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6Na2SO3 + 2KMnO4 → 5Na2SO4 + Na2O + 2MnO + K2SO3

The reaction of sodium sulfite and potassium permanganate yields sodium sulfate, sodium oxide, manganese(II) oxide, and potassium sulfite (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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO3Sodium sulfite6
Reducing
Reducing
KMnO4Potassium permanganate2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate5
Oxidized
Na2OSodium oxide1
MnOManganese(II) oxide2
Reduced
K2SO3Potassium sulfite1

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium sulfite and potassium permanganate
6Na2SO3Crystalline solid + 2KMnO4Crystalline solid
5Na2SO4Crystalline solidorthorhombic + Na2OCrystalline solid + 2MnOCrystalline solid + K2SO3Crystalline 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
−966.4
per 1 mol of
−161.1
−483.2
per 1 mol of
−193.3
per 1 mol of
−966.4
−483.2
per 1 mol of
−966.4

Changes in standard condition (2)

Reaction of sodium sulfite and potassium permanganate
6Na2SO3Crystalline solid + 2KMnO4Crystalline solid
5Na2SO4Crystalline solidmetastable + Na2OCrystalline solid + 2MnOCrystalline solid + K2SO3Crystalline 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
per 1 mol of

Changes in aqueous solution

Reaction of sodium sulfite and potassium permanganate
ΔrG−972.8 kJ/mol
K2.67 × 10170
pK−170.43
6Na2SO3Ionized aqueous solution + 2KMnO4Ionized aqueous solution
5Na2SO4Ionized aqueous solution + Na2OCrystalline solid + 2MnOCrystalline solid + K2SO3Ionized aqueous solution
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
−989.5−972.8−54
per 1 mol of
−164.9−162.1−9.0
−494.8−486.4−27
per 1 mol of
−197.9−194.6−11
per 1 mol of
−989.5−972.8−54
−494.8−486.4−27
per 1 mol of
−989.5−972.8−54

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]
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[1]
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]
K2SO3 (cr)-1125.5[1]
K2SO3 (ai)-1140.1[1]-1053.1[1]176[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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)