Home
Chemical reactions
16FeO + 2NaH2PO4 🔥→ 5Fe3O4 + 2P + 2NaOH + Fe(OH)2

16FeO + 2NaH₂PO₄ 🔥→ 5Fe₃O₄ + 2P + 2NaOH + Fe(OH)₂

Last updated: May 12, 2022

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOIron(II) oxide + 2NaH₂PO₄Sodium dihydrogenphosphate
🔥
⟶
5Fe₃O₄Iron(II,III) oxide + 2PPhosphorus + 2NaOHSodium hydroxide + Fe(OH)₂Iron(II) hydroxide

The reaction of iron(II) oxide and sodium dihydrogenphosphate yields iron(II,III) oxide, phosphorus, sodium hydroxide, and iron(II) hydroxide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of oxidizable species and reducible species

Table of contents

Reaction data

Chemical equation

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOIron(II) oxide + 2NaH₂PO₄Sodium dihydrogenphosphate
🔥
⟶
5Fe₃O₄Iron(II,III) oxide + 2PPhosphorus + 2NaOHSodium hydroxide + Fe(OH)₂Iron(II) hydroxide

General equation

Reaction of oxidizable species and reducible species: Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
🔥
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of iron(II) oxide and sodium dihydrogenphosphate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
FeO	Iron(II) oxide	16	Reducing	Oxidizable
NaH₂PO₄	Sodium dihydrogenphosphate	2	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Fe₃O₄	Iron(II,III) oxide	5	Oxidized	–
P	Phosphorus	2	Reduced	–
NaOH	Sodium hydroxide	2	–	–
Fe(OH)₂	Iron(II) hydroxide	1	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOCrystalline solid + 2NaH₂PO₄Crystalline solid
🔥
⟶
5Fe₃O₄Crystalline solid + 2PCrystalline solidwhite + 2NaOHCrystalline solid + Fe(OH)₂Crystalline solidprecipitated

	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	413.4	–	–	–
per 1 mol of Iron(II) oxide	25.84	–	–	–
per 1 mol of Sodium dihydrogenphosphate	206.7	–	–	–
per 1 mol of Iron(II,III) oxide	82.68	–	–	–
per 1 mol of Phosphorus	206.7	–	–	–
per 1 mol of Sodium hydroxide	206.7	–	–	–
per 1 mol of Iron(II) hydroxide	413.4	–	–	–

Changes in standard condition (2)

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOCrystalline solid + 2NaH₂PO₄Crystalline solid
🔥
⟶
5Fe₃O₄Crystalline solid + 2PCrystalline solidred, triclinic + 2NaOHCrystalline solid + Fe(OH)₂Crystalline solidprecipitated

	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	378.2	–	–	–
per 1 mol of Iron(II) oxide	23.64	–	–	–
per 1 mol of Sodium dihydrogenphosphate	189.1	–	–	–
per 1 mol of Iron(II,III) oxide	75.64	–	–	–
per 1 mol of Phosphorus	189.1	–	–	–
per 1 mol of Sodium hydroxide	189.1	–	–	–
per 1 mol of Iron(II) hydroxide	378.2	–	–	–

Changes in standard condition (3)

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOCrystalline solid + 2NaH₂PO₄Crystalline solid
🔥
⟶
5Fe₃O₄Crystalline solid + 2PCrystalline solidblack + 2NaOHCrystalline solid + Fe(OH)₂Crystalline solidprecipitated

	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	334.8	–	–	–
per 1 mol of Iron(II) oxide	20.93	–	–	–
per 1 mol of Sodium dihydrogenphosphate	167.4	–	–	–
per 1 mol of Iron(II,III) oxide	66.96	–	–	–
per 1 mol of Phosphorus	167.4	–	–	–
per 1 mol of Sodium hydroxide	167.4	–	–	–
per 1 mol of Iron(II) hydroxide	334.8	–	–	–

Changes in standard condition (4)

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOCrystalline solid + 2NaH₂PO₄Crystalline solid
🔥
⟶
5Fe₃O₄Crystalline solid + 2PAmorphous solidred + 2NaOHCrystalline solid + Fe(OH)₂Crystalline solidprecipitated

	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	398.4	–	–	–
per 1 mol of Iron(II) oxide	24.90	–	–	–
per 1 mol of Sodium dihydrogenphosphate	199.2	–	–	–
per 1 mol of Iron(II,III) oxide	79.68	–	–	–
per 1 mol of Phosphorus	199.2	–	–	–
per 1 mol of Sodium hydroxide	199.2	–	–	–
per 1 mol of Iron(II) hydroxide	398.4	–	–	–

Changes in aqueous solution

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 16FeOCrystalline solid + 2NaH₂PO₄Ionized aqueous solution
🔥
⟶
5Fe₃O₄Crystalline solid + 2PCrystalline solidwhite + 2NaOHIonized aqueous solution + Fe(OH)₂Crystalline solidprecipitated

	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	323.6	–	–	–
per 1 mol of Iron(II) oxide	20.23	–	–	–
per 1 mol of Sodium dihydrogenphosphate	161.8	–	–	–
per 1 mol of Iron(II,III) oxide	64.72	–	–	–
per 1 mol of Phosphorus	161.8	–	–	–
per 1 mol of Sodium hydroxide	161.8	–	–	–
per 1 mol of Iron(II) hydroxide	323.6	–	–	–

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
FeO (cr)	-272.0^[1]	–	–	–
NaH₂PO₄ (cr)	-1536.8^[1]	-1386.1^[1]	127.49^[1]	116.86^[1]
NaH₂PO₄ (ai)	-1536.41^[1]	-1392.17^[1]	149.4^[1]	–
NaH₂PO₄ (cr) 1 hydrate	-1833.0^[1]	–	–	–
NaH₂PO₄ (cr) 2 hydrate	-2128.4^[1]	–	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution

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
Fe₃O₄ (cr)	-1118.4^[1]	-1015.4^[1]	146.4^[1]	143.43^[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]
NaOH (cr)	-425.609^[1]	-379.494^[1]	64.455^[1]	59.54^[1]
NaOH (g)	-207.1^[1]	-210.0^[1]	228.43^[1]	48.37^[1]
NaOH (ai)	-470.114^[1]	-419.150^[1]	48.1^[1]	-102.1^[1]
NaOH (cr) 1 hydrate	-734.543^[1]	-629.338^[1]	99.50^[1]	90.17^[1]
NaOH (l) 2 hydrate	-1019.076^[1]	-873.091^[1]	195.979^[1]	239.41^[1]
NaOH (l) 3.5 hydrate	-1459.798^[1]	-1236.356^[1]	286.089^[1]	354.43^[1]
NaOH (l) 4 hydrate	-1605.15^[1]	-1356.64^[1]	318.70^[1]	–
NaOH (l) 5 hydrate	-1894.31^[1]	-1596.34^[1]	386.06^[1]	–
NaOH (l) 7 hydrate	-2469.02^[1]	-2073.80^[1]	526.31^[1]	–
Fe(OH)₂ (cr) precipitated	-569.0^[1]	-486.5^[1]	88^[1]	–
Fe(OH)₂ (g)	-372^[1]	–	–	–

* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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