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Chemical reactions
3NH4SCN + 16Fe2O3 → N2O↑ + 3FeSO4 + 3FeCO3 + 26FeO + 4NH3↑

3NH₄SCN + 16Fe₂O₃ → N₂O↑ + 3FeSO₄ + 3FeCO₃ + 26FeO + 4NH₃↑

Last updated: May 12, 2022

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNAmmonium thiocyanate + 16Fe₂O₃Iron(III) oxide
⟶
N₂O↑Dinitrotgen monoxide + 3FeSO₄Iron(II) sulfate + 3FeCO₃Iron(II) carbonate + 26FeOIron(II) oxide + 4NH₃↑Ammonia

The reaction of ammonium thiocyanate and iron(III) oxide yields dinitrotgen monoxide, iron(II) sulfate, iron(II) carbonate, iron(II) oxide, and ammonia (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 + 16Fe₂O₃Iron(III) oxide
⟶
N₂O↑Dinitrotgen monoxide + 3FeSO₄Iron(II) sulfate + 3FeCO₃Iron(II) carbonate + 26FeOIron(II) oxide + 4NH₃↑Ammonia

General equation

Reaction of reducing species and reducible species: Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
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	16	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
N₂O	Dinitrotgen monoxide	1	Oxidized	–
FeSO₄	Iron(II) sulfate	3	Redoxed product	–
FeCO₃	Iron(II) carbonate	3	Reduced	–
FeO	Iron(II) oxide	26	Reduced	–
NH₃	Ammonia	4	–	–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNCrystalline solid + 16Fe₂O₃Crystalline solid
⟶
N₂O↑Gas + 3FeSO₄Crystalline solid + 3FeCO₃Crystalline solidsiderite + 26FeOCrystalline solid + 4NH₃↑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	1242.0	–	–	–
per 1 mol of Ammonium thiocyanate	414.00	–	–	–
per 1 mol of Iron(III) oxide	77.625	–	–	–
per 1 mol of Dinitrotgen monoxide	1242.0	–	–	–
per 1 mol of Iron(II) sulfate	414.00	–	–	–
per 1 mol of Iron(II) carbonate	414.00	–	–	–
per 1 mol of Iron(II) oxide	47.769	–	–	–
per 1 mol of Ammonia	310.50	–	–	–

Changes in aqueous solution (1)

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNIonized aqueous solution + 16Fe₂O₃Crystalline solid
⟶
N₂O↑Gas + 3FeSO₄Crystalline solid + 3FeCO₃Crystalline solidsiderite + 26FeOCrystalline solid + 4NH₃↑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	1174.1	–	–	–
per 1 mol of Ammonium thiocyanate	391.37	–	–	–
per 1 mol of Iron(III) oxide	73.381	–	–	–
per 1 mol of Dinitrotgen monoxide	1174.1	–	–	–
per 1 mol of Iron(II) sulfate	391.37	–	–	–
per 1 mol of Iron(II) carbonate	391.37	–	–	–
per 1 mol of Iron(II) oxide	45.158	–	–	–
per 1 mol of Ammonia	293.52	–	–	–

Changes in aqueous solution (2)

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNIonized aqueous solution + 16Fe₂O₃Crystalline solid
⟶
N₂O↑Gas + 3FeSO₄Crystalline solid + 3FeCO₃Crystalline solidsiderite + 26FeOCrystalline solid + 4NH₃↑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	1037.4	–	–	–
per 1 mol of Ammonium thiocyanate	345.80	–	–	–
per 1 mol of Iron(III) oxide	64.838	–	–	–
per 1 mol of Dinitrotgen monoxide	1037.4	–	–	–
per 1 mol of Iron(II) sulfate	345.80	–	–	–
per 1 mol of Iron(II) carbonate	345.80	–	–	–
per 1 mol of Iron(II) oxide	39.900	–	–	–
per 1 mol of Ammonia	259.35	–	–	–

Changes in aqueous solution (3)

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNIonized aqueous solution + 16Fe₂O₃Crystalline solid
⟶
N₂O↑Aqueous solution + 3FeSO₄Crystalline solid + 3FeCO₃Crystalline solidsiderite + 26FeOCrystalline solid + 4NH₃↑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	1148.2	–	–	–
per 1 mol of Ammonium thiocyanate	382.73	–	–	–
per 1 mol of Iron(III) oxide	71.763	–	–	–
per 1 mol of Dinitrotgen monoxide	1148.2	–	–	–
per 1 mol of Iron(II) sulfate	382.73	–	–	–
per 1 mol of Iron(II) carbonate	382.73	–	–	–
per 1 mol of Iron(II) oxide	44.162	–	–	–
per 1 mol of Ammonia	287.05	–	–	–

Changes in aqueous solution (4)

Reaction of ammonium thiocyanate and iron(III) oxide: 3NH₄SCNIonized aqueous solution + 16Fe₂O₃Crystalline solid
⟶
N₂O↑Aqueous solution + 3FeSO₄Crystalline solid + 3FeCO₃Crystalline solidsiderite + 26FeOCrystalline solid + 4NH₃↑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	1011.4	–	–	–
per 1 mol of Ammonium thiocyanate	337.13	–	–	–
per 1 mol of Iron(III) oxide	63.212	–	–	–
per 1 mol of Dinitrotgen monoxide	1011.4	–	–	–
per 1 mol of Iron(II) sulfate	337.13	–	–	–
per 1 mol of Iron(II) carbonate	337.13	–	–	–
per 1 mol of Iron(II) oxide	38.900	–	–	–
per 1 mol of Ammonia	252.85	–	–	–

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
N₂O (g)	82.05^[1]	104.20^[1]	219.85^[1]	38.45^[1]
N₂O (aq)	56.1^[1]	–	–	–
FeSO₄ (cr)	-928.4^[1]	-820.8^[1]	107.5^[1]	100.58^[1]
FeSO₄ (ai)	-998.3^[1]	-823.43^[1]	-117.6^[1]	–
FeSO₄ (cr) 1 hydrate	-1243.69^[1]	–	–	–
FeSO₄ (cr) 4 hydrate	-2129.2^[1]	–	–	–
FeSO₄ (cr) 7 hydrate	-3014.57^[1]	-2509.87^[1]	409.2^[1]	394.47^[1]
FeCO₃ (cr) siderite	-740.57^[1]	-666.67^[1]	92.9^[1]	82.13^[1]
FeO (cr)	-272.0^[1]	–	–	–
NH₃ (g)	-46.11^[1]	-16.45^[1]	192.45^[1]	35.06^[1]
NH₃ (ao)	-80.29^[1]	-26.50^[1]	111.3^[1]	–

* (g):Gas, (aq):Aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (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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