Difference between revisions of "Phosphorus pentoxide"
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| − | '''Phosphorus pentoxide''' is | + | {{Chembox |
| + | | Name = Phosphorus pentoxide | ||
| + | | Reference = | ||
| + | | IUPACName = Phosphorus pentoxide | ||
| + | | PIN = | ||
| + | | SystematicName = | ||
| + | | OtherNames = Diphosphorus pentoxide<br>Phosphorus(V) oxide<br>Phosphoric anhydride<br>Tetraphosphorus decaoxide<br>Tetraphosphorus decoxide | ||
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| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
| + | | SMILES = | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| + | | Appearance = White powder | ||
| + | | BoilingPt = | ||
| + | | BoilingPtC = | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = Sublimes | ||
| + | | Density = 2.39 g/cm<sup>3</sup> | ||
| + | | Formula = P<sub>2</sub>O<sub>5</sub><br>P<sub>4</sub>O<sub>10</sub> | ||
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 283.886 g/mol | ||
| + | | MeltingPt = | ||
| + | | MeltingPtC = 360 | ||
| + | | MeltingPt_ref = | ||
| + | | MeltingPt_notes = (sublimes) | ||
| + | | Odor = Odorless | ||
| + | | pKa = | ||
| + | | pKb = | ||
| + | | Solubility = Reacts exothermically | ||
| + | | SolubleOther = Reacts with [[ethanol]], [[methanol]], [[isopropanol]]<br>Soluble in [[sulfuric acid]]<br>Insoluble in [[acetic acid]], [[acetone]], [[ammonia]], [[benzene]], [[chloroform]], [[dichloromethane]], [[hexane]], [[toluene]], [[xylene]] | ||
| + | | Solvent = | ||
| + | | VaporPressure = 1 mmHg at 385 °C | ||
| + | }} | ||
| + | | Section3 = {{Chembox Structure | ||
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| + | | Section4 = {{Chembox Thermochemistry | ||
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| + | | Section5 = {{Chembox Explosive | ||
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| + | | DetonationV = | ||
| + | | REFactor = | ||
| + | }} | ||
| + | | Section6 = {{Chembox Hazards | ||
| + | | AutoignitionPt = Non-flammable | ||
| + | | ExploLimits = Non-flammable | ||
| + | | ExternalMSDS = [https://www.fishersci.ca/viewmsds.do?catNo=A244500 FisherScientific] | ||
| + | | FlashPt = Non-flammable | ||
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| + | | LC50 = | ||
| + | | MainHazards = Corrosive | ||
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| + | }} | ||
| + | | Section7 = {{Chembox Related | ||
| + | | OtherAnions = | ||
| + | | OtherCations = | ||
| + | | OtherFunction = | ||
| + | | OtherFunction_label = | ||
| + | | OtherCompounds = [[Dinitrogen pentoxide]] | ||
| + | }} | ||
| + | }} | ||
| + | '''Phosphorus pentoxide''' or '''diphosphorus pentoxide''' is an inorganic chemical compound with molecular formula '''P<sub>4</sub>O<sub>10</sub>''', more often written as '''P<sub>2</sub>O<sub>5</sub>'''. | ||
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
Phosphorus pentoxide is the anhydride of [[phosphoric acid]]. It will react exothermically with water to yield the said acid. | Phosphorus pentoxide is the anhydride of [[phosphoric acid]]. It will react exothermically with water to yield the said acid. | ||
| + | |||
| + | : P<sub>2</sub>O<sub>5</sub> + 3 H<sub>2</sub>O → 2 H<sub>3</sub>PO<sub>4</sub> | ||
| + | |||
| + | Phosphorus pentoxide is also a very potent dehydrating agent. It is even capable of robbing water from [[sulfuric acid]], allowing one to distill [[sulfur trioxide]] from it. | ||
| + | |||
| + | : P<sub>2</sub>O<sub>5</sub> + H<sub>2</sub>SO<sub>4</sub> → H<sub>3</sub>PO<sub>4</sub> + SO<sub>3</sub> | ||
| + | |||
| + | This can be a quick method of preparing SO<sub>3</sub> without the use for contact process. | ||
===Physical=== | ===Physical=== | ||
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==Availability== | ==Availability== | ||
| − | Phosphorus pentoxide is sold by chemical suppliers. | + | Phosphorus pentoxide is sold by chemical suppliers, but is somewhat difficult to acquire. Storing it is also tricky due to its strong hygroscopy, though this can be limited by keeping the compound in a sealed bag. |
==Preparation== | ==Preparation== | ||
| − | Phosphorus pentoxide can be made by burning elemental phosphorus. | + | Phosphorus pentoxide can be made by burning elemental phosphorus, in a moisture-free environment. One way is to burn phosphorus in a large stainless steel pot with a lid, which has been kept in a dry box. The resulting phosphorus pentoxide fumes from the fire are allowed to settle and cool, then they're scraped off the pot in a dry environment. If you don't need high purity pentoxide, you can do this in open air, but you must move quickly. |
==Projects== | ==Projects== | ||
*Dry solvents, especially the halogenated ones, which cannot be dried with alkali metals | *Dry solvents, especially the halogenated ones, which cannot be dried with alkali metals | ||
| − | *Make pure phosphoric acid | + | *Make pure [[phosphoric acid]] |
*Convert primary amides into nitriles | *Convert primary amides into nitriles | ||
*Make [[dinitrogen pentoxide]] | *Make [[dinitrogen pentoxide]] | ||
*Make [[dichlorine heptoxide]] | *Make [[dichlorine heptoxide]] | ||
| + | *Make [[sulfur trioxide]] and [[oleum]] | ||
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| − | + | Phosphorus pentoxide is an extremely powerful desiccant, and contact with bare hand must be avoided. Contact with eyes will result in severe eye damage, even blindness. | |
===Storage=== | ===Storage=== | ||
| − | + | Phosphorus pentoxide must be kept in closed and sealed bottles, away from any moisture. Never store it in aluminium, and galvanized or tin-plated containers! Stainless steel or glass containers are ideal.<ref>http://datasheets.scbt.com/sc-203187.pdf</ref> | |
===Disposal=== | ===Disposal=== | ||
| + | Phosphorus pentoxide can be neutralized by very slowly adding it to crushed ice, followed by addition of a cooled carbonate/bicarbonate solution. | ||
==References== | ==References== | ||
<references/> | <references/> | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=1779 P2O5 and P4O10] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=61801 Recycling Phosphorus Pentoxide] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=98442 P2O5] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=157615 Is diphosphorus pentoxide hygroscopic?] | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
Latest revision as of 20:00, 12 September 2021
| Names | |
|---|---|
| IUPAC name
Phosphorus pentoxide
| |
| Other names
Diphosphorus pentoxide
Phosphorus(V) oxide Phosphoric anhydride Tetraphosphorus decaoxide Tetraphosphorus decoxide | |
| Properties | |
| P2O5 P4O10 | |
| Molar mass | 283.886 g/mol |
| Appearance | White powder |
| Odor | Odorless |
| Density | 2.39 g/cm3 |
| Melting point | 360 °C (680 °F; 633 K) (sublimes) |
| Boiling point | Sublimes |
| Reacts exothermically | |
| Solubility | Reacts with ethanol, methanol, isopropanol Soluble in sulfuric acid Insoluble in acetic acid, acetone, ammonia, benzene, chloroform, dichloromethane, hexane, toluene, xylene |
| Vapor pressure | 1 mmHg at 385 °C |
| Hazards | |
| Safety data sheet | FisherScientific |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Dinitrogen pentoxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Phosphorus pentoxide or diphosphorus pentoxide is an inorganic chemical compound with molecular formula P4O10, more often written as P2O5.
Contents
Properties
Chemical
Phosphorus pentoxide is the anhydride of phosphoric acid. It will react exothermically with water to yield the said acid.
- P2O5 + 3 H2O → 2 H3PO4
Phosphorus pentoxide is also a very potent dehydrating agent. It is even capable of robbing water from sulfuric acid, allowing one to distill sulfur trioxide from it.
- P2O5 + H2SO4 → H3PO4 + SO3
This can be a quick method of preparing SO3 without the use for contact process.
Physical
Phosphorous pentoxide is a white solid, with a pungent odor and strong deliquescent. Its density is 2.30 g/cm3. It boils at 423 °C under atmospheric pressure; if heated more rapidly it can sublimate.
Availability
Phosphorus pentoxide is sold by chemical suppliers, but is somewhat difficult to acquire. Storing it is also tricky due to its strong hygroscopy, though this can be limited by keeping the compound in a sealed bag.
Preparation
Phosphorus pentoxide can be made by burning elemental phosphorus, in a moisture-free environment. One way is to burn phosphorus in a large stainless steel pot with a lid, which has been kept in a dry box. The resulting phosphorus pentoxide fumes from the fire are allowed to settle and cool, then they're scraped off the pot in a dry environment. If you don't need high purity pentoxide, you can do this in open air, but you must move quickly.
Projects
- Dry solvents, especially the halogenated ones, which cannot be dried with alkali metals
- Make pure phosphoric acid
- Convert primary amides into nitriles
- Make dinitrogen pentoxide
- Make dichlorine heptoxide
- Make sulfur trioxide and oleum
Handling
Safety
Phosphorus pentoxide is an extremely powerful desiccant, and contact with bare hand must be avoided. Contact with eyes will result in severe eye damage, even blindness.
Storage
Phosphorus pentoxide must be kept in closed and sealed bottles, away from any moisture. Never store it in aluminium, and galvanized or tin-plated containers! Stainless steel or glass containers are ideal.[1]
Disposal
Phosphorus pentoxide can be neutralized by very slowly adding it to crushed ice, followed by addition of a cooled carbonate/bicarbonate solution.
