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Review

V-Containing Mixed Oxide Catalysts for Reduction–Oxidation-Based Reactions with Environmental Applications: A Short Review

by
M. Olga Guerrero-Pérez
Departamento de Ingeniería Química, Universidad de Málaga, E-29071 Málaga, Spain
Catalysts 2018, 8(11), 564; https://doi.org/10.3390/catal8110564
Submission received: 19 October 2018 / Revised: 5 November 2018 / Accepted: 6 November 2018 / Published: 20 November 2018
(This article belongs to the Special Issue New Developments in Heterogeneous Partial and Total Oxidation Catalysis)
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Abstract

:
V-containing mixed oxide catalytic materials are well known as active for partial oxidation reactions. Oxidation reactions are used in industrial chemistry and for the abatement of pollutants. An analysis of the literature in this field during the past few years shows a clear increase in the use of vanadium-based materials as catalysts for environmental applications. The present contribution makes a brief revision of the main applications of vanadium containing mixed oxides in environmental catalysis, analyzing the properties that present the catalysts with a better behavior that, in most cases, is related with the stabilization of reduced vanadium species (as V4+/V3+) during reaction.

1. Introduction: Main Applications of Vanadium Oxide-Based Materials in Catalysis

The chemical reactions that involve a change in the oxidation state of products (oxidations and reductions) are of great importance in industrial chemistry and environmental engineering, since most degradation reactions of pollutants involve oxidation or reduction. To catalyze these reactions, the catalytic material must have redox sites able to reduce/oxidize the starting molecule.
Most partial oxidation reactions take place through the Mars-van-Krevelen mechanism, in which the lattice oxygen of the oxide catalysts is incorporated to the oxidation product [1]; then, such a reduced site is reoxidized by the molecular oxygen reactant, restoring the original catalyst state. Experimental evidence of such a mechanism has been found for different oxidation reactions and several oxide catalysts [2]. Effective catalysts must exchange their lattice oxygen during reaction; they must have dynamic structures capable of changing the oxidation state during the reaction cycles. The vanadium oxides are able to be with oxidation states V, IV, and III, and to interconvert with relative ease, which makes them effective oxidation catalysts [3]. However, not all redox reactions of environmental interest operate on this mechanism.
The most studied catalytic systems for partial oxidation reactions are those containing vanadium [4]. VOx-based catalysts are efficient oxidation catalysts due to their redox properties, and during the past few decades several studies have focused on the development of mixed-oxide catalytic systems containing vanadium; in this manner, the use of another compound (dopant, component, or support) modulates the activity of the catalysts. Thus, there are several well-known mixed-oxide vanadium-containing catalytic systems that have been developed during the past few decades: For example, the VPO (Vanadium-Phosphorous-Oxides) catalyst [5,6,7,8,9], which is commercially used for the transformation of n-butane into maleic anhydride; Vanadium-Animony Oxides (VSbO) [10,11,12,13,14], which is used mainly for ammoxidation reactions; or the Mo–V multioxide system [15,16,17,18,19,20], used for propane transformation into acrylic acid. Figure 1 illustrates an analysis of the literature on vanadium oxide catalysts, underlining their main uses and their evolution during the last few decades. Figure 1A plots the total number of papers when the words “vanadium oxide catalysts”. The total number of papers published per year has remained fairly stable in the last 20 years; however, the number of these papers that also include the word “environmental” is increasing. The percentage of “environmental” with respect to the total number per year is also shown in Figure 1A; it increases continuously, from 1–5% in 1988–1991 to more than 60% during the last three years (from 2015). A deep analysis of these papers shows how, in the 1990s, most studies focused on the development of VOx-supported catalysts for partial oxidation and ammoxidation reactions; thus, they were mainly focused on chemical reactions for the production of chemical intermediates with an interest in petrochemical industry (such as butane to maleic anhydride [21], toluene to benzonitrile [22,23], methane to formaldehyde [24], propane to acrylonitrile [10,11], and alkane oxydehydrogenation (ODH) [25], among others). It is observed, therefore, in the study of the historical evolution of the bibliography as in the eighties–nineties that the interest was in the synthesis of molecules and, although these applications are still being developed, the interest in the applications in environmental catalysis is increasing. Figure 1B illustrates the main environmental applications in which these materials are used, based on the number of papers that, in addition to “Vanadium Oxide Catalysts”, also contain “SCR”, “photocatalysis”, and “total oxidation”. These data reveal that SCR (selective catalytic reduction) is the most studied environmental process in which vanadium-based catalysts have been explored.
Figure 1 clearly accounts for the significant number of review papers that focus on vanadium oxide catalytic-based materials for alkane partial (am)oxidations, including oxidative dehydrogenations [26,27,28,29,30]. Figure 1 also illustrates that many environmental applications have been developed with VOx catalytic materials during the past twenty years. Thus, the objective of this contribution is to review the main environmental catalytic applications for vanadium oxide catalytic materials.

2. Removal of NOx

One of the most important environmental issues that catalysis engineering must face is the abatement of harmful compounds, such as oxides of nitrogen (NOx), from both stationary and mobile sources. During the last few years, more efforts have focused on the development of catalytic converter technologies for diesel-powered vehicle engines that operate at high air/fuel ratios. Several techniques seem feasible for NOx abatement, one of the most promising being ammonia- or urea-selective catalytic reduction (SCR) [31].
Several catalytic systems have shown to be promising for this process, with active phases such as Cu- and Fe-based catalysts [31,32,33] or Mn–Ce–O mixed oxides [34,35]; V-based catalysts are also very promising [36]. CeO2- and TiO2-supported vanadia catalysts have been extensively studied for NOx removal. Forzatti’s group investigated V–Mo–O/TiO2 catalysts [37] and they reported that the ternary V–Mo–O/TiO2 were more active in the SCR reaction at low temperatures than the corresponding binary VOx/TiO2 and MoOx/TiO2 at a given metal oxide loading. They described that the simultaneous presence of V and Mo enhances the redox properties of the catalysts and, thus, their reactivity. The improved catalytic properties of Mo–V–O oxides have also been reported for partial oxidation reactions, such as the dehydrogenation of propane [38,39,40], propane ammoxidation to acrylonitrile [41,42,43], or the selective propane oxidation into acrylic acid [44,45]. It has been demonstrated that molybdenum favors the presence of reduced vanadium V4+ species, which are stabilized in a rutile-like structure that is responsible for the redox cycle [46]. Temperature Programmed Reduction (TPR) experiments [37] show that the addition of Mo to V/TiO2 favors vanadium reduction, with Mo–V–O catalysts being more easily reduced with respect the corresponding binary supported samples and their bulk counterparts. Similar results were found with W: Rhe V–W–O/TiO2 catalysts presented a higher SCR performance than VOx/TiO2 and WOx/TiO2 catalytic systems [47,48], since tungsten sites improve the reducibility and formation of reduced vanadium species [49]. Thus, both Mo and/or W enhance the reduction of VOx species, this V4+/V3+ species being the active sites for NO2 formation [50]. NO oxidation to NO2 is important to the SCR reaction at low temperatures due to the so-called “fast-SCR” and “standard SCR”, according to Reactions (A) and (B), respectively [49]:
(A)
NO + NO2 + NH3 → N2 + H2O “fast-SCR”
(B)
NO + NH3 + O2 → N2 + H2O “standard SCR”
Nova et al. studied the mechanism of the fast-SCR over V-containing catalysts using transient conditions [51]. They described that the first step was the NO2 dimerization and disproportion to nitric and nitrous acid; then, adsorbed ammonia forms ammonium nitrite (which decomposes to N2 and water) and ammonium nitrate (only if there is no suitable reducing agent). When NO is included in the feed, it can effectively reduce ammonium nitrate to ammonium nitrite, which could decompose to N2; thus, complete selectivity to N2 was achieved by adding NO to the NH3/NO2 mixtures. The same group also investigated the redox features in this mechanism over V-based catalysts [52]. It was shown that both NO2 and HNO3 reoxidize the V–W–O/TiO2 catalysts at a much lower temperature than O2; furthermore, they significantly enhance NO + NH3 reactivity below 250 °C via the buildup of adsorbed nitrates, which act as a reservoir of oxidizing agents. These features were not observed over a V-free WO3/TiO2 catalyst, pointing out the role of the vanadium redox properties, and can explain the higher efficiency of the “fast” SCR compared with the “standard” SCR. Thus, vanadium sites are the active (redox) species of these catalysts, which are reduced by the reaction between NO and NH3 and then reoxidized either by oxygen (standard SCR) or by nitrates (fast SCR) [51,52]. Wokaun et al. also investigated this [53] through transient experiments and in situ Raman spectroscopy to study the reoxidation of the vanadium species on a W–V–O/TiO2 sample. They found that the vanadium reduced species (V4+) formed during the reduction of NO with NH3 are reoxidized faster by NO2 than by oxygen, resulting in an increased reaction rate of the fast SCR reaction. Thus, reduced vanadium species appear as the most active sites and the use of a co-element (such as Mo and/or W) modulates vanadium oxide activity [54] [55]. Conversely, basic elements, such as K or Ca, titrate surface acidity and decrease the reducibility of vanadium oxide species, being detrimental to catalytic behavior [56,57,58]. Thus, the poisoning effects impinge both the surface acidity and reducibility of vanadium oxide species.
Carbon materials are convenient catalytic supports, since they provide a high surface area and mechanical and chemical stability; the structure of vanadium oxide species on carbons has been extensively described [59,60]. The structure found is similar to that on oxide supports and surface polymeric or isolated VOx species, depending on the coverage. Lazaro et al. [61,62,63] have reported the use of carbon-based monoliths as supports for vanadium and tungsten oxide catalysts for the SCR process. They found some advantages with respect the conventional titania-supported catalysts, since carbon-supported ones were not deactivated by SO2 [64]. In addition, the higher surface area of carbons with respect to TiO2 enables to disperse a higher amount of active vanadium species per weight of support [59]. Following this approach, they proposed a novel synthesis procedure by the sulphation of the catalysts with a mixture of SO2 + O2 [65,66]. They found that the pre-sulphidating catalysts duplicate conversion values. Their work showed that both ammonia adsorption and activating sites were different in the sulphated catalysts; in addition, sulphated catalysts present sulphate groups located near vanadia sites, thus facilitating vanadium reoxidation during redox cycles. In addition, sulphate groups did not contribute to the gasification of the most labile carbon groups of support.
Literature shows the promoting effect of cerium, both as a dopant and as support for the V-based catalysts during the SCR reaction. Ge et al. [67] studied the effect of adding Ce to V–W–O/TiO2 catalysts with low vanadium loadings. Cerium was present mainly as Ce3+ and was beneficial for the oxidation of NO to NO2, accelerating the SCR reaction. Huang et al. [68] also described that Ce-containing VOx/TiO2 and VMoOx/TiO2 catalysts exhibited high resistance to H2O and SO2 poisoning at low temperatures; they reported that Ce sites led to a higher concentration of chemisorbed oxygen, minimizing nonselective oxidation of ammonia to NOx. Diffuse Reflectance Infrared Fourier Transform Spectroscopy (DRIFTS) measurements [69] revealed that Ce contributes to the formation of NO2 and monodentate nitrate species, both being reactive intermediates for the SCR reaction; the characterization also indicated that the redox cycle in the presence of Ce (V4+ + Ce4+ ↔ V5+ + Ce3+) accounts for an excellent SCR catalytic performance for the Ce-doped V-based catalysts.

3. Removal of H2S

H2S is a major contaminant produced in most energy-related industries, such as petroleum, natural gas, fuels, and fuel cells. H2S causes acid rain. In addition, it leads to corrosion in pipelines and acts as a poison for many catalysts, even at low levels, making it necessary to remove it in many industrial processes, such as fuel cells applications. Conventional treatments, including adsorption, or biological treatments present disadvantages, making the transformation to a useful product the better option. In this sense, the selective oxidation of H2S to elemental sulfur with air is the most attractive process, but it requires the design of partial oxidation catalysts facilitating oxidation to S and avoiding further oxidation to SO2. V2O5 oxide was reported as the most active catalyst in a study performed with 21 metal oxides for both the Clauss process and partial oxidation [70]. As well as in other partial oxidation processes that have already been presented, it is easier to modulate the activity with a mixed metal oxide and/or through the use of a support. López-Nieto and coworkers [71,72] proposed the use of a mesoporous zirconium phosphate as a support for VOx species, and they reported such catalysts as active and selective for the H2S transformation to S, reporting that the catalytic behavior was dependent on VOx loading. They reported that V2O5 crystals were necessary in order to have active and selective catalysts, identifying this oxide as the active phase. However, the characterization results of tested catalysts have demonstrated the formation of a partially reduced crystalline phase, V4O9-like, during the catalytic test. This was then confirmed by carrying out the catalyst characterization during the reaction using operando Raman-GC and XAS [73]. They demonstrated that the V2O5 crystalline phase was present in fresh catalysts and was transformed to V4O9 under H2S partial oxidation. Furthermore, they found that the reduced V species were related with a low selectivity to SO2. Following a similar approach, other groups investigated the use of supported catalysts, such as VOx/TiO2 [74], VOx/CeO2 [75,76], and VOx/SiO2 [77], and of vanadium oxides bronzes [78], which were the mechanism they found to be quite similar to the one already described and demonstrated by López-Nieto’s group, with the oxidation and subsequent regeneration of the vanadium active phases, from V5+ to V4+ under reaction conditions.

4. Removal of N-Containing Organic Pollutants

Total oxidation of organic compounds is a major topic; however, there are only few studies on the removal of nitrogen-containing organic compounds (NCOCs). The design of this process is not easy, since catalysts that oxidize the organic part to CO2 without oxidizing the nitrogen component to molecular N2 rather than to NOx are challenging. Metal-based catalysts with Cu and Cr or Pt have been tested for this process, but in all cases quite a high NOx selectivity was detected [79]. Vanadium-based catalysts are widely used for selective partial oxidation processes; our group reported their use for the selective destruction of N-containing organic volatile compounds [80]. Sb–V–O catalysts were selected for such studies since they are well known as active and selective for the propane ammoxidation process [14] and, subsequently, they are able to activate nitrogen atoms [81,82], avoiding further oxidation to NOx under ammoxidation reaction conditions. Thus, the catalytic behavior of Sb–V–O-supported catalysts on the destruction of dimethyl formamide (DMF) was evaluated [80], since DMF is commonly used as industrial solvent in the production of polyurethane products and acrylic fibers. It is also used in the pharmaceutical industry, in the formulation of pesticides, and in the manufacture of synthetic leathers, fibers films, and surface coatings. Several Sb–V–O catalysts with different supports (Al2O3 and Nb2O5) and different Sb precursors were tested [80]. The activity results are shown in Figure 2 (DMF conversion vs. total Sb+V coverage) and 3 (selectivity to N-containing products vs. total Sb + V coverage). Figure 2 shows some interesting results regarding DMF conversion. Figure 2A shows the effect of coverage on alumina support, where it can be observed that bare alumina is quite active, but selective to NOx (Figure 3); when Sb and V are incorporated to the alumina, the conversion increases to near 100% and the selectivity to NOx decreases. Those catalysts in which rutile VSbO4 phase forms were able to oxidize the N-containing organic compounds, avoiding the formation of NOx. Bare niobia support exhibits, unlike alumina, a significant production of ammonia, due to its higher acidity. The addition of V and Sb on Nb2O5 support covers the acidic sites and provides redox functionality, increasing the selectivity to N2 (Figure 3).
Figure 4 shows the conversion and selectivity profiles versus temperature at high Sb + V coverage on both Al2O3 and Nb2O5. Above 400 °C, the selectivity to N2 decreases at the expense of the formation of NOx. In addition, the selectivity to CO decreases with temperature, in this case at the expense of CO2 formation. The catalysts with high coverage afford promising results; selectivities to NOx and organics are low (at moderate temperatures), and the system could be used with a CO to CO2 converter in a second bed. The presence of a rutile VSbO4 active phase eliminates the overoxidation to NOx and appears to be responsible for better selectivity on the alumina series. During the catalytic cycle, the surface V5+ species undergo reduction and they become stabilized as V3+/V4+ in the VSbO4 structure [83,84]. The better selectivity to N-containing products was subsequently related to the presence of VSbO4.

5. Total Oxidation Process

VOCs (Volatile Organic Compounds) are recognized as hazardous molecules that contribute to photochemical smog and are toxic, since some of them may cause cancer and other diseases. They present a high vapor pressure and low water solubility and can be found in the air both indoors (due to furniture, cleaners, pesticides, air fresheners, cosmetics, tobacco smoke, adhesives, flooring, carpets, varnishes, paint strippers, sealants, etc.) and outdoors (oil and gas extraction and processing, wood/coal combustion, diesel and gasoline emissions, etc.). The nature of these molecules depends on the source, including alkanes, alcohols, ketones, aldehydes, aromatics, paraffins, olefins, and halogenated hydrocarbons. Among the most common and toxic not halogenated compounds are phenol, acetone, formaldehyde, benzene, propylene, toluene, and styrene. There are a few techniques available to reduce VOC emission when they are highly diluted, catalytic complete or “deep” oxidation being one of the most suitable techniques [85]. Thermal incineration (noncatalytic) requires higher temperatures, with the corresponding emissions of undesirable products, such as NOx and dioxins, and it is a quite high-energy-demanding process. Thus, there are many studies that have focused on the best catalytic formulation for the VOCs’ catalytic total oxidation, which is not an easy task, due to the large variety of organic molecules present in VOC mixtures. Both noble metals and transition metal oxides have been reported as promising catalysts. Noble-metal-based catalysts [86], especially Pt and Pd, present very good activity performances, but they are quite expensive materials and can be deactivated by sintering or poisoning. Due to that, transition and rare earth metal oxide catalysts have been explored. Although V-based catalysts possess redox active sites, vanadium is not commonly used in these formulations; other transition metals, such as copper oxide, manganese dioxide, iron oxide, nickel oxide, chromium oxide, and cobalt oxide, are used instead [87].
V–W–O-supported catalysts, used for the SCR process as has been discussed, have also been studied for VOC oxidation [88] and have been reported as active for the abatement of several polychlorinated VOCs, showing that this catalytic system was useful for the combined reduction of NOx and decomposition of these halogenated (dioxins), even in the presence of sulfur dioxide [89]. This is an important issue in this case, since SO2 is usually present with VOC pollutants and it is well known that it is able to poison noble-metal-based catalysts. However, at low temperatures (150 °C), polychlorinated molecules remain adsorbed on the catalysts without being oxidized [88]. Similar results were reported over VOx/TiO2 catalysts [90,91]. The total oxidation of nonchlorinated VOCs over vanadium-supported catalysts have also been studied by Debecker and coworkers [92], who reported very promising results where oligomeric polyvanadates would be the active site. This group also reported [93] the promoting effect of W and Mo on VOx/TiO2 catalysts for the total oxidation reaction for both halogenated and nonhalogenated molecules, obtaining similar results to those already exposed for the SCR process. They attributed this synergy between V and Mo/W oxides to the additional Brønsted acid sites brought by these promoters, since such acid sites would favor the adsorption of the VOC molecule.

6. Photocatalysis

Photocatalysts use the energy of impinging photons and may carry out a wide variety of important chemical reactions, such as (i) environmental remediation, (ii) the destruction of organic pollutants for water or air purification, (iii) solar fuels production, (iv) production of fuels, (v) and H2 from water or methane/methanol from CO2, among other applications. TiO2 [94] is commonly used as a photocatalyst since it is an available and safe semiconductor, which is stable in solution; only 5% of the incident Sun radiation can be used by TiO2, due to its bandwidth (3.2 nm eV = 390 nm). Subsequently, other photocatalytic systems, including the use of doped TiO2, in order to modify the bandwidth, have been extensively studied during the last few decades. Doping TiO2 with transition metal ions, such as V, has been one of the most important approaches [95,96,97,98]; however, this increases carrier-recombination centers, decreasing the quantum efficiency of doped TiO2 photocatalytic materials [95,96]. Another approach is doping with nonmetals, such as N [99]. Gu et al. [100] investigated the effect of doping TiO2 nanocrystal catalysts with vanadium and nitrogen, reporting an enhanced photocatalytic activity for the co-doped catalytic materials compared to V-doped TiO2 and N-doped TiO2. Here [100], a co-doped TiO2 nanocrystal had a narrower band gap (2.76 eV) than mono-doped TiO2 (2.91 eV for V–TiO2 and 2.92 eV for N–TiO2). They demonstrated that the existence of V ions in the lattice facilitates the incorporation of N atoms into the anatase lattice, enhancing absorption in the visible light region and quantum efficiency.
Bismuth vanadate, BiVO4, has also been extensively studied, since it is a semiconductor material with some properties that make it an attractive photocatalyst, such as low toxicity, low production cost, resistance to corrosion, high photostability, and narrow band gap (≈2.4 eV) with a good response to visible light. Recently, the synthesis methods and properties of these materials have been reviewed by Madhavan and coworkers [101], who showed how the photocatalytic efficiency of these materials could be improved by the control of the morphology and composition during synthesis. Nanostructured VO2 dioxide is also a semiconductor material that, with the appropriate synthesis procedure, can have a band gap of ≈2.7 eV and that shows a promising photocatalytic activity for hydrogen production [102].

7. Conclusions

This review underlines the possibilities of vanadium compounds in redox catalysis, which stand on the possibility of vanadium oxides to have different oxidation states during reaction. Additives that foster phases with reduced vanadium sites during reaction enhance redox cycles, facilitating changes in oxidation states. These cycles also modify the capability of the catalysts to absorb/desorb reactants and other intermediates. Vanadium-based materials are very promising catalysts in partial oxidation reactions, which are useful for industrial chemical processes (petroleumchemistry), as well as for environmental applications.

Funding

This work was funded by Plan Propio de Investigación (Universidad de Málaga).

Acknowledgments

M.A. Bañares (ICP CSIC) for revising the manuscript and his helpful discussions.

Conflicts of Interest

The author declares no conflict of interest.

References

  1. Mars, P.; van Krevelen, D.W. Oxidations Carried Out by Means of Vanadium Oxide Catalysts. Spec. Suppl. Chem. Eng. Sci. 1954, 3, 41–59. [Google Scholar] [CrossRef]
  2. Doornkamp, C.; Ponec, V. The universal character of the Mars and Van Krevelen mechanism. J. Mol. Catal. A Chem. 2000, 162, 19–32. [Google Scholar] [CrossRef]
  3. Haber, J. Fifty years of my romance with vanadium oxide catalysts. Catal. Today 2009, 142, 100–113. [Google Scholar] [CrossRef]
  4. Guerrero-Pérez, M.O. Supported, Bulk and bulk-supported vanadium oxide Catalysts: A short review with an historical perspective. Catal. Today 2017, 285, 226–233. [Google Scholar] [CrossRef]
  5. Guliants, V.V.; Benziger, J.B.; Sundaresan, S.; Wachs, I.E.; Jehng, J.-M.; Roberts, J.E. The effect of phase composition of model VPO catalysts for partial oxidation of n-butane. Catal. Today 1996, 28, 275–295. [Google Scholar] [CrossRef]
  6. Centi, G. Vanadyl Pyrophosphate—A critical overview. Catal. Today 1993, 16, 5–26. [Google Scholar] [CrossRef]
  7. Hutchings, G.J. Effect of promoters and reactant concentration on the selective oxidation of n-butane to maleic anhydride using vanadium phosphorus oxide catalysts. Appl. Catal. 1991, 72, 1–32. [Google Scholar] [CrossRef]
  8. Carreon, M.A.; Guliants, V.V.; Guerrero-Perez, M.O.; Bañares, M.A. Phase transformations in mesostructured VPO/surfactant composites. Microporous Mesoporous Mater. 2004, 71, 57–63. [Google Scholar] [CrossRef]
  9. Berenguer, R.; Fornells, J.; García-Mateos, F.J.; Guerrero-Perez, M.O.; Rodriguez-Mirasol, J.; Cordero, T. Novel Synthesis Mehod of porous VPO Catalysts with fibrous structure by electrospinning. Catal. Today 2016, 277, 266–273. [Google Scholar] [CrossRef]
  10. Nilsson, R.; Lindblad, T.; Andersson, A. Ammoxidation of Propane over Antimony Vanadium-Oxide Catalysts. J. Catal. 1994, 148, 501–513. [Google Scholar] [CrossRef]
  11. Centi, G.; Perathoner, S.; Trifiro, F. V Sb-oxide catalysts for the ammoxidation of propane. Appl. Catal. A Gen. 1997, 157, 143–172. [Google Scholar] [CrossRef]
  12. Catani, R.; Centi, G.; Trifiro, F.; Grasselli, R.K. Kinetics and reaction network in propane ammoxidation to acrylonitrile over vanadium-antimony-aluminum based mixed oxides. Ind. Eng. Chem. Res. 1992, 31, 107–119. [Google Scholar] [CrossRef]
  13. Guerrero-Pérez, M.O.; Bañares, M.A. Operando Raman study of alumina-supported Sb-V-O catalyst during propane ammoxidation to acrylonitrile with on line activity measurement. Chem. Commun. 2002, 12, 1292–1293. [Google Scholar] [CrossRef]
  14. Guerrero-Pérez, M.O.; Fierro, J.L.G.; Vicente, M.A.; Bañares, M.A. Effect of Sb/V ratio and of Sb+V coverage on the molecular structure and activity of alumina-supported Sb-V-O catalysts for the ammoxidation of propane to acrylonitrile. J. Catal. 2002, 206, 339–348. [Google Scholar] [CrossRef]
  15. García-González, E.; López-Nieto, J.M.; Botella, P.; González-Calbet, J.M. On the nature and structure of a new MoVTeO crystalline phase. Chem. Mater. 2002, 14, 4416–4421. [Google Scholar] [CrossRef]
  16. Vitry, D.; Dubois, J.-L.; Ueda, W. Strategy in achieving propane selective oxidation over multi-functional Mo-based oxide catalysts. J. Mol. Catal. A Chem. 2004, 220, 67–76. [Google Scholar] [CrossRef]
  17. Guliants, V.V.; Bhandari, R.; Al-Saeedi, J.N.; Vasudevan, V.K.; Soman, R.S.; Guerrero-Pérez, O.; Bañares, M.A. Bulk mixed Mo-V-Te-O Catalysts for propane oxidation to acrylic acid. Appl. Catal. A Gen. 2004, 274, 123–132. [Google Scholar] [CrossRef]
  18. Vitry, D.; Morikawa, V.; Dubois, J.L.; Ueda, W. Mo-V-Te-(Nb)-O mixed metal oxides prepared by hydrothermal synthesis for catalytic selective oxidations of propane and propene to acrylic acid. Appl. Catal. A Gen. 2003, 251, 411–424. [Google Scholar] [CrossRef]
  19. López-Medina, R.; Fierro, J.L.G.; Guerrero-Pérez, M.O.; Bañares, M.A. Structural changes occurring at the surface of alumina-supported nanoscaled Mo–V–Nb–(Te)–O catalytic system during the selective oxidation of propane to acrylic acid. Appl. Catal. A Gen. 2011, 406, 34–42. [Google Scholar] [CrossRef]
  20. López-Medina, R.; Sobczak, I.; Golinska-Mazwa, H.; Ziolek, M.; Bañares, M.A.; Guerrero-Pérez, M.O. Spectroscopic surface characterization of MoVNbTe nanostructured catalysts for the partial oxidation of propane. Catal. Today 2012, 187, 195–200. [Google Scholar] [CrossRef]
  21. Efendiev, A.D.; Tretyakov, V.F.; Rozovskii, A.Y.; Shakhtakhtinskii, T.N. Modifying action of wáter on vanadium-phosphoric catalyst. Kinet. Catal. 1990, 31, 446–447. [Google Scholar]
  22. Rapolu, C.S.R.; Panja, K.R. Highly selective V-P-O/Al2O3 catalysts in the ammoxidation of toluene to benzonitrile. J. Chem. Soc. Chem. Commun. 1993, 14, 1175–1176. [Google Scholar] [CrossRef]
  23. Centi, G. Nature of active layer in vanadium oxide supported on titanium oxide and control of its reactivity in the selective oxidation and ammoxidation of alkylaromatics. Appl. Catal. A Gen. 1996, 147, 267–298. [Google Scholar] [CrossRef]
  24. Parmaliana, A.; Frusteri, F.; Mezzapica, A.; Scurrell, M.S.; Giordano, N. Novel high activity catalyst for partial oxidation of Methane to formaldehyde. J. Chem. Soc. Chem. Commun. 1993, 9, 751–753. [Google Scholar] [CrossRef]
  25. Kao, C.-Y.; Huang, K.-T.; Wan, B.-Z. Ethane Oxydehydrogenation over Supported Vanadium Oxides. Ind. Eng. Chem. Res. 1994, 33, 2066–2072. [Google Scholar] [CrossRef]
  26. Chieregato, A.; López Nieto, J.M.; Cavani, F. Mixed-oxide Catalysts with vanadium as the key element for gas-phase reactions. Coord. Chem. Rev. 2015, 301–302, 3–23. [Google Scholar] [CrossRef]
  27. Carrero, C.A.; Schloegl, R.; Wachs, I.E.; Schomaecker, R. Critical literature review of the kinetics for the oxidative dehydrogenation of propane over well-defined supported vanadium oxide catalysts. ACS Catal. 2014, 4, 3357–3380. [Google Scholar] [CrossRef]
  28. Wachs, I.E. Catalysis science of supported vanadium oxide Catalysts. Dalton Trans. 2013, 42, 11762–11769. [Google Scholar] [CrossRef] [PubMed]
  29. Kim, H.; Ferguson, G.A.; Cheng, L.; Zygmunt, S.A.; Stair, P.C.; Curtiss, L.A. Structure-specific reactivity of alumina-supported monomeric vanadium oxide species. J. Phys. Chem. C 2012, 116, 2927–2932. [Google Scholar] [CrossRef]
  30. Fornés, V.; López, C.; López, H.H.; Martínez, A. Catalytic performance of mesoporous VOx/SBA-15 catalysts for the partial oxidation of Methane to formaldehyde. Appl. Catal. A Gen. 2003, 249, 345–354. [Google Scholar] [CrossRef]
  31. Beale, A.M.; Gao, F.; Lezcano-Gonzalez, I.; Peden, C.H.F.; Szanyi, J. Recent advances in automotive Catalysis for NOx emission control by small-pore microporous materials. Chem. Soc. Rev. 2015, 44, 7371–7405. [Google Scholar] [CrossRef] [PubMed]
  32. Shangguan, W.F.; Teraoka, Y.; Kagawa, S. Promotion effect of potassium on the catalytic property of CuFe2O4 for the simultaneous removal of NO(x) and diesel soot particulate. Appl. Catal. B 1998, 16, 149–154. [Google Scholar] [CrossRef]
  33. Fickel, D.W.; D’Addio, E.; Lauterbach, J.A.; Lobo, R.F. The ammonia selective catalytic reduction activity of copper-exchanged small-pore zeolites. Appl. Catal. B 2011, 102, 441–448. [Google Scholar] [CrossRef]
  34. Qi, G.; Yang, R.T.; Chang, R. MnOx-CeO2 mixed oxides prepared by co-precipitation for selective catalytic reduction of NO with NH3 at low temperatures. Appl. Catal. B 2004, 51, 93–106. [Google Scholar] [CrossRef]
  35. Kapteijn, F.; Singoredjo LAndreini, A.; Moulijn, J.A. Activity and selectivity of pure manganese oxides in the selective catalytic reduction of nitric oxide with ammonia. Appl. Catal. B 1994, 3, 173–189. [Google Scholar] [CrossRef]
  36. Xu, J.; Chen, G.; Guo, F.; Xie, J. Development of wide-temperature vanadium-based catalysts for selective catalytic reducing of NOx with ammonia: Review. Chem. Eng. J. 2018, 353, 507–518. [Google Scholar] [CrossRef]
  37. Casagrande, L.; Lietti, L.; Nova, I.; Forzatti, P.; Baiker, A. SCR of NO by NH3 over TiO2-supported V2O5-MoO3 catalysts: Reactivity and redox behavior. Appl. Catal. B 1999, 22, 63–77. [Google Scholar] [CrossRef]
  38. Zhao, Z.; Gao, X.; Wachs, I.E. Comparative Study of Bulk and Supported V−Mo−Te−Nb−O Mixed Metal Oxide Catalysts for Oxidative Dehydrogenation of Propane to Propylene. J. Phys. Chem. B 2003, 107, 6333–6342. [Google Scholar] [CrossRef]
  39. Yang, S.; Iglesia, E.; Bell, A.T. Oxidative Dehydrogenation of Propane over V2O5/MoO3/Al2O3 and V2O5/Cr2O3/Al2O3: Structural Characterization and Catalytic Function. J. Phys. Chem. B 2005, 109, 8987–9000. [Google Scholar] [CrossRef] [PubMed]
  40. Bañares, M.A.; Khatib, S.J. Structure–activity relationships in alumina-supported molybdena–vanadia catalysts for propane oxidative dehydrogenation. Catal. Today 2004, 96, 251–257. [Google Scholar] [CrossRef]
  41. Guerrero-Pérez, M.O.; Al-Saeedi, J.N.; Guliants, V.V.; Bañares, M.A. Catalytic properties of mixed Mo-V-Sb-Nb-O oxides catalysts for the ammoxidation of propane to acrylonitrile. Appl. Catal. A 2004, 260, 93–99. [Google Scholar] [CrossRef]
  42. Watanabe, H.; Koyasu, Y. New synthesis route for Mo–V–Nb–Te mixed oxides catalyst for propane ammoxidation. Appl. Catal. A 2000, 194–195, 479–485. [Google Scholar] [CrossRef]
  43. Vaarkamp, M.; Ushikubo, T. Limitations of V–Sb–W and Mo–V–Nb–Te mixed oxides in catalyzing propane ammoxidation. Appl. Catal A 1998, 174, 99–107. [Google Scholar] [CrossRef]
  44. Ueda, W.; Vitry, D.; Katou, T. Structural organization of catalytic functions in Mo-based oxides for propane selective oxidation. Catal. Today 2004, 96, 235–240. [Google Scholar] [CrossRef]
  45. Al-Saeedi, J.N.; Guliants, V.V.; Guerrero-Pérez, M.O.; Bañares, M.A. Bulk structure and catalytic properties of mixed Mo–V–Sb–Nb oxides for selective propane oxidation to acrylic acid. J. Catal. 2003, 215, 108–115. [Google Scholar] [CrossRef]
  46. Guerrero-Pérez, M.O.; Alemany, L.J. Alumina-supported Mo-V-Te-O Catalysts for the ammoxidation of propane to acrylonitrile. Appl. Catal. A 2008, 341, 119–126. [Google Scholar] [CrossRef]
  47. Lietti, L.; Forzatti, P.; Bregani, F. Steady-state and transient reactivity study of TiO2-supported V2O5-WO3 De-NOx catalysts: Relevance of the vanadium-tungsten interaction on the catalytic activity. Ind. Eng. Chem. Res. 1996, 35, 3884–3892. [Google Scholar] [CrossRef]
  48. Chen, J.P.; Yang, R.T. Role of WO3 in mixed V2O5-WO3/TiO2 catalysts for selective catalytic reduction of nitric oxide with ammonia. Appl. Catal. A 1992, 80, 135–148. [Google Scholar] [CrossRef]
  49. Zhang, S.; Zhong, Q. Surface characterization studies on the interaction of V2O5-WO3/TiO2 catalyst for low temperature SCR of NO with NH3. J. Sol. Sta. Chem. 2015, 221, 49–56. [Google Scholar] [CrossRef]
  50. Zhang, S.; Zhong, Q. Promotional effect of WO3 on O2- over V2O5/TiO2 catalyst for selective catalytic reduction of NO with NH3. J. Mol. Catal. A 2013, 373, 108–113. [Google Scholar] [CrossRef]
  51. Nova, I.; Ciardelli, C.; Tronconi, E.; Chatterjee, D.; Bandl-Konrad, B. NH2-NO/NO2 chemistry over V-based Catalysts and its role in the mechanism of the Fast SCR reaction. Catal. Today 2006, 114, 3–12. [Google Scholar] [CrossRef]
  52. Tronconi, E.; Nova ICiardelli, C.; Chatterjee, D.; Weibel, M. Redox features in the catalytic mechanism of the “standard” and “fast” NH3-SCR of NOx over a V-based catalyst investigated by dynamic methods. J. Catal. 2007, 245, 1–10. [Google Scholar] [CrossRef]
  53. Koebel, M.; Madia, G.; Raimondi, F.; Wokaun, A. Enhanced reoxidation of vanadia by NO2 in the fast SCR reaction. J. Catal. 2002, 209, 159–165. [Google Scholar] [CrossRef]
  54. Amiridis, M.D.; Duevel, R.V.; Wachs, I.E. The effect of metal oxide additives on the activity of V2O5/TiO2 catalysts for the selective catalytic reduction of nitric oxide by ammonia. Appl. Catal. B 1999, 20, 111–122. [Google Scholar] [CrossRef]
  55. Guerrero-Pérez, M.O.; Bañares, M.A. Operando Raman–GC studies of alumina-supported Sb-V-O catalysts and role of the preparation method. Catal. Today 2004, 96, 265–272. [Google Scholar] [CrossRef]
  56. Lietti, L.; Forzatti, P.; Ramis, G.; Busca, G.; Bregani, F. Potassium doping of vanadia/titania de-NOxing catalysts: Surface characterization and reactivity study. Appl. Catal. B 1993, 3, 13–35. [Google Scholar] [CrossRef]
  57. Chen, L.; Li, J.; Ge, M. The poisoning effect of alkali metals doping over nano V2O5-WO3/TiO2 catalysts on selective catalytic reduction of NOx by NH3. Chem. Eng. J. 2011, 170, 531–537. [Google Scholar] [CrossRef]
  58. Kong, M.; Liu, Q.; Zhou, J.; Jiang, L.; Tian, Y.; Yang, J.; Ren, S. Effect of different potassium species on the deactivation of V2O5-WO3/TiO2 SCR catalyst: Comparison of K2SO4, KCl and K2O. Chem. Eng. J. 2018, 348, 637–643. [Google Scholar] [CrossRef]
  59. Guerrero-Pérez, M.O.; Rosas, J.M.; López-Medina, R.; Bañares, M.A.; Rodríguez-Mirasol, J.; Cordero, T. On the Nature of Surface Vanadium Oxide Species on Carbons. J. Phys. Chem. C 2012, 116, 20396–20403. [Google Scholar] [CrossRef]
  60. Zhu, Z.; Liu, Z.; Liu, S.; Niu, H. A novel carbon-supported vanadium oxide catalyst for NO reduction with NH3 at low temperatures. Appl. Catal. B 1999, 23, L229–L233. [Google Scholar] [CrossRef]
  61. García-Bordejé, E.; Calvillo, L.; Lázaro, M.J.; Moliner, R. Vanadium supported on carbon-coated monoliths for the SCR of NO at low temperature: Effect of pore structure. Appl. Catal. B 2004, 50, 235–242. [Google Scholar] [CrossRef]
  62. García-Bordejé, E.; Calvillo, L.; Lázaro, M.J.; Moliner, R. Study of configuration and coating thickness of vanadium on carbon-coated monoliths in the SCR of NO at low temperature. Ind. Eng. Chem. Res. 2004, 43, 4073–4079. [Google Scholar] [CrossRef]
  63. García-Bordejé, E.; Monzón, A.; Lázaro, M.J.; Moliner, R. Promotion by a second metal or SO2 over vanadium supported on mesoporous carbon-coated monoliths for the SCR of NO at low temperature. Catal. Today 2005, 102–103, 177–182. [Google Scholar]
  64. García-Bordejé, E.; Lázaro, M.J.; Moliner, R.; Galindo, J.F.; Sotres, J.; Baró, A.M. Structure of vanadium oxide supported on mesoporous carbon-coated monoliths and relationship with its catalytic performance in the SCR of NO at low temperatures. J. Catal. 2004, 223, 395–403. [Google Scholar] [CrossRef]
  65. García-Bordejé, E.; Pinilla, J.L.; Lázaro, M.J.; Moliner, R.; Fierro, J.L.G. Role of sulphates on the mechanism of NH3-SCR of NO at low temperatures over presulphated vanadium supported on carbon-coated monoliths. J. Catal. 2005, 233, 166–175. [Google Scholar] [CrossRef]
  66. García-Bordejé, E.; Pinilla, J.L.; Lázaro, M.J.; Moliner, R. NH3-SCR of NO at low temperatures over sulphated vanadia on carbon-coated monoliths: Effect of H2O and SO2 traces in the gas feed. Appl. Catal. B 2006, 66, 281–287. [Google Scholar] [CrossRef]
  67. Chen, L.; Li, J.; Ge, M. Promotional effect of ce-doped V2O5-WO3/TiO2 with low vanadium loadings for selective catalytic reduction of NOx by NH3. J. Phys. Chem. C 2009, 113, 21177–21184. [Google Scholar] [CrossRef]
  68. Guan, B.; Lin, H.; Zhu, L.; Huang, Z. Selective catalytic reduction of NOx with NH3 over Mn, Ce Substitution Ti0.9V0.1O2-δ nanocomposites catalysts prepared by self-propagating high-temperature synthesis method. J. Phys. Chem. C 2011, 115, 12850–12863. [Google Scholar] [CrossRef]
  69. Liu, Z.; Zhang, S.; Li, J.; Zhu, J.; Ma, L. Novel V2O5-CeO2/TiO2 catalyst with low vanadium loading for the selective catalytic reduction of NOx by NH3. Appl. Catal. B 2014, 158–159, 11–19. [Google Scholar] [CrossRef]
  70. Davydov, A.A.; Marshneva, V.I.; Shepotko, M.L. Metal oxides in hydrogen sulfide oxidation by oxygen and sulfur dioxide I. The comparison study of the catalytic activity. Mechanism of the interactions between H2S and SO2 on some oxides. Appl. Catal. A 2003, 244, 93–100. [Google Scholar] [CrossRef]
  71. Soriano, M.D.; Jiménez-Jiménez, J.; Concepción, P.; Jiménez-López, A.; Rodríguez-Castellón, E.; Nieto, J.M.L. Selective oxidation of H2S to sulfuro ver vanadia supported on mesoporous zirconium phosphate heterostructure. Appl. Catal. B 2009, 92, 271–279. [Google Scholar] [CrossRef]
  72. León, M.; Jiménez-Jiménez, J.; Jiménez-López, A.; Rodríguez-Castellón, E.; Soriano, D.; Nieto, J.M.L. Vanadium oxide-porous phosphate heterostructure Catalysts for the selective oxidation of H2S to sulphur. Solid State Sci. 2010, 12, 996–1001. [Google Scholar] [CrossRef]
  73. Holgado, J.P.; Soriano, M.D.; Jiménez-Jiménez, J.; Concepción, P.; Jiménez-López, A.; Caballero, A.; Rodríguez-Castellón, E.; Nieto, J.M.L. Operando XAS and Raman study on the structure of a supported vanadium oxide catalyst during the oxidation of H2S to sulphur. Catal. Today 2010, 155, 296–301. [Google Scholar] [CrossRef]
  74. Pongthawornsakun, B.; Phatyenchuen, S.; Panpranot, J.; Praserthdam, P. The low temperature selective oxidation of H2S to elemental sulfur on TiO2 supported V2O5 catalysts. J. Environ. Chem. Eng. 2018, 6, 1414–1423. [Google Scholar] [CrossRef]
  75. Palma, V.; Barba, D.; Ciambelli, P. H2S removal in biogas by direct catalytic oxidation to sulphur on V2O5/CeO2 catalysts. Chem. Eng. Trans. 2012, 29, 631–636. [Google Scholar]
  76. Palma, V.; Barba, D. Low temperature catalytic oxidation of H2S over V2O5/CeO2 catalysts. Int. J. Hydrogen Energy 2014, 39, 21524–21530. [Google Scholar] [CrossRef]
  77. Cecilia, J.A.; Soriano, M.D.; Natoli, A.; Rodríguez-Castellón, E.; López Nieto, J.M. Selective oxidation of hydrogen sulfide to sulfur using vanadium oxide supported on porous clay heterostructures (PCHs) formed by pillars silica, silica-zirconia or silica-titania. Materials 2018, 11, 1562. [Google Scholar] [CrossRef] [PubMed]
  78. Soriano, M.D.; Vidal-Moya, A.; Rodríguez-Castellón, E.; Melo, F.V.; Blasco, M.T.; Nieto, J.M.L. Partial oxidation of hydrogen sulfide to sulfur over vanadium oxides bronzes. Catal. Today 2016, 259, 237–244. [Google Scholar] [CrossRef] [Green Version]
  79. Haber, J.; Janas, J.; Krysciak-Czerwenka, J.; Machej, T.; Sadowska, H.; Hellden, S. Total oxidation of nitrogen-containing organic compounds to N2, CO2 and H2O. Appl. Catal. A 2002, 229, 23–34. [Google Scholar] [CrossRef]
  80. Guerrero-Pérez, M.O.; Janas, J.; Machej, T.; Haber, J.; Lewandowska, A.E.; Fierro, J.L.G.; Bañares, M.A. Selective destruction of nitrogen-contaning organic volatile compounds over Sb-V-O catalysts. Appl. Catal. B 2007, 71, 85–93. [Google Scholar] [CrossRef]
  81. Guerrero-Pérez, M.O.; Peña, M.A.; Fierro, J.L.G.; Bañares, M.A. A study about the propane ammoxidation to acrylonitrile with an alumina-supported Sb-V-O catalyst. Ind. End. Chem. Res. 2006, 45, 4537–4543. [Google Scholar] [CrossRef]
  82. Rojas, E.; Calatayud MGuerrero-Pérez, M.O.; Bañares, M.A. Correlation between Theoretical and Experimental Investigations of the Ammonia Adsorption Process on the (110)-VSbO4 Surface. Catal. Today 2010, 158, 178–185. [Google Scholar] [CrossRef]
  83. Guerrero-Pérez, M.O.; Bañares, M.A. Operando Raman-GC study of supported alumina Sb and V based Catalysts: Effect of Sb/V molar ratio and total Sb+V coverage in the structure of catalysts during propane ammoxidation. J. Phys. Chem. C 2007, 111, 1315–1322. [Google Scholar] [CrossRef]
  84. Guerrero-Pérez, M.O.; Kim, T.; Bañares, M.A.; Wachs, I.E. The Nature of Catalytic Active Sites for Sb-V-O mixed Metal Oxides. J. Phys. Chem. C 2008, 112, 16858–16863. [Google Scholar] [CrossRef]
  85. Spivey, J.J. Complete Catalytic Oxidation of Volatile Organics. Ind. Eng. Chem. Res. 1987, 26, 2165–2180. [Google Scholar] [CrossRef]
  86. Liotta, L. Catalytic oxidation of volatile organic compounds on supported noble metals. Appl. Catal. B 2010, 100, 403–412. [Google Scholar] [CrossRef]
  87. Shahzad Kamal, M.; Razzak, S.A.; Hossain, M.M. Catalytic oxidation of volatile organic compounds (VOCs)—A review. Atmos. Environ. 2016, 140, 117–134. [Google Scholar] [CrossRef]
  88. Weber, R.; Sakurai, T.; Hagenmaier, H. Low temperature decomposition of PCDD/PCDF, chlorobenzenes and PAHs by TiO2-based V2O5-WO3 catalysts. Appl. Catal. B 1999, 20, 249–256. [Google Scholar] [CrossRef]
  89. Jones, J.; Ross, J.R. The development of supported vanadia catalysts for the combined catalytic removal of the oxides of nitrogen and of chlorinated hydrocarbons from flue gases. Catal. Today 1997, 35, 97–105. [Google Scholar] [CrossRef]
  90. Krishnamoorthy, S.; Baker, J.P.; Amiridis, M.D. Catalytic oxidation of 1,2-dichlorobenzene over V2O5/TiO2-based catalysts. Catal. Today 1998, 40, 39–46. [Google Scholar] [CrossRef]
  91. Delaible, R.; Debecker, D.P.; Bertinchamps, F.; Gaigneaux, E.M. Revisiting the behaviour of vanadia-based catalysts in the abatement of (chloro)-aromatic pollutants: Towards an integrated understanding. Top. Catal. 2009, 52, 501–516. [Google Scholar] [CrossRef]
  92. Debecker, D.P.; Bouchmella, K.; Delaible, R.; Eloy, P.; Poleunis, C.; Bertrand, P.; Gaigneaux, E.M.; Mutin, P.H. One-step non-hydrolytic sol–gel preparation of efficient V2O5-TiO2 catalysts for VOC total oxidation. Appl. Catal. B 2010, 94, 38–45. [Google Scholar] [CrossRef]
  93. Debecker, D.P.; Delaigle, R.; Bouchmella, K.; Eloy PGaigneaux, E.M.; Mutin, P.H. Total oxidation of benzene and chlorobenzene with MoO3- and WO3-promoted V2O5/TiO2 catalysts prepared by a nonhydrolytic sol–gel route. Catal. Today 2010, 157, 125–130. [Google Scholar] [CrossRef]
  94. Linsebigler, A.L.; Guangquan, L.; Yates, J.T. Photocatalysis on TiO2 Surfaces: Principles, Mechanisms, and Selected Results. Chem. Rev. 1995, 95, 735–758. [Google Scholar] [CrossRef]
  95. Yu, J.C.; Raymund, J.L.; Kwok, W.M. Enhanced photocatalytic activity of Ti1-xVxO2 solid solution on the degradation of acetone. J. Phot. Phot. A 1997, 111, 199–203. [Google Scholar] [CrossRef]
  96. Yamashita, H.; Harada, M.; Misaka, J.; Takeuchi, M.; Ikeue, K.; Anpo, M. Degradation of propanol diluted in wáter under visible light irradiation using metal ion-implanted titanium dioxide photocatalysts. J. Photochem. Photobiol. A Chem. 2002, 148, 257–261. [Google Scholar] [CrossRef]
  97. Wu, J.C.S.; Chen, C.H. A visible-light response vanadium-doped titania nanocatalyst by sol-gel method. J. Photochem. Photobiol. A Chem. 2004, 163, 509–515. [Google Scholar] [CrossRef]
  98. Tian, B.; Li, C.; Gu, F.; Jiang, H.; Hu, Y.; Zhang, J. Flame sprayed V-doped TiO2 nanoparticles with enhanced photocatalytic activity under visible light irradiation. Chem. Eng. J. 2009, 151, 220–227. [Google Scholar] [CrossRef]
  99. Burda, C.; Lou, Y.; Chen, X.; Samia, A.C.S.; Stout, J.; Gole, J.L. Enhanced nitrogen doping in TiO2 nanoparticles. Nano Lett. 2003, 3, 1049–1051. [Google Scholar] [CrossRef]
  100. Gu, D.-E.; Yang, B.-C.; Hu, Y.-D. V and N co-doped nanocrystal anatase TiO2 photocatalysts with enhanced photocatalytic activity under visible light irradiation. Catal. Commun. 2008, 9, 1472–1476. [Google Scholar] [CrossRef]
  101. Malathi, A.; Madhavan, J.; Ashokkumar, M.; Arunachalam, P. A review on BiVO4 photocatalyst: Activity enhancement methods for solar photocatalytic applications. Appl. Catal. A 2018, 555, 47–74. [Google Scholar]
  102. Wang, Y.; Zhang, Z.; Zhu, Y.; Li, Z.; Vajtai, R.; Ci, L.; Ajayan, P.M. Nanostructured VO2 photocatalysts for hydrogen production. ACS Nano 2008, 2, 1492–1496. [Google Scholar] [CrossRef] [PubMed]
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Figure 1. (A) Number of articles published by year during the last 10 years with “vanadium oxide catalysts” (black bars) and, among these, those that have “environmental” (grey bars). The lines indicate the % that grey bars represent with respect to the black ones. Note: Words in title, abstract, or keywords according to Scopus. (B) Number of articles published by year during the last 10 years with “vanadium oxide catalysts” (black bars) and, among these, those devoted to total oxidation (red), photocatalysis (green), and SCR (selective catalytic reduction) (blue).
Figure 1. (A) Number of articles published by year during the last 10 years with “vanadium oxide catalysts” (black bars) and, among these, those that have “environmental” (grey bars). The lines indicate the % that grey bars represent with respect to the black ones. Note: Words in title, abstract, or keywords according to Scopus. (B) Number of articles published by year during the last 10 years with “vanadium oxide catalysts” (black bars) and, among these, those devoted to total oxidation (red), photocatalysis (green), and SCR (selective catalytic reduction) (blue).
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Figure 2. Dimethyl formamide (DMF) conversion values vs. total Sb + V coverage for: (A) Al2O3 and (B) Nb2O5-supported catalysts. Reaction conditions: 1 mL of catalyst; GHSV = 10,000 h−1; 1000 ppm of DMF; temperature reaction: 250 °C. Reprinted from “Selective destruction of nitrogen-containing organic volatile compounds over Sb–V–O catalysts” Appl. Catal. B Environ. 2007, 71, 85–93 [80]. Copyright ©2006 Elsevier B.V., with permission from Elsevier 4461960513380.
Figure 2. Dimethyl formamide (DMF) conversion values vs. total Sb + V coverage for: (A) Al2O3 and (B) Nb2O5-supported catalysts. Reaction conditions: 1 mL of catalyst; GHSV = 10,000 h−1; 1000 ppm of DMF; temperature reaction: 250 °C. Reprinted from “Selective destruction of nitrogen-containing organic volatile compounds over Sb–V–O catalysts” Appl. Catal. B Environ. 2007, 71, 85–93 [80]. Copyright ©2006 Elsevier B.V., with permission from Elsevier 4461960513380.
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Figure 3. Selectivity to N-products vs. total Sb + V coverage at 400 °C for: (A) Tartaric (T) and (B) standard (ST) alumina-supported catalysts; (C) tartaric (T) and (D) standard (ST) Nb2O5-supported catalysts. Reaction conditions: 1 ml of catalyst; GHSV = 10,000 h−1; 1000 ppm of DMF. Reprinted from “Selective destruction of nitrogen-containing organic volatile compounds over Sb–V–O catalysts” Appl. Catal. B Environ. 2007, 71, 85–93. Copyright ©2006 Elsevier B.V., with permission from Elsevier 4461960513380.
Figure 3. Selectivity to N-products vs. total Sb + V coverage at 400 °C for: (A) Tartaric (T) and (B) standard (ST) alumina-supported catalysts; (C) tartaric (T) and (D) standard (ST) Nb2O5-supported catalysts. Reaction conditions: 1 ml of catalyst; GHSV = 10,000 h−1; 1000 ppm of DMF. Reprinted from “Selective destruction of nitrogen-containing organic volatile compounds over Sb–V–O catalysts” Appl. Catal. B Environ. 2007, 71, 85–93. Copyright ©2006 Elsevier B.V., with permission from Elsevier 4461960513380.
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Figure 4. DMF conversion and selectivity profiles for principal reaction products vs. temperature for: (A) 2Sb5V/Al–T; (B) 2Sb5V/Al–ST; (C) 2Sb5V/Nb–T; (D) 2Sb5V/Nb–ST. Reaction conditions: 1 ml of catalyst; GHSV = 10,000 h−1; 1000 ppm of DMF. Reprinted from “Selective destruction of nitrogen-containing organic volatile compounds over Sb–V–O catalysts” Appl. Catal. B Environ. 2007, 71, 85–93 [80]. Copyright ©2006 Elsevier B.V., with permission from Elsevier 4461960513380.
Figure 4. DMF conversion and selectivity profiles for principal reaction products vs. temperature for: (A) 2Sb5V/Al–T; (B) 2Sb5V/Al–ST; (C) 2Sb5V/Nb–T; (D) 2Sb5V/Nb–ST. Reaction conditions: 1 ml of catalyst; GHSV = 10,000 h−1; 1000 ppm of DMF. Reprinted from “Selective destruction of nitrogen-containing organic volatile compounds over Sb–V–O catalysts” Appl. Catal. B Environ. 2007, 71, 85–93 [80]. Copyright ©2006 Elsevier B.V., with permission from Elsevier 4461960513380.
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Guerrero-Pérez, M.O. V-Containing Mixed Oxide Catalysts for Reduction–Oxidation-Based Reactions with Environmental Applications: A Short Review. Catalysts 2018, 8, 564. https://doi.org/10.3390/catal8110564

AMA Style

Guerrero-Pérez MO. V-Containing Mixed Oxide Catalysts for Reduction–Oxidation-Based Reactions with Environmental Applications: A Short Review. Catalysts. 2018; 8(11):564. https://doi.org/10.3390/catal8110564

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Guerrero-Pérez, M. Olga. 2018. "V-Containing Mixed Oxide Catalysts for Reduction–Oxidation-Based Reactions with Environmental Applications: A Short Review" Catalysts 8, no. 11: 564. https://doi.org/10.3390/catal8110564

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