Industrial Phosphoruspentoxide with reasonable price

Phosphorus pentoxide

Phosphorus oxide (P2O5);Diphosphorus pentoxide;Phosphoric anhydride;Phosphorus pentaoxide;Phosphorus pentoxide;Diphosphorus pentaoxide;Phosphoric pentoxide;Diphosphorus pentaoxide (P2O5);Phosphorus oxide;Phosphoric acid anhydride;Phosphoric oxide;24377-84-2;50811-86-4;59778-57-3;72906-42-4;2566863-42-9

1314-56-3

O5P2

YWEUIGNSBFLMFL-UHFFFAOYSA-N

141.94500

141.92200

615-868-1

0545

1807

DTXSID9047754

/There are/ several crystalline & amorphous modifications; commercial form, hexagonal|White, orthogonal crystals|Exists in several forms but is often referred to by its empirical formula P2O5. Three crystalline polymorphs (H, O, O'), two distinct liquids,and several amorphous or glassy solids are recognized. The best-characterized form is the H (hexagonal) or alpha modification that consists of P4O10 molecules.

2809100000

Oxides and Peroxides

145.79000

1.1788

White to yellow crystalline powder

2.30 g/cm³

562 °C

500 °C @ Press: 550 Torr

340-360°C

1.433-1.436

soluble in sulfuric acid. Insoluble in acetone and ammonia. Decomposes in water.Readily absorbs moisture from the air forming a syrup of meta-, pyro-, and orthophosphoric acids. Reacts violently with water releasing considerable heat [Oldbury Chemicals, p. 9].

Storage Room low temperature ventilation drying ,Separate storage of caustic soda and flammable materials

1 mm Hg ( 384 °C)

4.9 (vs air)

Non-combustible. But encountering water and organic materials such as wood, cotton or straw, it reacts violently to release heat, may cause a fire.

Very deliquescent. Readily absorbs moisture from the air. Exothermic hydrolysis by water to form phosphoric acid. The reaction with alcohol is similar.|Heat of formation: -365.83 kcal/mole. Specific heat: 0.170 cal/g/ °C. Heat of fusion: 8.2 kcal/mole.|Sublimation temperature 360 °C.|Most important chemical property is its avidity for water. Below 100 °C, it is one of the most dehydrating agents known, extracting water from substances that are considered good dehydrating agents. For example it converts pure HNO3 to N2O5, H2SO4 to SO3, dehydrates amides to nitriles, reacts with alcohols to produce esters of simple and polymeric phosphoric acids, and effects ring closures and other condensation reactions.|For more Other Experimental Properties (Complete) data for PHOSPHORUS PENTOXIDE (6 total), please visit the HSDB record page.

Readily absorbs moisture from the air forming a syrup of meta-, pyro-, and orthophosphoric acids. Reacts violently with water releasing considerable heat [Oldbury Chemicals, p. 9]. There is a possibility that this very rapid, exothermic reaction would create a toxic acidic mist in a spill of the chemical into water.

Anhydrides

Water-Reactive

PHOSPHORIC ANHYDRIDE reacts violently and exothermically with water. The heat can ignite surrounding or admixed combustible materials. Undergoes hazardous or violent reactions with metal hydroxides and oxides, formic acid, hydrogen fluoride and hydrofluoric acid, iodides, metals (in particular potassium and sodium), oxidizing agents (bromine pentafluoride, chlorine trifluoride, perchloric acid, oxygen difluoride, hydrogen peroxide), ammonia, and proparygl alcohol. [Bretherick, 5th ed., 1995, p. 1781; EPA, 1998]. A violent explosion occurs if a solution of perchloric acid in chloroform is poured over phosphorus pentaoxide [EPA, 1998].

Corrosive

22.7 kcal/mole of P4O10