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Chemical reactions
3NH4SCN + 23Fe2O3 🔥→ 3N2↑ + 3FeS + 3FeCO3 + 12Fe3O4 + 4Fe(OH)3

3NH₄SCN + 23Fe₂O₃ 🔥→ 3N₂↑ + 3FeS + 3FeCO₃ + 12Fe₃O₄ + 4Fe(OH)₃

Last updated: May 12, 2022

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNAmmonium thiocyanate + 23Fe₂O₃Iron(III) oxide
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3N₂↑Nitrogen + 3FeSIron(II) sulfide + 3FeCO₃Iron(II) carbonate + 12Fe₃O₄Iron(II,III) oxide + 4Fe(OH)₃Iron(III) hydroxide

The reaction of ammonium thiocyanate and iron(III) oxide yields nitrogen, iron(II) sulfide, iron(II) carbonate, 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 thiocyanate and iron(III) oxide: 3NH₄SCNAmmonium thiocyanate + 23Fe₂O₃Iron(III) oxide
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3N₂↑Nitrogen + 3FeSIron(II) sulfide + 3FeCO₃Iron(II) carbonate + 12Fe₃O₄Iron(II,III) oxide + 4Fe(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 thiocyanate and iron(III) oxide

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NH₄SCN	Ammonium thiocyanate	3	Reducing	Reducing
Fe₂O₃	Iron(III) oxide	23	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
N₂	Nitrogen	3	Oxidized	–
FeS	Iron(II) sulfide	3	Reduced	–
FeCO₃	Iron(II) carbonate	3	Reduced	–
Fe₃O₄	Iron(II,III) oxide	12	Reduced	–
Fe(OH)₃	Iron(III) hydroxide	4	–	–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNCrystalline solid + 23Fe₂O₃Crystalline solid
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3N₂↑Gas + 3FeSCrystalline solidiron-rich pyrrhotite, α + 3FeCO₃Crystalline solidsiderite + 12Fe₃O₄Crystalline solid + 4Fe(OH)₃Crystalline 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	−41.8	–	–	–
per 1 mol of Ammonium thiocyanate	−13.9	–	–	–
per 1 mol of Iron(III) oxide	−1.82	–	–	–
per 1 mol of Nitrogen	−13.9	–	–	–
per 1 mol of Iron(II) sulfide	−13.9	–	–	–
per 1 mol of Iron(II) carbonate	−13.9	–	–	–
per 1 mol of Iron(II,III) oxide	−3.48	–	–	–
per 1 mol of Iron(III) hydroxide	−10.4	–	–	–

Changes in aqueous solution

Reaction of ammonium thiocyanate and iron(III) oxide ◆ Δ_rG −92.8 kJ/mol K 1.81 × 10¹⁶ pK −16.26: 3NH₄SCNIonized aqueous solution + 23Fe₂O₃Crystalline solid
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3N₂↑Gas + 3FeSCrystalline solidiron-rich pyrrhotite, α + 3FeCO₃Crystalline solidsiderite + 12Fe₃O₄Crystalline solid + 4Fe(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	–	−92.8	–	–
per 1 mol of Ammonium thiocyanate	–	−30.9	–	–
per 1 mol of Iron(III) oxide	–	−4.03	–	–
per 1 mol of Nitrogen	–	−30.9	–	–
per 1 mol of Iron(II) sulfide	–	−30.9	–	–
per 1 mol of Iron(II) carbonate	–	−30.9	–	–
per 1 mol of Iron(II,III) oxide	–	−7.73	–	–
per 1 mol of Iron(III) hydroxide	–	−23.2	–	–

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
NH₄SCN (cr)	-78.7^[1]	–	–	–
NH₄SCN (ai)	-56.07^[1]	13.40^[1]	257.7^[1]	39.7^[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
N₂ (g)	0^[1]	0^[1]	191.61^[1]	29.125^[1]
FeS (cr) iron-rich pyrrhotite, α	-100.0^[1]	-100.4^[1]	60.29^[1]	50.54^[1]
FeCO₃ (cr) siderite	-740.57^[1]	-666.67^[1]	92.9^[1]	82.13^[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]	–	–

* (g):Gas, (cr):Crystalline solid, (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