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3Na2SO3 + 2KMnO4 → 3Na2SO4 + 2MnO2 + K2O

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Reaction of sodium sulfite and potassium permanganate
3Na2SO3Sodium sulfite + 2KMnO4Potassium permanganate
⟶
3Na2SO4Sodium sulfate + 2MnO2Manganese(IV) oxide + K2OPotassium oxide

The reaction of sodium sulfite and potassium permanganate yields sodium sulfate, manganese(IV) oxide, and potassium oxide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of sodium sulfite and potassium permanganate
3Na2SO3Sodium sulfite + 2KMnO4Potassium permanganate
⟶
3Na2SO4Sodium sulfate + 2MnO2Manganese(IV) oxide + K2OPotassium oxide

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 sodium sulfite and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO3Sodium sulfite3
Reducing
Reducing
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate3
Oxidized
–
MnO2Manganese(IV) oxide2
Reduced
–
K2OPotassium oxide1
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium sulfite and potassium permanganate
◆
ΔrG−550.2 kJ/mol
K2.46 × 1096
pK−96.39
3Na2SO3Crystalline solid + 2KMnO4Crystalline solid
⟶
3Na2SO4Crystalline solidorthorhombic + 2MnO2Crystalline solid + K2OCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−586.0−550.2−132.3−19.3
per 1 mol of
−195.3−183.4−44.10−6.43
−293.0−275.1−66.15−9.65
per 1 mol of
−195.3−183.4−44.10−6.43
−293.0−275.1−66.15−9.65
per 1 mol of
−586.0−550.2−132.3−19.3

Changes in standard condition (2)

Reaction of sodium sulfite and potassium permanganate
3Na2SO3Crystalline solid + 2KMnO4Crystalline solid
⟶
3Na2SO4Crystalline solidorthorhombic + 2MnO2Amorphous solidprecipitated + K2OCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−550.9–––
per 1 mol of
−183.6–––
−275.4–––
per 1 mol of
−183.6–––
−275.4–––
per 1 mol of
−550.9–––

Changes in standard condition (3)

Reaction of sodium sulfite and potassium permanganate
3Na2SO3Crystalline solid + 2KMnO4Crystalline solid
⟶
3Na2SO4Crystalline solidmetastable + 2MnO2Crystalline solid + K2OCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
––−116.2−16.0
per 1 mol of
––−38.73−5.33
––−58.10−8.00
per 1 mol of
––−38.73−5.33
––−58.10−8.00
per 1 mol of
––−116.2−16.0

Changes in standard condition (4)

Reaction of sodium sulfite and potassium permanganate
3Na2SO3Crystalline solid + 2KMnO4Crystalline solid
⟶
3Na2SO4Crystalline solidmetastable + 2MnO2Amorphous solidprecipitated + K2OCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
––––
per 1 mol of
––––
––––
per 1 mol of
––––
––––
per 1 mol of
––––

Changes in aqueous solution

Reaction of sodium sulfite and potassium permanganate
◆
ΔrG−565.3 kJ/mol
K1.09 × 1099
pK−99.04
3Na2SO3Ionized aqueous solution + 2KMnO4Ionized aqueous solution
⟶
3Na2SO4Ionized aqueous solution + 2MnO2Crystalline solid + K2OCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−634.9−565.3−236.6–
per 1 mol of
−211.6−188.4−78.87–
−317.4−282.6−118.3–
per 1 mol of
−211.6−188.4−78.87–
−317.4−282.6−118.3–
per 1 mol of
−634.9−565.3−236.6–

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Na2SO3 (cr)-1100.8[1]-1012.5[1]145.94[1]120.25[1]
Na2SO3 (ai)-1115.87[1]-1010.39[1]87.9[1]–
Na2SO3 (cr)
7 hydrate
-3162.3[1]-2676.1[1]444[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 formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
––154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[1]–
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[1]–––
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid, (g):Gas

References

List of references

  1. 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
    National Institute of Standards and Technology (NIST)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education