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8P + 3Al(OH)3 + 3H2O → 3AlPO4 + 5PH3↑

8P + 3Al(OH)₃ + 3H₂O → 3AlPO₄ + 5PH₃↑

Last updated: June 13, 2022

Reaction of phosphorus, aluminium hydroxide, and water: 8PPhosphorus + 3Al(OH)₃Aluminium hydroxide + 3H₂OWater
⟶
3AlPO₄Aluminium phosphate + 5PH₃↑Phosphine

The reaction of phosphorus, aluminium hydroxide, and water yields aluminium phosphate and phosphine. This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of nonmetal and base in aqueous solution

Table of contents

Reaction data

Chemical equation

Reaction of phosphorus, aluminium hydroxide, and water: 8PPhosphorus + 3Al(OH)₃Aluminium hydroxide + 3H₂OWater
⟶
3AlPO₄Aluminium phosphate + 5PH₃↑Phosphine

General equation

Reaction of nonmetal and base in aqueous solution: NonmetalSelf redox agent + BaseNon-redox agent + H₂ONon-redox agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of phosphorus, aluminium hydroxide, and water

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
P	Phosphorus	8	–	Nonmetal
Al(OH)₃	Aluminium hydroxide	3	–	Base
H₂O	Water	3	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
AlPO₄	Aluminium phosphate	3	Oxidized	–
PH₃	Phosphine	5	Reduced	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of phosphorus, aluminium hydroxide, and water ◆ Δ_rG −157 kJ/mol K 3.20 × 10²⁷ pK −27.51: 8PCrystalline solidwhite + 3Al(OH)₃Crystalline solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−465	−157	572	−230.8
per 1 mol of Phosphorus	−58.1	−19.6	71.5	−28.85
per 1 mol of Aluminium hydroxide	−155	−52.3	191	−76.93
per 1 mol of Water	−155	−52.3	191	−76.93
per 1 mol of Aluminium phosphate	−155	−52.3	191	−76.93
per 1 mol of Phosphine	−93.0	−31.4	114	−46.16

Changes in standard condition (2)

Reaction of phosphorus, aluminium hydroxide, and water: 8PCrystalline solidwhite + 3Al(OH)₃Amorphous solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−489	–	–	–
per 1 mol of Phosphorus	−61.1	–	–	–
per 1 mol of Aluminium hydroxide	−163	–	–	–
per 1 mol of Water	−163	–	–	–
per 1 mol of Aluminium phosphate	−163	–	–	–
per 1 mol of Phosphine	−97.8	–	–	–

Changes in standard condition (3)

Reaction of phosphorus, aluminium hydroxide, and water ◆ Δ_rG −61 kJ/mol K 4.86 × 10¹⁰ pK −10.69: 8PCrystalline solidred, triclinic + 3Al(OH)₃Crystalline solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−324	−61	718	−209.8
per 1 mol of Phosphorus	−40.5	−7.6	89.8	−26.23
per 1 mol of Aluminium hydroxide	−108	−20	239	−69.93
per 1 mol of Water	−108	−20	239	−69.93
per 1 mol of Aluminium phosphate	−108	−20	239	−69.93
per 1 mol of Phosphine	−64.8	−12	144	−41.96

Changes in standard condition (4)

Reaction of phosphorus, aluminium hydroxide, and water: 8PCrystalline solidred, triclinic + 3Al(OH)₃Amorphous solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−348	–	–	–
per 1 mol of Phosphorus	−43.5	–	–	–
per 1 mol of Aluminium hydroxide	−116	–	–	–
per 1 mol of Water	−116	–	–	–
per 1 mol of Aluminium phosphate	−116	–	–	–
per 1 mol of Phosphine	−69.6	–	–	–

Changes in standard condition (5)

Reaction of phosphorus, aluminium hydroxide, and water: 8PCrystalline solidblack + 3Al(OH)₃Crystalline solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−151	–	–	–
per 1 mol of Phosphorus	−18.9	–	–	–
per 1 mol of Aluminium hydroxide	−50.3	–	–	–
per 1 mol of Water	−50.3	–	–	–
per 1 mol of Aluminium phosphate	−50.3	–	–	–
per 1 mol of Phosphine	−30.2	–	–	–

Changes in standard condition (6)

Reaction of phosphorus, aluminium hydroxide, and water: 8PCrystalline solidblack + 3Al(OH)₃Amorphous solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−175	–	–	–
per 1 mol of Phosphorus	−21.9	–	–	–
per 1 mol of Aluminium hydroxide	−58.3	–	–	–
per 1 mol of Water	−58.3	–	–	–
per 1 mol of Aluminium phosphate	−58.3	–	–	–
per 1 mol of Phosphine	−35.0	–	–	–

Changes in standard condition (7)

Reaction of phosphorus, aluminium hydroxide, and water: 8PAmorphous solidred + 3Al(OH)₃Crystalline solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−405	–	–	–
per 1 mol of Phosphorus	−50.6	–	–	–
per 1 mol of Aluminium hydroxide	−135	–	–	–
per 1 mol of Water	−135	–	–	–
per 1 mol of Aluminium phosphate	−135	–	–	–
per 1 mol of Phosphine	−81.0	–	–	–

Changes in standard condition (8)

Reaction of phosphorus, aluminium hydroxide, and water: 8PAmorphous solidred + 3Al(OH)₃Amorphous solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−429	–	–	–
per 1 mol of Phosphorus	−53.6	–	–	–
per 1 mol of Aluminium hydroxide	−143	–	–	–
per 1 mol of Water	−143	–	–	–
per 1 mol of Aluminium phosphate	−143	–	–	–
per 1 mol of Phosphine	−85.8	–	–	–

Changes in aqueous solution (1)

Reaction of phosphorus, aluminium hydroxide, and water ◆ Δ_rG −157 kJ/mol K 3.20 × 10²⁷ pK −27.51: 8PCrystalline solidwhite + 3Al(OH)₃Crystalline solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Gas

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−465	−157	572	−230.8
per 1 mol of Phosphorus	−58.1	−19.6	71.5	−28.85
per 1 mol of Aluminium hydroxide	−155	−52.3	191	−76.93
per 1 mol of Water	−155	−52.3	191	−76.93
per 1 mol of Aluminium phosphate	−155	−52.3	191	−76.93
per 1 mol of Phosphine	−93.0	−31.4	114	−46.16

Changes in aqueous solution (2)

Reaction of phosphorus, aluminium hydroxide, and water ◆ Δ_rG −98 kJ/mol K 1.48 × 10¹⁷ pK −17.17: 8PCrystalline solidwhite + 3Al(OH)₃Crystalline solid + 3H₂OLiquid
⟶
3AlPO₄Crystalline solid + 5PH₃↑Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−539	−98	121	–
per 1 mol of Phosphorus	−67.4	−12	15.1	–
per 1 mol of Aluminium hydroxide	−180	−33	40.3	–
per 1 mol of Water	−180	−33	40.3	–
per 1 mol of Aluminium phosphate	−180	−33	40.3	–
per 1 mol of Phosphine	−108	−20	24.2	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
P (cr) white	0^[1]	0^[1]	41.09^[1]	23.84^[1]
P (cr) red, triclinic	-17.6^[1]	-12.1^[1]	22.80^[1]	21.21^[1]
P (cr) black	-39.3^[1]	–	–	–
P (am) red	-7.5^[1]	–	–	–
P (g)	314.64^[1]	278.25^[1]	163.193^[1]	20.786^[1]
Al(OH)₃ (cr)	-1284^[2]	-1306^[2]	71^[2]	93.1^[2]
Al(OH)₃ (am)	-1276^[1]	–	–	–
H₂O (cr)	–	–	–	–
H₂O (l)	-285.830^[1]	-237.129^[1]	69.91^[1]	75.291^[1]
H₂O (g)	-241.818^[1]	-228.572^[1]	188.825^[1]	33.577^[1]

* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (l):Liquid

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
AlPO₄ (cr)	-1733.8^[1]	-1617.9^[1]	90.79^[1]	93.18^[1]
PH₃ (g)	5.4^[1]	13.4^[1]	210.23^[1]	37.11^[1]
PH₃ (ao)	-9.50^[1]	25.36^[1]	120.1^[1]	–

* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

1
Janiel J. Reed (1989)
The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list
2
James G. Speight (2017)
Lange's Handbook of Chemistry, 17th edition
https://www.accessengineeringlibrary.com/content/book/9781259586095
McGraw Hill Education
- Amazon
Citation list
- ^ Δ_fH°, -1284 kJ · mol⁻¹ - p.254
- ^ Δ_fG°, -1306 kJ · mol⁻¹ - p.254
- ^ S°, 71 J · K⁻¹ · mol⁻¹ - p.254
- ^ C_p°, 93.1 J · K⁻¹ · mol⁻¹ - p.254

Δ_rG	−157 kJ/mol
K	3.20 × 10²⁷
pK	−27.51

Δ_rG	−61 kJ/mol
K	4.86 × 10¹⁰
pK	−10.69

Δ_rG	−157 kJ/mol
K	3.20 × 10²⁷
pK	−27.51

Δ_rG	−98 kJ/mol
K	1.48 × 10¹⁷
pK	−17.17

8P + 3Al(OH)3 + 3H2O → 3AlPO4 + 5PH3↑

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition (1)

Changes in standard condition (2)

Changes in standard condition (3)

Changes in standard condition (4)

Changes in standard condition (5)

Changes in standard condition (6)

Changes in standard condition (7)

Changes in standard condition (8)

Changes in aqueous solution (1)

Changes in aqueous solution (2)

Thermodynamic data of reactants

Thermodynamic data of products

References

List of references

Related categories

Type of reaction

General equation

Reactant

Product

8P + 3Al(OH)₃ + 3H₂O → 3AlPO₄ + 5PH₃↑