Vanadium pentoxide
| Vanadium(V) oxide | |
|---|---|
| |
| |
| IUPAC name | Divanadium pentaoxide |
| Other names | Vanadium pentoxide Vanadic anhydride Divanadium pentoxide |
| Identifiers | |
| InChI | InChI=1/5O.2V/rO5V2/c1-6(2)5-7(3)4 |
| InChIKey | GNTDGMZSJNCJKK-HHIHJEONAP |
| Standard InChI | InChI=1S/5O.2V |
| Standard InChIKey | GNTDGMZSJNCJKK-UHFFFAOYSA-N |
| CAS number | [] |
| EC number | |
| UN number | 2862 |
| RTECS | YW2450000 |
| ChemSpider | |
| PubChem | |
| Properties[1] | |
| Chemical formula | V2O5 |
| Molar mass | 181.88 g/mol |
| Appearance | Orange-yellow solid |
| Density | 3.357 g/cm3 |
| Melting point |
690 °C (963 K) |
| Boiling point |
1750 °C decomp. |
| Solubility in water | 0.8 g/100 mL (20 °C) |
| Structure[2] | |
| Crystal structure | Orthorhombic |
| Space group | Pmmn, No. 59 |
| Lattice constant | a = 1151 pm, b = 355.9 pm, c = 437.1 pm |
| Coordination geometry | Distorted trigonal bipyramidal (V) |
| Hazards | |
| Material safety data sheet (MSDS) | ICSC 0596 |
| EU index number | 023-001-00-8 |
| GHS pictograms |   
|
| GHS signal word | DANGER |
| GHS hazard statements | H341, H361, H372, H332, H302, H335, H411 |
| NFPA 704 |
 |
| Flash point | Non-flammable |
| LD50 | 10 mg/kg |
| Related compounds | |
| Other anions | Vanadium oxytrichloride |
| Other cations | Niobium(V) oxide Tantalum(V) oxide |
| Other vanadium oxides | Vanadium(II) oxide Vanadium(III) oxide Vanadium(IV) oxide |
| Template:Tick(what is this?) (verify) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Vanadium(V) oxide (vanadia) is the chemical compound with the formula V2O5. Commonly known as vanadium pentoxide, this orange solid is the most important compound of vanadium. Upon heating it reversibly loses oxygen. Related to this ability, V2O5 catalyses several useful aerobic oxidation reactions, the largest scale of which underpins the production of sulfuric acid from sulfur dioxide. It is a poisonous orange solid which, because of its high oxidation state, is both an amphoteric oxide and an oxidising agent. Unlike most metal oxides, it dissolves slightly in water to give a pale yellow, acidic solution.
The mineral form of this compound, shcherbinaite,[3] is extremely rare, almost always found among fumaroles. A mineral trihydrate, V2O5·3H2O, is also known under the name of navajoite.[4]
Contents
Chemical properties
Acid-base reactions
V2O5 is an amphoteric oxide. Thus it reacts with strong non-reducing acids to form solutions containing the pale yellow salts containing dioxovanadium(V) centers:
- V2O5 + 2HNO3 → 2VO2(NO3) + H2O
It also reacts with strong alkali to form polyoxovanadates, which have a complex structure that depends on pH.[5] If excess aqueous sodium hydroxide is used, the product is a colourless salt, sodium orthovanadate, Na3VO4. If acid is slowly added to a solution of Na3VO4, the colour gradually deepens through orange to red before brown hydrated V2O5 precipitates around pH 2. These solutions contain mainly the ions HVO42− and V2O74− between pH 9 and pH 13, but below pH 9 more exotic species such as V4O124− and HV10O285− predominate.
Thionyl chloride converts it to VOCl3:
- V2O5 + 3SOCl2 → 2VOCl3 + 3SO2
Redox reactions
V2O5 is easily reduced in acidic media to the stable vanadium(IV) species, the blue vanadyl ion (VO(H2O)52+). This conversion illustrates the redox properties of V2O5. For example, hydrochloric acid and hydrobromic acid are oxidised to the corresponding halogen, e.g.,
- V2O5 + 6HCl + 7H2O → 2[VO(H2O)5]2+ + 4Cl− + Cl2
Solid V2O5 is reduced by oxalic acid, carbon monoxide, and sulfur dioxide to give vanadium(IV) oxide, VO2 as a deep-blue solid. Further reduction using hydrogen or excess CO can lead to complex mixtures of oxides such as V4O7 and V5O9 before black V2O3 is reached. Vanadates or vanadyl(V) compounds in acid solution are reduced by zinc amalgam through the interestingly colorful pathway:
| VO2+ | → | VO2+ | → | V3+ | → | V2+ |
| yellow | blue | green | purple |
The ions are, of course, all hydrated to varying degrees.
Preparation
Technical grade V2O5 is produced as a black powder used for the production of vanadium metal and ferrovanadium.[5] A vanadium ore or vanadium-rich residue is treated with sodium carbonate to produce sodium metavanadate, NaVO3. This material is then acidified to pH 2–3 using H2SO4 to yield a precipitate of "red cake" (see above). The red cake is then melted at 690 °C to produce the crude V2O5.
Vanadium(V) oxide is also the main product when vanadium metal is heated with excess oxygen, but this product is contaminated with other lower oxides. A more satisfactory laboratory preparation involves the decomposition of ammonium metavanadate at around 200 °C:
- 2NH4VO3 → V2O5 + 2NH3 + H2O
Uses
Ferrovanadium production
In terms of quantity, the major use for vanadium(V) oxide is in the production of ferrovanadium (see above). The oxide is heated with scrap iron and ferrosilicon, with lime added to form a calcium silicate slag. Aluminium may also be used, producing the iron-vanadium alloy along with alumina as a by-product.[5] In 2005 a shortage of V2O5 caused a price rise to around $40/kg, which in turn caused a rise in the price of ferrovanadium.
Sulfuric acid production
Aonther important use of vanadium(V) oxide is in the manufacture of sulfuric acid, an important industrial chemical with an annual production of 165 million metric tons in 2001, with an approximate value of US$8 billion. Vanadium(V) serves the crucial purpose of catalysing the mildly exothermic oxidation of sulfur dioxide to sulfur trioxide by air in the contact process:
- 2SO2 + O2 ⇌ 2SO3
The discovery of this simple reaction, for which V2O5 is the most effective catalyst, allowed sulfuric acid to become the cheap commodity chemical it is today. The reaction is performed between 400 and 620 °C; below 400 °C the V2O5 is inactive as a catalyst, and above 620 °C it begins to break down. Since it is known that V2O5 can be reduced to VO2 by SO2, one likely catalytic cycle is as follows:
- SO2 + V2O5 → SO3 + 2VO2
followed by
- 2VO2 +½O2 → V2O5
Paradoxically, it is also used as catalyst in the selective catalytic reduction (SCR) of NOx emissions in some power plants. Due to its effectiveness in converting sulfur dioxide into sulfur trioxide, and thereby sulfuric acid, special care must be taken with the operating temperatures and placement of a power plant's SCR unit when firing sulfur-containing fuels.
Other oxidations
Maleic anhydride is another important industrial material, used for the manufacture of polyester resins and alkyd resins.[6] Vanadium(V) oxide can catalyse its production from a variety of organic starting materials such as n-butane, furfural and benzene, the last of which is the usual commercial method. In a related process, phthalic anhydride, used for making plasticisers for PVC manufacture, may be produced by V2O5 catalysed oxidation of ortho-xylene or naphthalene at 350–400 °C.
Other applications
Due to its high thermal coefficient of resistance, vanadium(V) oxide finds use as a detector material in bolometers and microbolometer arrays for thermal imaging. It also find an application as ethanol sensor in ppm levels (up to 0.1 ppm).
Possible new uses include the preparation of bismuth vanadate ceramics for use in solid oxide fuel cells.[7] Another new application is in vanadium redox batteries, a type of flow battery used for energy storage, including large power facilities such as wind farms.
Biological activity
Despite being highly toxic in humans, vanadium occurs in some organisms, notably the Ascidiacea (sea squirts). These organisms contain the protein vanabins, the role of which is unclear. Vanadate (VO43−), formed by hydrolysis of V2O5 at high pH, appears to inhibit enzymes that process phosphate (PO43−). However the exact mode of action remains elusive.[5]
References
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-162. ISBN 0-8493-0462-8.
- ↑ Shklover, V.; Haibach, T.; Ried, F.; Nesper, R.; Novak, P. Crystal structure of the product of Mg2+ insertion into V2O5 single crystals. J. Solid State Chem. 1996, 123 (2), 317–23. DOI: 10.1006/jssc.1996.0186.
- ↑ Template:WebMineral.
- ↑ Template:Mindat.
- ↑ 5.0 5.1 5.2 5.3 Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 1140, 1144. ISBN 0-08-022057-6.
- ↑ Basic Organic Chemistry: Part 5, Industrial Products; Tedder, J. M.; Nechvatal, A.; Tubb, A. H., Eds.; John Wiley & Sons: Chichester, UK, 1975.
- ↑ Vaidhyanathan, B.; Balaji, K.; Rao, K. J. Microwave-Assisted Solid-State Synthesis of Oxide Ion Conducting Stabilized Bismuth Vanadate Phases. Chem. Mater. 1998, 10 (11), 3400–4. DOI: 10.1021/cm980092f
Further reading
- Vanadium Pentoxide. In Cobalt in Hard Metals and Cobalt Sulfate, Gallium Arsenide, Indium Phosphide and Vanadium Pentoxide; IARC Monographs on the Evaluation of Carcinogenic Risks to Humans 86; International Agency for Research on Cancer: Lyon, France, 2006; pp 227–92. ISBN 92-832-1286-X, <http://monographs.iarc.fr/ENG/Monographs/vol86/mono86-10.pdf>.
External links
- International Chemical Safety Card 0596
- NIOSH Pocket Guide to Chemical Hazards 0653
- NIOSH Pocket Guide to Chemical Hazards 0654
- Vanadium Pentoxide and other Inorganic Vanadium Compounds (Concise International Chemical Assessment Document 29)
- IPCS Environmental Health Criteria 81: Vanadium
- IPCS Health and Safety Guide 042: Vanadium and some vanadium salts
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