the concentration of these vacancies gradually decreases. Vacancies may however, aggregate and part of vanadium oxide edges may produce a new structure (non-isolated species). This may also occur, as a result of increases on the vanadium loading [A. M. Elfadly, A. M. Badawi, F. Z. Yehia, Y. A. Mohamed, M. A. Betiha, and A. M. Rabie, Selective nano alumina supported vanadium oxide catalysis for oxidative dehydrogenation of ethylbenzene to styrene using CO.sub.2 as soft oxidant, Egypt. J. Pet., vol. 22, no. 3, pp. 373-380, December 2013incorporated herein by reference in its entirety].

[0091] TPR results may also point to the catalyst oxygen-carrying capacity and the oxygen releasing rate. This is the case, since the oxygen-carrying capacity of the catalyst can be determined according to Eq. 8 (two moles of hydrogen reduce one male of oxygen). FIG. 3B shows the histogram plots of hydrogen consumption at different Al.sub.2O.sub.3 to ZrO.sub.2 ratios with same 15 wt % VO.sub.x. It appears that the hydrogen consumption was comparable between the catalyst samples containing -Al.sub.2O.sub.3/ZrO.sub.2 ratios of 2:1 and those of 1:1. However, catalyst reducibility was significantly decreased with -Al.sub.2O.sub.3/ZrO.sub.2 ratios of 1:2.

[0092] Repeated TPR/TPO experiments were conducted to confirm catalyst reducibility and re-oxidation ability during the multiple cycles. This also may allow considering thermal sintering in the high temperature range of the redox cycles. Regarding the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 (2:1) sample, it was selected in this study due to its high oxygen-carrying capacity as revealed in hydrogen consumption analysis. FIG. 5 shows the TPR profiles for the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 (2:1) sample under repeated TPR/TPO cycles. The TPR profiles remained almost unchanged during consecutive cycles with the only exception being the first cycle. It is hypothesized that it is during the first cycle that the decomposition of the residual metal precursors is completed. Once these metal precursors are removed, the hydrogen consumption became very stable over the repeated TPR/TPO cycles.

[0093] Regarding calcination temperature, it is reported that it directly affects the redox properties of supported catalysis [Y. H. Kim and H. Lee, Redox Property of Vanadium Oxide and Its Behavior in Catalytic Oxidation, vol. 20, no. 12, 1999incorporated herein by reference in its entirety]. However in the examples provided herein, all samples were calcined at same temperature of 750 C. which is the expected temperature of operation of the ODH in a twin fluidized bed configuration. Thus, and for the purposes of the present disclosure, only the composition of ZrO.sub.2 was the parameter affecting both reduction and oxidation of the ODH catalyst, as well as poly-vanadate surface species formed. Regarding poly-vanadates, they can be formed during the reduction cycle, when oxygen vacancies are created [A. M. Elfadly, A. M. Badawi, F. Z. Yehia, Y. A. Mohamed, M. A. Betiha, and A. M. Rabie, Selective nano alumina supported vanadium oxide catalysts for oxidative dehydrogenation of ethylbenzene to styrene using CO2 as soft oxidant, Egypt. J. Pet., vol. 22, no. 3, pp. 373-380, December 2013incorporated herein by reference in its entirety].

[0094] Concerning the percent of vanadium reduced during redox cycles, it was calculated as given by Eq. 10:

[00005]$\begin{array}{cc}\mathrm{Fraction}.Math..Math.\mathrm{of}.Math..Math.\mathrm{Vanadium}.Math..Math.\mathrm{Reduced}.Math..Math.\left(f\right).Math.\%=\frac{{\mathrm{Mw}}_v{V}_{H_2}}{v{V}_g{W}_0}100.Math.\%& \left(\mathrm{Eq}..Math.10\right)\end{array}$

where (1) W.sub.v is the amount of reduced vanadium (g), (2) M.sub.wv represents the molecular weight of vanadium (g/mol), (3) V.sub.H2 stands for the volume of reacted hydrogen (cm.sup.3 at STP), (4) V.sub.g denotes the molar volume of gas (mol/cm.sup.3 at STP), (5) W.sub.o is initial weight of vanadium and v represents the stoichiometric number of hydrogen of the VO.sub.x reduction reaction (H.sub.2+VO.sub.x=H.sub.2O+V.sub.2O.sub.3).

[0095] Assuming that V.sub.2O.sub.5 is the initial reducible catalyst species present on the support [S. Al-Ghamdi, M. Volpe, M. M. Hossain, and H. de Lasa, VO.sub.x/c-Al.sub.2O.sub.3 catalyst for oxidative dehydrogenation of ethane to ethylene: Desorption kinetics and catalytic activity, Appl. Catal. A Gen., vol. 450, pp. 120-130, January 2013incorporated herein by reference in its entirety], the percent of V.sub.2O.sub.5 reduced was found to be 59% for first cycle and 57.7+/2% for the following cycles.

Example 5

Scanning Electron Microscopy (SEM)

[0096] Shape and morphology of the active metal crystals were examined by SEM (Tescan Lyra-3) with a high performance focused ion beam (FIB) at various magnifications (up to 500 kx) using 20 kv voltage. For SEM analysis, the samples were prepared by using a 5 nm Au coating.

[0097] SEM characterization was conducted to investigate active species shape, before and after reduction in TPR. FIG. 6A is an SEM image with magnification of 50 kx, of fresh samples of VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2(2:1) catalyst which were calcinated at 500 C. The images revealed that the impregnation of vanadium oxide resulted in non-uniform sizes and shapes of particles. The pH of the impregnation solution and the support surface affects the nature of vanadium oxide on the support. Al.sub.2O.sub.3 has a surface pH of 8.9, which results in polyvanadate formation (VOV bond). However, thermal treatment converts polyvanadates into monovanadates [I. E. Wachs, Catalysis science of supported vanadium oxide catalysts, Dalton Trans., vol. 42, no. 33, pp. 11762-9, September 2013incorporated herein by reference in its entirety]. Therefore, the fresh sample has isolated and bulk phase VO.sub.x as indicated by XRD peaks.

[0098] FIG. 6B is an SEM image for the reduced sample of VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 (2:1), which reduced at 500 C. under H.sub.2 flow. Since there are many forms of VO.sub.x that can appear on the support surface, such as V.sub.2O.sub.5 and VO.sub.2, these reduced oxides are mostly present in crystalline and agglomerated form.

[0099] Reduction of samples at 500 C. did not affect alumina and/or zirconia phases. However, a slight weight loss may occur, as -alumina tends to be modified into -alumina when the temperature rises to 700 C. This results in the loss of surface area. Therefore, the support can be considered stable. Similar results were concluded in open literature [Anna G. and Aftanas G., The global approach to TPD and isothermal adsorptiondesorption kinetics., Proceedings on, Tatransk Matliare (SK), 26-30, May 2003incorporated herein by reference in its entirety]. The major change happens after the reduction of VO.sub.x on the support surface and it is reversible

Example 6

NH.SUB.3 .Temperature Programmed Desorption (NH.SUB.3.-TPD)

[0100] The purpose of the NH.sub.3-TPD test was to determine catalyst total acidity as catalyst acidity affects metal-support interactions. The metal support interactions were also evaluated by TPD kinetics analysis. Furthermore, NH.sub.3-TPD was utilized to determine the quantity and strength of the acid sites available, on the surface of the prepared catalyst samples. NH.sub.3-TPD experiments were conducted using a Micromeritics: AutoChem II 2029 Analyzer. A catalyst sample (0.15-0.20 g) was placed in a U-shaped quartz container and degassed for 2 h at 300 C., in a flow of helium at 30 ml/min. The samples were then cooled to 120 C. and brought to saturation with ammonia (due to its strong basicity and small molecular size) using a NH.sub.3/He gas mixture (5% NH.sub.3/He), for one hour at a rate of 50 ml/min. Furthermore, ammonia allows one to determine the total acidity and strength of acid sites, for wide range of temperatures [R. Bulnek, P. imanec, and M. Setnika, Possibility of VO.sub.x/SiO.sub.2 Complexes Speciation: Comparative Multi-wavelength Raman and DR UV-vis Study, Phys. Procedia, vol. 44, pp. 195-205, January 2013incorporated herein by reference in its entirety]. After that, the ammonia flow was stopped, and replaced by a He purge gas, fed at the rate of 50 ml/min. This was done for 1 h, at 120 C. to remove the physically adsorbed ammonia. Following this step, the temperature was raised up to 500 C. at different heating rates (10, 20 and 30 C./min). As the temperature was increased, the ammonia desorbed as it gained enough energy to overcome the activation energy barrier. The desorbed concentration of ammonia was recorded using a TCD detector. FIG. 7 shows the NH.sub.3-TPD profiles of the catalyst samples with various Al.sub.2O.sub.3/ZrO.sub.2 ratios. ZrO.sub.2 affects metal-support interactions especially at low and intermediate metal loading [J. R. Soto, S. G. Cho, Y. Il Pae, and S. Hayashi, Characterization of Vanadium OxideZirconia Catalyst, vol. 177, no. 0076, pp. 170-177, 1996incorporated herein by reference in its entirety]. It can be seen from FIG. 7 that desorption profiles of the samples have not significantly changed after the ZrO.sub.2 modification. Total acidity was calculated by calibrating the TCD signals to the volume of NH.sub.3 desorbed and by numerical integration of the area under the TPD profile (FIG. 7). A heating rate of 10 C./min was used, and samples were weighted during TPD test. All samples weighted 0.2 g. Eq 11 was used to calculate sample total acidity as follows:

[00006]$\begin{array}{cc}\mathrm{Total}.Math..Math.\mathrm{acidity}.Math..Math.\left(\mathrm{ml}.Math..Math.{\mathrm{NH}}_3.Math.\text{/}.Math.g\right)=\frac{a}{w.Math..Math.}& \left(\mathrm{Eq}..Math.11\right)\end{array}$

where, a is the area under the curve after TCD signal calibration (ml NH.sub.3 C./min), w represents sample weight and stands for the heating rate C./min.

[0101] Sample total acidity was found to be in the range between 2 and 6 (mlNH.sub.3/g.cat) as shown in Table 2. The total acidity was reduced when decreasing the Al.sub.2O.sub.3/ZrO.sub.2 ratios (increasing the ZrO.sub.2 content). Zirconia and vanadium loading diminishes samples acidity by blocking acid sites [D. Sun, R. Narita, F. Sato, Y. Yamada, and S. Sato, Catalytic Dehydration of 1,2-Propanediol into Propanal over Ag-Modified Silica;Alumina, Chem. Lett., vol. 43, no. 4, pp. 450-452, 2014incorporated herein by reference in its entirety]. However, increasing the ZrO.sub.2 ratio decreased total acidity.

TABLE-US-00002 TABLE 2 Estimated.sup.b TPD model parameters for catalyst samples at 10 C./min heating rate. K.sub.des, 0 E.sub.des V.sub.des (ml Sample (cm.sup.3/min) kJ/mol R.sup.2 AIC.sup.c NH.sub.3/g .Math. cat) 15% VO.sub.x Al.sub.2O.sub.3ZrO.sub.2(2:1) 3.9 10.sup.6 75.44 3.5 0.99 64252 5.87 15% VO.sub.x Al.sub.2O.sub.3ZrO.sub.2(1:1) 5.6 10.sup.6 77.88 3.8 0.99 64055 3.4 15% VO.sub.x/Al.sub.2O.sub.3ZrO.sub.2(1:2) 14.9 10.sup.6 80.52 4.sup. 0.99 51751 2.75 .sup.bConfidence interval was set to be 95% .sup.cAkiake information criterion

[0102] This observation suggests that ZrO.sub.2 enhances vanadia species isolation on the surface of the catalyst. This creates more active sites, since ZrO.sub.2 as mentioned before, has a lower acidity than alumina [S. Al-Ghamdi, M, Volpe, M. M. Hossain, and H. de Lasa, VO.sub.x/c-Al.sub.2O.sub.3 catalyst for oxidative dehydrogenation of ethane to ethylene: Desorption kinetics and catalytic activity, Appl. Catal. A Gen., vol. 450, pp. 120-130, January 2013incorporated herein by reference in its entirety].

[0103] The NH.sub.3-TPD data was further treated to estimate the desorption kinetic parameters such as the desorption energy E.sub.des and the frequency factor k.sub.des,0. These kinetic parameters are very important to assess the metal-support interaction. The NH.sub.3-TPD data can be modeled as described in [R. Bulnek, P. imanec, and M. Setnika, Possibility of VO.sub.x/SiO.sub.2 Complexes Speciation: Comparative Multi-wavelength Raman and DR UV-vis Study, Phys. Procedia, vol. 44, pp. 195-205, January 2013incorporated herein by reference in its entirety] and used to estimate these parameters under the following assumptions: [0104] iHomogeneous catalyst surface, k.sub.d=(E.sub.des/RT). [0105] iiAmmonia does not re-adsorb during experiment. [0106] iiiUniform adsorbate concentration in the gas flow. [0107] ivFirst order adsorption rate in surface coverage.
A high gas flow rate was maintained to satisfy the previous assumptions. The rate of NH.sub.3 desorption can be expressed as [D. Ahchieva, M. Peglow, S. Heinrich, L. Mrl, T. Wolff, and F. Klose, Oxidative dehydrogenation of ethane in a fluidized bed membrane reactor, Appl. Catal. A Gen., vol. 296, no. 2, pp. 176-185, December 2005incorporated herein by reference in its entirety]:

[00007]$\begin{array}{cc}{r}_{\mathrm{des}}=-V_m\left(\frac{d.Math..Math.{}_{\mathrm{des}}}{\mathrm{dt}}\right)=k_{d,0}.Math.{}_{\mathrm{des}}.Math.\exp \left[\frac{E_{\mathrm{des}}}{R}.Math.\left(\frac{1}{T}-\frac{1}{T_m}\right)\right]& \left(\mathrm{Eq}..Math.12\right)\end{array}$

where, (1) .sub.des is the surface coverage, (2) d.sub.d,0 represent the pre-exponential factor, (3) T.sub.m stands for the centering temperature. By rising the temperature gradually with a constant value , the following equations can be applied:

[00008]$\begin{array}{cc}T=T_0+.Math..Math.t& \left(\mathrm{Eq}..Math.13\right)\\ \frac{\mathrm{dT}}{\mathrm{dt}}=& \left(\mathrm{Eq}..Math.14\right)\\ \left(\frac{d.Math..Math.{}_{\mathrm{des}}}{\mathrm{dt}}\right)=\left(\frac{d.Math..Math.{}_{\mathrm{des}}}{\mathrm{dT}}\right).Math.\left(\frac{\mathrm{dT}}{\mathrm{dt}}\right)=\left(\frac{d.Math..Math.{}_{\mathrm{des}}}{\mathrm{dt}}\right)& \left(\mathrm{Eq}..Math.15\right)\end{array}$

Eq. 13 and Eq. 14 give:

[00009]$\begin{array}{cc}\left(\frac{d.Math..Math.{}_{\mathrm{des}}}{\mathrm{dt}}\right)=\frac{k_{\mathrm{des},0}}{v_m}.Math.{}_{\mathrm{des}}.Math.\exp \left[\frac{-E_{\mathrm{des}}}{R}.Math.\left(\frac{1}{T}-\frac{1}{T_m}\right)\right].Math..Math.\mathrm{where}.Math.\text{:}& \left(\mathrm{Eq}..Math.16\right)\\ {}_{\mathrm{des}}=1-\frac{V_{\mathrm{des}}}{V_m}& \left(\mathrm{Eq}..Math.17\right)\end{array}$

Combining Eq. 10 and Eq. 11 would result in:

[00010]$\begin{array}{cc}\left(\frac{d.Math..Math.{}_{\mathrm{des}}}{\mathrm{dt}}\right)=\frac{k_{\mathrm{des},0}}{v_m}.Math.{}_{\mathrm{des}}.Math.\exp \left[\frac{-E_{\mathrm{des}}}{R}.Math.\left(\frac{1}{T}-\frac{1}{T_m}\right)\right]& \left(\mathrm{Eq}..Math.18\right)\end{array}$

[0108] Eq. 18 was fitted to the experimental data using the Mathematica NonlinearModelFit built-in function at a heating rate of 10 C./min for all samples. In all experiments, ammonia pre-adsorbed at 120 C. and samples weight was 0.2 g. Parameters obtained are shown in Table 2.

[0109] The coefficient of determination R.sup.2 was found to be above 0.99. In all cases, this indicates a good regression. Akaike Information Criterion (AIC) was also used as a measure of the relative quality of a statistical model to the experimental data set. In the literature, when it is used, it is reported, to give large negative values if the fit is good, this can be seen in Table 2.

[0110] As seen in Table 2, that the activation energies for the ZrO.sub.2 containing samples are higher than those of the bare Al.sub.2O.sub.3 and the VO.sub.x/Al.sub.2O.sub.3. This suggests a stronger interaction between vanadium species and the support [S. Al-Ghamdi, M. Volpe, M. M. Hossain, and H. de Lasa, VO.sub.xc-Al.sub.2O.sub.3 catalyst for oxidative dehydrogenation of ethane to ethylene: Desorption kinetics and catalytic activity, Appl. Catal. A Gen., vol. 450, pp. 120-130, January 2013incorporated herein by reference in its entirety]. This also confirms the presence of isolated vanadium oxide species. On the other hand, vanadium species interaction may result in the formation of VO.sub.2 which will lead to a lowering of the catalyst oxygen-carrying capacity [R. Bulnek, P. imanec, and M. Setnika, Possibility of VO.sub.x/SiO.sub.2 Complexes Speciation: Comparative Multi-wavelength Raman and DR UV-vis Study, Phys. Procedia, vol. 44, pp. 195-205, January 2013incorporated herein by reference in its entirety]. On the whole, the intermediate interaction between active sites and supports is favorable. TPD kinetics show increased metal-support interaction, indicated by high desorption energy due to the introduction of ZrO.sub.2. Higher metal-support interaction decreases the VO.sub.x reducibility. Thus, catalyst activity is consistent with TPR results. Furthermore, decreased catalyst activity can reduce conversion of ethane. However, it is expected to increase ethylene selectivity by controlling O.sub.2 release.

Example 7

CREC Riser Simulator Setup

[0111] The reactivity and the stability of the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 catalyst samples were established using a CREC Riser Simulator, whose set-up is shown in FIG. 8A [S. Al-Ghamdi, M. Volpe, M. M. Hossain, and H. de Lasa, VO.sub.x/c-Al.sub.2O.sub.3 catalyst for oxidative dehydrogenation of ethane to ethylene: Desorption kinetics and catalytic activity, Appl. Catal. A Gen., vol. 450, pp. 120-130, January 2013incorporated herein by reference in its entirety]. The reactor has a capacity of 53 cm.sup.3. It is a batch unit designed for catalyst evaluation and kinetic studies under fluidized bed reactor conditions. The major components of the CREC Riser Simulator are shown in FIG. 8B. These components include a vacuum box, a series of sampling valves, a timer, two pressure transducers and three temperature controllers. The product gas was analyzed by gas chromatography (GC) with a thermal conductivity detector (TCD) and a flame ionization detector (FID).

[0112] As shown in FIG. 8B, the main reactor consists of a lower shell and an upper shell. These two shells allow easy access to the reactor to load and unload catalyst samples. The lower shell houses a basket that contains the catalyst sample. The catalyst basket is bound by two grids, trapping the catalyst and restraining its mobility within this chamber. This reactor was designed in a way that an annular space is created between the outer portion of the basket and the inner part of the lower reactor shell containing the basket. This annular space facilitates the recirculation of gaseous reactants and/or products by rotation of an impeller positioned above the catalyst basket. A metallic gasket is used to seal the upper and the lower shells of the reactor. A packing gland assembly with a cooling jacket supports and seals the impeller shaft. Upon the rotation of the impeller at high speed (up to 7500 rpm), gas is forced both outward in the impeller section and downwards in the outer reactor annulus, causing the solids material (catalyst) to become fully fluidized.

Example 8

Ethane ODH Experiments

[0113] The ODH of ethane to ethylene experiments were conducted at various temperatures and contact times. The selected temperatures for the experiments were chosen to be consistent with the reduction temperatures of the catalysts, as reported in the TPR analysis.

[0114] In a typical run, 0.4 g of oxidized catalyst sample was loaded into the reactor basket and the leak test was conducted Following the leak test the system was purged by flowing argon. The temperature program was started to heat the reactor to the desired temperature. The argon flow was maintained to keep the reactor from any interference of gas phase oxygen. Once the reactor temperature reached to the desired temperature, the argon flow was discontinued. The reactor isolation valve was closed when it reached the desired pressure level. At this stage the vacuum pump was turned on to evacuate the vacuum box down to 20.7 kPa (3.75 psi). The catalyst was fluidized by rotating the impeller. At this point, the ethane feed was injected into the reactor by using a preloaded gas tight syringe. The reaction continued for a pre-specified time. At the termination point, the isolation valve between the reactor and vacuum box opened automatically and transferred all the reactant and products into the vacuum box. The gas samples in the vacuum bottle were analyzed using an Agilent 7890A GC equipped with both a TCD and a FID detector. For each catalytic run, the product samples were analyzed three times to ensure the accuracy of the analysis. Finally, the product analysis data were used to calculate conversion and selectivity of various products. The following definitions were used in calculating the conversion and selectivity, respectively:

[00011]$\begin{array}{cc}\mathrm{Conversion}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}=\frac{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}.Math..Math.\mathrm{converted}}{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}.Math..Math.\mathrm{fed}}100.Math.\%& \left(\mathrm{Eq}..Math.19\right)\\ \mathrm{Selectivity}.Math..Math.\mathrm{to}.Math..Math.\mathrm{product}=\frac{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{product}}{\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{alkane}.Math..Math.\mathrm{reacted}-\mathrm{Moles}.Math..Math.\mathrm{of}.Math..Math.\mathrm{product}}100.Math.\%& \left(\mathrm{Eq}..Math.20\right)\end{array}$

[0115] The fluidized ODH of ethane experiments were conducted in a CREC Riser Simulator using pure ethane feed (99.95% ethane). For comparison, all three catalysts (VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2) with different -Al.sub.2O.sub.3/ZrO.sub.2 ratios (constant 15% VO.sub.x loading) were evaluated under same experimental conditions. The catalyst activity and product selectivity was evaluated using 0.4 g of oxidized catalysts and 2 ml of ethane injection. The product analysis of the preliminary experiments shows that C.sub.2H.sub.6, C.sub.2H.sub.4, CO.sub.2 and CO are the major products of the gas phase oxygen free ODH of ethane reaction. Based on this product analysis, the following possible reactions are considered to be involved under the studied reaction conditions:

[0116] Desired reaction, ethane to ethylene:

[00012]$\begin{array}{cc}{C}_2.Math.H_6.Math.\stackrel{\mathrm{VOx}/\mathrm{Al}.Math..Math.2.Math.O.Math..Math.3-\mathrm{ZrO}.Math..Math.2}{}.Math.C_2.Math.H_4+H_2.Math.O& \left(\mathrm{Eq}..Math.21\right)\end{array}$

Undesired, complete oxidation of ethane:

[00013]$\begin{array}{cc}{C}_2.Math.H_6.Math.\stackrel{\mathrm{VOx}/\mathrm{Al}.Math..Math.2.Math.O.Math..Math.3-\mathrm{ZrO}.Math..Math.2}{}.Math.{\mathrm{CO}}_2+\mathrm{CO}+3.Math..Math.H_2.Math.O& \left(\mathrm{Eq}..Math.22\right)\end{array}$

Undesired, complete oxidation of ethylene:

[00014]$\begin{array}{cc}{C}_2.Math.H_4.Math.\stackrel{\mathrm{VOx}/\mathrm{Al}.Math..Math.2.Math.O.Math..Math.3-\mathrm{ZrO}.Math..Math.2}{}.Math.{\mathrm{CO}}_2+\mathrm{CO}+2.Math..Math.H_2.Math.O& \left(\mathrm{Eq}..Math.23\right)\end{array}$

Therefore, the ODH reaction between the catalyst and the ethane feed has to be developed at the reaction conditions maximizing the desired ethylene, product selectivity and minimizing complete CO.sub.x combustion.

[0117] The temperature during the experiments was varied from 525 C. to 600 C., while the contact time was adjusted between 20 and 50 s. Alter each ODH run, the catalyst was regenerated by supplied air at 550 C. for 10 min.

[0118] In older to demonstrate the effects of ZrO.sub.2, the ethane conversion and product data are reported per gram VO.sub.x loading on the Al.sub.2O.sub.3/ZrO.sub.2 support basis. FIG. 9 displays the product selectivity at various Al.sub.2O.sub.3/ZrO.sub.2 ratios. It can be noticed that all the catalyst samples studied give good selectivity to ethylene, although the highest 37.9% ethane conversion was achieved at the 2:1 -Al.sub.2O.sub.3/ZrO.sub.2 ratio. The ethane conversion further decreased with the increase of the ZrO.sub.2 content (decreasing -Al.sub.2O.sub.3/ZrO.sub.2 ratio). This was expected after the TPR analysis of the samples, which showed that the oxygen-carrying capacity of the samples decreased with the increase of the ZrO.sub.2 content on the support. Interestingly, ethane selectivity slightly increased when the -Al.sub.2O.sub.3/ZrO.sub.2 ratio was decreased from 2:1 to 1:1. At these -Al.sub.2O.sub.3/ZrO.sub.2 ratios, up to 90% ethylene selectivity was achieved at 600 C. Further increases of ZrO.sub.2, diminished however, ethylene selectivity significantly.

[0119] On the basis of the results obtained on can conclude that overall, both the ethane conversion and ethylene selectivity were increased by augmenting the ZrO.sub.2. This is due to enhanced catalyst activity via the formation of reducible poly-vanadates [E. Nouri, M. Shahmirfi, H. R. Rezaie, and F. Talayian, The effect of alumina content on the structural properties of ZrO.sub.2-Al.sub.2O.sub.3 unstabilized composite nanopowders, pp. 1-8, 2012; I. E. Wachs, Catalysis science of supported vanadium oxide catalysts, Dalton Trans., vol. 42, no. 33, pp. 11762-9, September 2013each incorporated herein by reference in its entirety]. This agrees with the TPR results obtained as well in this study. However, at high ZrO.sub.2 content, crystalline VO.sub.x species are also formed. This results in both a decreasing ethane conversion and ethylene selectivity. TPD kinetics also shows an increased metal-support interaction due to high desorption energies. This high desorption energies were likely caused by an increased surface heterogeneity, which can favor catalyst ethylene selectivity by controlling the lattice O.sub.2 released [Qing Sun, Yuchuan Fu, Jingwei Liu, Aline Auroux, Jianyi Shen, Structural, acidic and redox properties of V.sub.2O.sub.5-TiO.sub.2-SO.sub.4.sup.2 catalysts, Appl. Cat. A 334 (2008) 26-34incorporated herein by reference in its entirety].

[0120] FIG. 10 shows ethane conversion and ethylene selectivity over three reduction and oxidation cycles for a VO.sub.x/Al.sub.2O.sub.3-ZrO.sub.2 (2:1) catalyst sample. Stable performance was consistently obtained, which indicates the sample thermal stability and ability to be regenerated. This observation is well in agreement with consecutive TPR/TPO data which also show a close level of reducibility during repeated reductions and oxidations.

[0121] FIG. 11 displays the relationship between ethane conversion and ethylene selectivity with reaction temperature. It can be seen that as the reaction temperature increases, with the unprompted VO.sub.x/-Al.sub.2O.sub.3 catalyst, the conversion of ethane is increased from 13.75% at 550 C. to 18.80% at 600 C. On the contrary, with the VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2, the ethane conversion was slightly decreased from 13.75% at 550 C. to 11.45% at 600 C.

[0122] FIG 12 shows product selectivity when using VO.sub.x/c-Al.sub.2O.sub.3 and when using VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 (2:1) catalyst samples. Ethylene selectivity reaches 90.3% when utilizing a VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 (2:1) catalyst sample and only 42% when utilizing a VO.sub.x/c-Al.sub.2O.sub.3 sample. This can be attributed to the ZrO.sub.2 effect, which enhances metal-support interaction, as mentioned earlier. Lower vanadium reducibility decreases O.sub.2 availability for combustion reactions, consequently suppressing the formation of CO.sub.2 and CO gases. Catalyst selectivity to CO.sub.x gases versus temperature is also shown in FIG. 12. The highest CO.sub.2 selectivities obtained were 44.2% for a VO.sub.x/-Al.sub.2O.sub.3-ZrO.sub.2 (2:1) sample and 15.5% for a sample without ZrO.sub.2.

[0123] Furthermore, in the sample containing ZrO.sub.2, the formation of CO.sub.x decreased with increasing temperature, indicating the ZrO.sub.2 enhanced catalyst activity and selectivity at a high temperature of 600 C. This is in agreement with TPR results as reported in FIG. 3. On the other hand, the VO.sub.x/c-Al.sub.2O.sub.3 sample produced more CO.sub.x at higher temperatures which was assigned to the increased influence of complete combustion in ODH. At higher temperature, selective role of catalyst appears as removal of H.sub.2 which as same as in TPR results, the selective O.sub.2 comes from VO-support bond which release this oxygen at higher temperature [R. Bulnek, P. imanec, and M. Setnika, Possibility of VO.sub.x/SiO.sub.2 Complexes Speciation: Comparative Multi-wavelength Raman and DR UV-vis Study, Phys. Procedia, vol. 44, pp. 195-205, January 2013incorporated herein by reference in its entirety].

[0124] The reaction time influence in the experiments in the CREC Riser Simulator at 550 C. is shown in FIGS. 13A and 13B, for both VO.sub.x--Al.sub.2O.sub.3-ZrO.sub.2 (1:2) and VO.sub.x/-Al.sub.2O.sub.3. In both cases, the ethane conversion augments progressively, as expected, with reaction time. Furthermore, as shown in FIG. 13A, the ZrO.sub.2 addition stabilizes ethylene and CO.sub.x selectivities in the 75%-78% and 20-24% ranges respectively. These results are in significant contrast with the observations for the ODH catalyst sample without ZrO.sub.2 (FIG. 13B), where selectivities to ethylene and CO.sub.x range in the 40-50% and 20-25% respectively.

[0125] Thus, it can be noticed that the introduction of ZrO.sub.2 in the alumina support, enhances ethylene selectivity and stability. This is consistent with the ZrO.sub.2 lowering support total acidity and also reducing Lewis acidity, as shown in NH.sub.3-TPD analysis. This leads to limited cracking and CO.sub.x production. Similar results were obtained by others, when the SAPO-34 catalyst was employed in ethane ODH, where CH.sub.4 traces were detected, as a result of an increased cracking influence [L. Marchese, Acid SAPO-34 Catalysts for Oxidative Dehydrogenation of Ethane, J. Catal., vol. 208, no. 2, pp. 479-484, June 2002incorporated herein by reference in its entirety]. Thus, it can be hypothesized that, by decreasing acidity, vanadium reductivity is mitigated. This affects both the reduction oxidation rates, explaining the lower ethane conversions for the alumina loaded with ZnO.sub.2, as shown in FIG. 13A. ZrO.sub.2 enhances however the metal-support interaction leading to higher ethylene selectivity to ethylene values as a result of dehydrogenation.

[0126] It should be mentioned that as expected at a certain point of ZrO.sub.2 loading, the reduction of V.sub.2O.sub.5 species become more difficult. This is shown in XRD and TPR profiles, where VO.sub.2 was detected, when fresh samples were treated with H.sub.2 at higher temperatures (above 500 C.). This can affect the nature of the VO.sub.x species on the support surface and the types of bonds between these species.

[0127] It was reported that the V-support interaction and the V loading, determine the type of surface bonds and thus, what type of VO.sub.x species exist on the support surface [I. E. Wachs, Catalysis science of supported vanadium oxide catalysts., Dalton Trans., vol. 42, no. 33, pp. 11762-9, September 2013incorporated herein by reference in its entirety]. There are several types of VO.sub.x species, such as isolated vanadium oxide species, dimeric vanadium oxide species, two-dimensional vanadium oxide chains and V.sub.2O.sub.5 crystals. VO.sub.x on different supports were reported to contain isolated, dimeric and crystalline V.sub.2O.sub.5 [R. Bulnek, P. imanec, and M. Setnika, Possibility of VO.sub.x/SiO.sub.2 Complexes Speciation: Comparative Multi-wavelength Raman and DR UV-vis Study, Phys. Procedia, vol. 44, pp. 195-205, January 2013incorporated herein by reference in its entirety]. These VO.sub.x species contain VO terminal bonds with VOV and VO-support bonds. The VOV bond is associated with polymeric VO.sub.x species. Previous studies showed that the VOV has no effect in ODH reactions.

[0128] In summary, it can be stated that even if the specific details of various vanadium species formed on -Alumina VOx catalyst doped with ZrO.sub.2 are not precisely known, it is proven that under the specified loadings of ZrO.sub.2 dopant, there is a significant and valuable enhancement of ethylene selectivity for this ODH fluidizable catalyst.

[0129] Thus, the foregoing discussion discloses and describes merely exemplary embodiments of the present invention. As will be understood by those skilled in the art, the present invention may be embodied in other specific forms without departing from the spirit or essential characteristics thereof. Accordingly, the disclosure of the present invention is intended to be illustrative, but not limiting of the scope of the invention, as well as other claims. The disclosure, including any readily discernible variants of the teachings herein, defines, in part, the scope of the foregoing claim terminology such that no inventive subject matter is dedicated to the public.