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Chemical reactions
6NH4SCN + 6KMnO4 → 3NH4NO2 + 6MnO2 + 4KSCN + 2KHS + 2NH4HCO3

6NH₄SCN + 6KMnO₄ → 3NH₄NO₂ + 6MnO₂ + 4KSCN + 2KHS + 2NH₄HCO₃

Last updated: May 12, 2022

Reaction of ammonium thiocyanate and potassium permanganate: 6NH₄SCNAmmonium thiocyanate + 6KMnO₄Potassium permanganate
⟶
3NH₄NO₂Ammonium nitrite + 6MnO₂Manganese(IV) oxide + 4KSCNPotassium thiocyanate + 2KHSPotassium hydrogensulfide + 2NH₄HCO₃Ammonium hydrogencarbonate

The reaction of ammonium thiocyanate and potassium permanganate yields ammonium nitrite, manganese(IV) oxide, potassium thiocyanate, potassium hydrogensulfide, and ammonium hydrogencarbonate (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of reducing species and oxidizing species

Table of contents

Reaction data

Chemical equation

Reaction of ammonium thiocyanate and potassium permanganate: 6NH₄SCNAmmonium thiocyanate + 6KMnO₄Potassium permanganate
⟶
3NH₄NO₂Ammonium nitrite + 6MnO₂Manganese(IV) oxide + 4KSCNPotassium thiocyanate + 2KHSPotassium hydrogensulfide + 2NH₄HCO₃Ammonium hydrogencarbonate

General equation

Reaction of reducing species and oxidizing species: Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium thiocyanate and potassium permanganate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NH₄SCN	Ammonium thiocyanate	6	Reducing	Reducing
KMnO₄	Potassium permanganate	6	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
NH₄NO₂	Ammonium nitrite	3	Oxidized	–
MnO₂	Manganese(IV) oxide	6	Reduced	–
KSCN	Potassium thiocyanate	4	–	–
KHS	Potassium hydrogensulfide	2	–	–
NH₄HCO₃	Ammonium hydrogencarbonate	2	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of ammonium thiocyanate and potassium permanganate: 6NH₄SCNCrystalline solid + 6KMnO₄Crystalline solid
⟶
3NH₄NO₂Crystalline solid + 6MnO₂Crystalline solid + 4KSCNCrystalline solid + 2KHSCrystalline solid + 2NH₄HCO₃Crystalline solid

	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	−1423.9	–	–	–
per 1 mol of Ammonium thiocyanate	−237.32	–	–	–
per 1 mol of Potassium permanganate	−237.32	–	–	–
per 1 mol of Ammonium nitrite	−474.63	–	–	–
per 1 mol of Manganese(IV) oxide	−237.32	–	–	–
per 1 mol of Potassium thiocyanate	−355.98	–	–	–
per 1 mol of Potassium hydrogensulfide	−711.95	–	–	–
per 1 mol of Ammonium hydrogencarbonate	−711.95	–	–	–

Changes in standard condition (2)

Reaction of ammonium thiocyanate and potassium permanganate: 6NH₄SCNCrystalline solid + 6KMnO₄Crystalline solid
⟶
3NH₄NO₂Crystalline solid + 6MnO₂Amorphous solidprecipitated + 4KSCNCrystalline solid + 2KHSCrystalline solid + 2NH₄HCO₃Crystalline solid

	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	−1318.7	–	–	–
per 1 mol of Ammonium thiocyanate	−219.78	–	–	–
per 1 mol of Potassium permanganate	−219.78	–	–	–
per 1 mol of Ammonium nitrite	−439.57	–	–	–
per 1 mol of Manganese(IV) oxide	−219.78	–	–	–
per 1 mol of Potassium thiocyanate	−329.68	–	–	–
per 1 mol of Potassium hydrogensulfide	−659.35	–	–	–
per 1 mol of Ammonium hydrogencarbonate	−659.35	–	–	–

Changes in aqueous solution (1)

Reaction of ammonium thiocyanate and potassium permanganate ◆ Δ_rG −1459.8 kJ/mol K 5.57 × 10²⁵⁵ pK −255.75: 6NH₄SCNIonized aqueous solution + 6KMnO₄Ionized aqueous solution
⟶
3NH₄NO₂Ionized aqueous solution + 6MnO₂Crystalline solid + 4KSCNIonized aqueous solution + 2KHSIonized aqueous solution + 2NH₄HCO₃Ionized 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	−1625.1	−1459.8	−553.5	–
per 1 mol of Ammonium thiocyanate	−270.85	−243.30	−92.25	–
per 1 mol of Potassium permanganate	−270.85	−243.30	−92.25	–
per 1 mol of Ammonium nitrite	−541.70	−486.60	−184.5	–
per 1 mol of Manganese(IV) oxide	−270.85	−243.30	−92.25	–
per 1 mol of Potassium thiocyanate	−406.27	−364.95	−138.4	–
per 1 mol of Potassium hydrogensulfide	−812.55	−729.90	−276.8	–
per 1 mol of Ammonium hydrogencarbonate	−812.55	−729.90	−276.8	–

Changes in aqueous solution (2)

Reaction of ammonium thiocyanate and potassium permanganate: 6NH₄SCNIonized aqueous solution + 6KMnO₄Ionized aqueous solution
⟶
3NH₄NO₂Ionized aqueous solution + 6MnO₂Crystalline solid + 4KSCNIonized aqueous solution + 2KHSIonized aqueous solution + 2NH₄HCO₃Aqueous 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	−1619.5	–	–	–
per 1 mol of Ammonium thiocyanate	−269.92	–	–	–
per 1 mol of Potassium permanganate	−269.92	–	–	–
per 1 mol of Ammonium nitrite	−539.83	–	–	–
per 1 mol of Manganese(IV) oxide	−269.92	–	–	–
per 1 mol of Potassium thiocyanate	−404.88	–	–	–
per 1 mol of Potassium hydrogensulfide	−809.75	–	–	–
per 1 mol of Ammonium hydrogencarbonate	−809.75	–	–	–

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]
KMnO₄ (cr)	-837.2^[1]	-737.6^[1]	171.71^[1]	117.57^[1]
KMnO₄ (ai)	-793.8^[1]	-730.5^[1]	293.7^[1]	-60.2^[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
NH₄NO₂ (cr)	-256.5^[1]	–	–	–
NH₄NO₂ (ai)	-237.2^[1]	-111.6^[1]	236.4^[1]	-17.6^[1]
MnO₂ (cr)	-520.03^[1]	-465.14^[1]	53.05^[1]	54.14^[1]
MnO₂ (am) precipitated	-502.5^[1]	–	–	–
KSCN (cr)	-200.16^[1]	-178.31^[1]	124.26^[1]	88.53^[1]
KSCN (ai)	-175.94^[1]	-190.56^[1]	246.9^[1]	-18.4^[1]
KHS (cr)	-265.10^[1]	–	–	75.31^[1]
KHS (ai)	-269.9^[1]	-271.19^[1]	165.3^[1]	–
KHS (cr) 0.25 hydrate	-337.2^[1]	–	–	–
NH₄HCO₃ (cr)	-849.4^[1]	-665.9^[1]	120.9^[1]	–
NH₄HCO₃ (ai)	-824.50^[1]	-666.07^[1]	204.6^[1]	–
NH₄HCO₃ (aq)	-821.7^[1]	–	–	–

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