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Chemical reactions
8MgSO3 + 2KMnO4 → 7MgSO4 + MgO + 2Mn + K2SO3

8MgSO₃ + 2KMnO₄ → 7MgSO₄ + MgO + 2Mn + K₂SO₃

Last updated: June 13, 2022

Reaction of magnesium sulfite and potassium permanganate: 8MgSO₃Magnesium sulfite + 2KMnO₄Potassium permanganate
⟶
7MgSO₄Magnesium sulfate + MgOMagnesium oxide + 2MnManganese + K₂SO₃Potassium sulfite

The reaction of magnesium sulfite and potassium permanganate yields magnesium sulfate, magnesium oxide, manganese, and potassium sulfite (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 magnesium sulfite and potassium permanganate: 8MgSO₃Magnesium sulfite + 2KMnO₄Potassium permanganate
⟶
7MgSO₄Magnesium sulfate + MgOMagnesium oxide + 2MnManganese + K₂SO₃Potassium sulfite

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 magnesium sulfite and potassium permanganate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
MgSO₃	Magnesium sulfite	8	Reducing	Reducing
KMnO₄	Potassium permanganate	2	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
MgSO₄	Magnesium sulfate	7	Oxidized	–
MgO	Magnesium oxide	1	–	–
Mn	Manganese	2	Reduced	–
K₂SO₃	Potassium sulfite	1	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of magnesium sulfite and potassium permanganate: 8MgSO₃Crystalline solid + 2KMnO₄Crystalline solid
⟶
7MgSO₄Crystalline solid + MgOCrystalline solid + 2MnCrystalline solidα + K₂SO₃Crystalline 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	−977.0	–	–	–
per 1 mol of Magnesium sulfite	−122.1	–	–	–
per 1 mol of Potassium permanganate	−488.5	–	–	–
per 1 mol of Magnesium sulfate	−139.6	–	–	–
per 1 mol of Magnesium oxide	−977.0	–	–	–
per 1 mol of Manganese	−488.5	–	–	–
per 1 mol of Potassium sulfite	−977.0	–	–	–

Changes in standard condition (2)

Reaction of magnesium sulfite and potassium permanganate: 8MgSO₃Crystalline solid + 2KMnO₄Crystalline solid
⟶
7MgSO₄Crystalline solid + MgOCrystalline solid + 2MnCrystalline solidβ + K₂SO₃Crystalline 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	–	–	–	–
per 1 mol of Magnesium sulfite	–	–	–	–
per 1 mol of Potassium permanganate	–	–	–	–
per 1 mol of Magnesium sulfate	–	–	–	–
per 1 mol of Magnesium oxide	–	–	–	–
per 1 mol of Manganese	–	–	–	–
per 1 mol of Potassium sulfite	–	–	–	–

Changes in standard condition (3)

Reaction of magnesium sulfite and potassium permanganate: 8MgSO₃Crystalline solid + 2KMnO₄Crystalline solid
⟶
7MgSO₄Crystalline solid + MgOCrystalline solid + 2MnCrystalline solidγ + K₂SO₃Crystalline 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	−973.9	–	–	–
per 1 mol of Magnesium sulfite	−121.7	–	–	–
per 1 mol of Potassium permanganate	−486.9	–	–	–
per 1 mol of Magnesium sulfate	−139.1	–	–	–
per 1 mol of Magnesium oxide	−973.9	–	–	–
per 1 mol of Manganese	−486.9	–	–	–
per 1 mol of Potassium sulfite	−973.9	–	–	–

Changes in aqueous solution (1)

Reaction of magnesium sulfite and potassium permanganate ◆ Δ_rG −1164.2 kJ/mol K 9.10 × 10²⁰³ pK −203.96: 8MgSO₃Crystalline solid + 2KMnO₄Ionized aqueous solution
⟶
7MgSO₄Ionized aqueous solution + MgOCrystalline solid + 2MnCrystalline solidα + K₂SO₃Ionized 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	−1716.9	−1164.2	−1849	–
per 1 mol of Magnesium sulfite	−214.61	−145.53	−231.1	–
per 1 mol of Potassium permanganate	−858.45	−582.10	−924.5	–
per 1 mol of Magnesium sulfate	−245.27	−166.31	−264.1	–
per 1 mol of Magnesium oxide	−1716.9	−1164.2	−1849	–
per 1 mol of Manganese	−858.45	−582.10	−924.5	–
per 1 mol of Potassium sulfite	−1716.9	−1164.2	−1849	–

Changes in aqueous solution (2)

Reaction of magnesium sulfite and potassium permanganate ◆ Δ_rG −1253.1 kJ/mol K 3.42 × 10²¹⁹ pK −219.53: 8MgSO₃Crystalline solid + 2KMnO₄Ionized aqueous solution
⟶
7MgSO₄Un-ionized aqueous solution + MgOCrystalline solid + 2MnCrystalline solidα + K₂SO₃Ionized 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	−1576.1	−1253.1	−1072	–
per 1 mol of Magnesium sulfite	−197.01	−156.64	−134.0	–
per 1 mol of Potassium permanganate	−788.05	−626.55	−536.0	–
per 1 mol of Magnesium sulfate	−225.16	−179.01	−153.1	–
per 1 mol of Magnesium oxide	−1576.1	−1253.1	−1072	–
per 1 mol of Manganese	−788.05	−626.55	−536.0	–
per 1 mol of Potassium sulfite	−1576.1	−1253.1	−1072	–

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
MgSO₃ (cr)	-1008.3^[1]	-923.8^[1]	87.9^[1]	–
MgSO₃ (cr) 3 hydrate	-1931.8^[1]	-1674.7^[1]	209.2^[1]	–
MgSO₃ (cr) 6 hydrate	-2817.5^[1]	-2385.4^[1]	322.2^[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
MgSO₄ (cr)	-1284.9^[1]	-1170.6^[1]	91.6^[1]	96.48^[1]
MgSO₄ (ai)	-1376.12^[1]	-1199.5^[1]	-118.0^[1]	–
MgSO₄ (ao)	-1356.0^[1]	-1212.21^[1]	-7.1^[1]	–
MgSO₄ (cr) 1 hydrate	-1602.1^[1]	-1428.7^[1]	126.4^[1]	–
MgSO₄ (am) 1 hydrate	-1574.9^[1]	-1404.9^[1]	138.1^[1]	–
MgSO₄ (cr) 2 hydrate	-1896.2^[1]	–	–	–
MgSO₄ (cr) 4 hydrate	-2496.6^[1]	–	–	–
MgSO₄ (cr) 6 hydrate	-3087.0^[1]	-2631.8^[1]	348.1^[1]	348.11^[1]
MgSO₄ (cr) 7 hydrate	-3388.71^[1]	-2871.5^[1]	372^[1]	–
MgO (cr)	-597.98^[1]	-565.95^[1]	27.91^[1]	37.66^[1]
MgO (g)	17^[1]	–	–	–
Mn (cr) α	0^[1]	0^[1]	32.01^[1]	26.32^[1]
Mn (cr) β	–	–	34.39^[1]	26.53^[1]
Mn (cr) γ	1.55^[1]	1.42^[1]	32.43^[1]	27.57^[1]
Mn (g)	280.7^[1]	238.5^[1]	173.70^[1]	20.79^[1]
K₂SO₃ (cr)	-1125.5^[1]	–	–	–
K₂SO₃ (ai)	-1140.1^[1]	-1053.1^[1]	176^[1]	–

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

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