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Chemical reactions
6NH4Cl + 86Fe2O3 🔥→ 2Fe(NO3)3 + 3Cl2↑ + 54Fe3O4 + 8Fe(OH)3

6NH₄Cl + 86Fe₂O₃ 🔥→ 2Fe(NO₃)₃ + 3Cl₂↑ + 54Fe₃O₄ + 8Fe(OH)₃

Last updated: May 12, 2022

Reaction of ammonium chloride and iron(III) oxide: 6NH₄ClAmmonium chloride + 86Fe₂O₃Iron(III) oxide
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2Fe(NO₃)₃Iron(III) nitrate + 3Cl₂↑Chlorine + 54Fe₃O₄Iron(II,III) oxide + 8Fe(OH)₃Iron(III) hydroxide

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

Reaction of reducing species and reducible species

Table of contents

Reaction data

Chemical equation

Reaction of ammonium chloride and iron(III) oxide: 6NH₄ClAmmonium chloride + 86Fe₂O₃Iron(III) oxide
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2Fe(NO₃)₃Iron(III) nitrate + 3Cl₂↑Chlorine + 54Fe₃O₄Iron(II,III) oxide + 8Fe(OH)₃Iron(III) hydroxide

General equation

Reaction of reducing species and reducible species: Reducing speciesReducing agent + Reducible speciesOxidizing agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium chloride and iron(III) oxide

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NH₄Cl	Ammonium chloride	6	Reducing	Reducing
Fe₂O₃	Iron(III) oxide	86	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Fe(NO₃)₃	Iron(III) nitrate	2	Oxidized	–
Cl₂	Chlorine	3	Oxidized	–
Fe₃O₄	Iron(II,III) oxide	54	Reduced	–
Fe(OH)₃	Iron(III) hydroxide	8	–	–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium chloride and iron(III) oxide ◆ Δ_rG 4309.7 kJ/mol K 0.94 × 10⁻⁷⁵⁵ pK 755.03: 6NH₄ClIonized aqueous solution + 86Fe₂O₃Crystalline solid
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2Fe(NO₃)₃Ionized aqueous solution + 3Cl₂↑Gas + 54Fe₃O₄Crystalline solid + 8Fe(OH)₃Un-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	–	4309.7	–	–
per 1 mol of Ammonium chloride	–	718.28	–	–
per 1 mol of Iron(III) oxide	–	50.113	–	–
per 1 mol of Iron(III) nitrate	–	2154.8	–	–
per 1 mol of Chlorine	–	1436.6	–	–
per 1 mol of Iron(II,III) oxide	–	79.809	–	–
per 1 mol of Iron(III) hydroxide	–	538.71	–	–

Changes in aqueous solution (2)

Reaction of ammonium chloride and iron(III) oxide ◆ Δ_rG 4330.5 kJ/mol K 0.21 × 10⁻⁷⁵⁸ pK 758.67: 6NH₄ClIonized aqueous solution + 86Fe₂O₃Crystalline solid
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2Fe(NO₃)₃Ionized aqueous solution + 3Cl₂↑Un-ionized aqueous solution + 54Fe₃O₄Crystalline solid + 8Fe(OH)₃Un-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	–	4330.5	–	–
per 1 mol of Ammonium chloride	–	721.75	–	–
per 1 mol of Iron(III) oxide	–	50.355	–	–
per 1 mol of Iron(III) nitrate	–	2165.3	–	–
per 1 mol of Chlorine	–	1443.5	–	–
per 1 mol of Iron(II,III) oxide	–	80.194	–	–
per 1 mol of Iron(III) hydroxide	–	541.31	–	–

Changes in aqueous solution (3)

Reaction of ammonium chloride and iron(III) oxide: 6NH₄ClIonized aqueous solution + 86Fe₂O₃Crystalline solid
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2Fe(NO₃)₃Aqueous solution + 3Cl₂↑Gas + 54Fe₃O₄Crystalline solid + 8Fe(OH)₃Un-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	–	–	–	–
per 1 mol of Ammonium chloride	–	–	–	–
per 1 mol of Iron(III) oxide	–	–	–	–
per 1 mol of Iron(III) nitrate	–	–	–	–
per 1 mol of Chlorine	–	–	–	–
per 1 mol of Iron(II,III) oxide	–	–	–	–
per 1 mol of Iron(III) hydroxide	–	–	–	–

Changes in aqueous solution (4)

Reaction of ammonium chloride and iron(III) oxide: 6NH₄ClIonized aqueous solution + 86Fe₂O₃Crystalline solid
🔥
⟶
2Fe(NO₃)₃Aqueous solution + 3Cl₂↑Un-ionized aqueous solution + 54Fe₃O₄Crystalline solid + 8Fe(OH)₃Un-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	–	–	–	–
per 1 mol of Ammonium chloride	–	–	–	–
per 1 mol of Iron(III) oxide	–	–	–	–
per 1 mol of Iron(III) nitrate	–	–	–	–
per 1 mol of Chlorine	–	–	–	–
per 1 mol of Iron(II,III) oxide	–	–	–	–
per 1 mol of Iron(III) hydroxide	–	–	–	–

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
NH₄Cl (cr)	-314.43^[1]	-202.87^[1]	94.6^[1]	84.1^[1]
NH₄Cl (ai)	-299.66^[1]	-210.52^[1]	169.9^[1]	-56.5^[1]
Fe₂O₃ (cr)	-824.2^[1]	-742.2^[1]	87.40^[1]	103.85^[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
Fe(NO₃)₃ (ai)	-670.7^[1]	-338.3^[1]	123.4^[1]	–
Fe(NO₃)₃ (aq)	-674.9^[1]	–	–	–
Fe(NO₃)₃ (cr) 9 hydrate	-3285.3^[1]	–	–	–
Cl₂ (g)	0^[1]	0^[1]	223.066^[1]	33.907^[1]
Cl₂ (ao)	-23.4^[1]	6.94^[1]	121^[1]	–
Fe₃O₄ (cr)	-1118.4^[1]	-1015.4^[1]	146.4^[1]	143.43^[1]
Fe(OH)₃ (cr) precipitated	-823.0^[1]	-696.5^[1]	106.7^[1]	–
Fe(OH)₃ (ao)	–	-659.3^[1]	–	–

* (ai):Ionized aqueous solution, (aq):Aqueous solution, (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)
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