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13CuS + 8KMnO4 → CuSO4 + 12CuO + 4K2SO4 + 8MnS

13CuS + 8KMnO₄ → CuSO₄ + 12CuO + 4K₂SO₄ + 8MnS

Last updated: June 13, 2022

Reaction of copper(II) sulfide and potassium permanganate: 13CuSCopper(II) sulfide + 8KMnO₄Potassium permanganate
⟶
CuSO₄Copper(II) sulfate + 12CuOCopper(II) oxide + 4K₂SO₄Potassium sulfate + 8MnSManganese(II) sulfide

The reaction of copper(II) sulfide and potassium permanganate yields copper(II) sulfate, copper(II) oxide, potassium sulfate, and manganese(II) sulfide (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 copper(II) sulfide and potassium permanganate: 13CuSCopper(II) sulfide + 8KMnO₄Potassium permanganate
⟶
CuSO₄Copper(II) sulfate + 12CuOCopper(II) oxide + 4K₂SO₄Potassium sulfate + 8MnSManganese(II) sulfide

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 copper(II) sulfide and potassium permanganate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
CuS	Copper(II) sulfide	13	Reducing	Reducing
KMnO₄	Potassium permanganate	8	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
CuSO₄	Copper(II) sulfate	1	Oxidized	–
CuO	Copper(II) oxide	12	–	–
K₂SO₄	Potassium sulfate	4	Oxidized	–
MnS	Manganese(II) sulfide	8	Reduced	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper(II) sulfide and potassium permanganate ◆ Δ_rG −2653.3 kJ/mol K 6.89 × 10⁴⁶⁴ pK −464.84: 13CuSCrystalline solid + 8KMnO₄Crystalline solid
⟶
CuSO₄Crystalline solid + 12CuOCrystalline solid + 4K₂SO₄Crystalline solid + 8MnSCrystalline solidgreen

	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	−2735.8	−2653.3	−290	−29.1
per 1 mol of Copper(II) sulfide	−210.45	−204.10	−22.3	−2.24
per 1 mol of Potassium permanganate	−341.98	−331.66	−36.3	−3.64
per 1 mol of Copper(II) sulfate	−2735.8	−2653.3	−290	−29.1
per 1 mol of Copper(II) oxide	−227.98	−221.11	−24.2	−2.43
per 1 mol of Potassium sulfate	−683.95	−663.33	−72.5	−7.28
per 1 mol of Manganese(II) sulfide	−341.98	−331.66	−36.3	−3.64

Changes in standard condition (2)

Reaction of copper(II) sulfide and potassium permanganate: 13CuSCrystalline solid + 8KMnO₄Crystalline solid
⟶
CuSO₄Crystalline solid + 12CuOCrystalline solid + 4K₂SO₄Crystalline solid + 8MnSAmorphous solidprecipitated, pink

	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	−2732.6	–	–	–
per 1 mol of Copper(II) sulfide	−210.20	–	–	–
per 1 mol of Potassium permanganate	−341.57	–	–	–
per 1 mol of Copper(II) sulfate	−2732.6	–	–	–
per 1 mol of Copper(II) oxide	−227.72	–	–	–
per 1 mol of Potassium sulfate	−683.15	–	–	–
per 1 mol of Manganese(II) sulfide	−341.57	–	–	–

Changes in aqueous solution (1)

Reaction of copper(II) sulfide and potassium permanganate ◆ Δ_rG −2699.3 kJ/mol K 7.89 × 10⁴⁷² pK −472.90: 13CuSCrystalline solid + 8KMnO₄Ionized aqueous solution
⟶
CuSO₄Un-ionized aqueous solution + 12CuOCrystalline solid + 4K₂SO₄Ionized aqueous solution + 8MnSCrystalline solidgreen

	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	–	−2699.3	–	–
per 1 mol of Copper(II) sulfide	–	−207.64	–	–
per 1 mol of Potassium permanganate	–	−337.41	–	–
per 1 mol of Copper(II) sulfate	–	−2699.3	–	–
per 1 mol of Copper(II) oxide	–	−224.94	–	–
per 1 mol of Potassium sulfate	–	−674.83	–	–
per 1 mol of Manganese(II) sulfide	–	−337.41	–	–

Changes in aqueous solution (2)

Reaction of copper(II) sulfide and potassium permanganate ◆ Δ_rG −2668.9 kJ/mol K 3.72 × 10⁴⁶⁷ pK −467.57: 13CuSCrystalline solid + 8KMnO₄Ionized aqueous solution
⟶
CuSO₄Crystalline solid + 12CuOCrystalline solid + 4K₂SO₄Ionized aqueous solution + 8MnSCrystalline solidgreen

	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	−2987.9	−2668.9	−1068	−137
per 1 mol of Copper(II) sulfide	−229.84	−205.30	−82.15	−10.5
per 1 mol of Potassium permanganate	−373.49	−333.61	−133.5	−17.1
per 1 mol of Copper(II) sulfate	−2987.9	−2668.9	−1068	−137
per 1 mol of Copper(II) oxide	−248.99	−222.41	−89.00	−11.4
per 1 mol of Potassium sulfate	−746.98	−667.23	−267.0	−34.3
per 1 mol of Manganese(II) sulfide	−373.49	−333.61	−133.5	−17.1

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
CuS (cr)	-53.1^[1]	-53.6^[1]	66.5^[1]	47.82^[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
CuSO₄ (cr)	-771.36^[1]	-661.8^[1]	109^[1]	100.0^[1]
CuSO₄ (ai)	-844.50^[1]	-679.04^[1]	-79.5^[1]	–
CuSO₄ (ao)	–	-692.18^[1]	–	–
CuSO₄ (cr) 1 hydrate	-1085.83^[1]	-918.11^[1]	146.0^[1]	134^[1]
CuSO₄ (cr) 3 hydrate	-1684.31^[1]	-1399.96^[1]	221.3^[1]	205^[1]
CuSO₄ (cr) 5 hydrate	-2279.65^[1]	-1879.745^[1]	300.4^[1]	280^[1]
CuO (cr)	-157.3^[1]	-129.7^[1]	42.63^[1]	42.30^[1]
K₂SO₄ (cr)	-1437.79^[1]	-1321.37^[1]	175.56^[1]	131.46^[1]
K₂SO₄ (g)	-1096^[1]	-1033^[1]	364^[1]	108.8^[1]
K₂SO₄ (ai)	-1414.02^[1]	-1311.07^[1]	225.1^[1]	-251^[1]
MnS (cr) green	-214.2^[1]	-218.4^[1]	78.2^[1]	49.96^[1]
MnS (am) precipitated, pink	-213.8^[1]	–	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas, (am):Amorphous solid

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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