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Chemical reactions
6FeO + 3NaH2PO4 🔥→ 2FePO4 + 2Fe2O3 + Na3PO4 + 3H2↑

6FeO + 3NaH₂PO₄ 🔥→ 2FePO₄ + 2Fe₂O₃ + Na₃PO₄ + 3H₂↑

Last updated: May 12, 2022

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 6FeOIron(II) oxide + 3NaH₂PO₄Sodium dihydrogenphosphate
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2FePO₄Iron(III) phosphate + 2Fe₂O₃Iron(III) oxide + Na₃PO₄Sodium phosphate + 3H₂↑Hydrogen

The reaction of iron(II) oxide and sodium dihydrogenphosphate yields iron(III) phosphate, iron(III) oxide, sodium phosphate, and hydrogen (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: 6FeOIron(II) oxide + 3NaH₂PO₄Sodium dihydrogenphosphate
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2FePO₄Iron(III) phosphate + 2Fe₂O₃Iron(III) oxide + Na₃PO₄Sodium phosphate + 3H₂↑Hydrogen

General equation

Reaction of oxidizable species and reducible species: Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
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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	6	Reducing	Oxidizable
NaH₂PO₄	Sodium dihydrogenphosphate	3	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
FePO₄	Iron(III) phosphate	2	Oxidized	–
Fe₂O₃	Iron(III) oxide	2	Oxidized	–
Na₃PO₄	Sodium phosphate	1	–	–
H₂	Hydrogen	3	Reduced	–

Thermodynamic changes

Changes in standard condition

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 6FeOCrystalline solid + 3NaH₂PO₄Crystalline solid
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2FePO₄Crystalline solid + 2Fe₂O₃Crystalline solid + Na₃PO₄Crystalline solid + 3H₂↑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	81.6	–	–	–
per 1 mol of Iron(II) oxide	13.6	–	–	–
per 1 mol of Sodium dihydrogenphosphate	27.2	–	–	–
per 1 mol of Iron(III) phosphate	40.8	–	–	–
per 1 mol of Iron(III) oxide	40.8	–	–	–
per 1 mol of Sodium phosphate	81.6	–	–	–
per 1 mol of Hydrogen	27.2	–	–	–

Changes in aqueous solution (1)

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 6FeOCrystalline solid + 3NaH₂PO₄Ionized aqueous solution
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2FePO₄Crystalline solid + 2Fe₂O₃Crystalline solid + Na₃PO₄Ionized aqueous solution + 3H₂↑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	−0.1	–	–	–
per 1 mol of Iron(II) oxide	−0.017	–	–	–
per 1 mol of Sodium dihydrogenphosphate	−0.033	–	–	–
per 1 mol of Iron(III) phosphate	−0.050	–	–	–
per 1 mol of Iron(III) oxide	−0.050	–	–	–
per 1 mol of Sodium phosphate	−0.10	–	–	–
per 1 mol of Hydrogen	−0.033	–	–	–

Changes in aqueous solution (2)

Reaction of iron(II) oxide and sodium dihydrogenphosphate: 6FeOCrystalline solid + 3NaH₂PO₄Ionized aqueous solution
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2FePO₄Crystalline solid + 2Fe₂O₃Crystalline solid + Na₃PO₄Ionized aqueous solution + 3H₂↑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	−12.7	–	–	–
per 1 mol of Iron(II) oxide	−2.12	–	–	–
per 1 mol of Sodium dihydrogenphosphate	−4.23	–	–	–
per 1 mol of Iron(III) phosphate	−6.35	–	–	–
per 1 mol of Iron(III) oxide	−6.35	–	–	–
per 1 mol of Sodium phosphate	−12.7	–	–	–
per 1 mol of Hydrogen	−4.23	–	–	–

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
FePO₄ (cr)	-1297.5^[1]	–	–	–
FePO₄ (cr) 2 hydrate strengite	-1888.2^[1]	-1657.5^[1]	171.25^[1]	180.54^[1]
Fe₂O₃ (cr)	-824.2^[1]	-742.2^[1]	87.40^[1]	103.85^[1]
Na₃PO₄ (cr)	-1917.40^[1]	-1788.80^[1]	173.80^[1]	153.47^[1]
Na₃PO₄ (ai)	-1997.9^[1]	-1804.5^[1]	-43.3^[1]	–
H₂ (g)	0^[1]	0^[1]	130.684^[1]	28.824^[1]
H₂ (ao)	-4.2^[1]	17.6^[1]	577^[1]	–

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