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2K2SO3 + MnO2 → 2K2SO4 + Mn

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Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Potassium sulfite + MnO2Manganese(IV) oxide
⟶
2K2SO4Potassium sulfate + MnManganese

The reaction of potassium sulfite and manganese(IV) oxide yields potassium sulfate and manganese (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 potassium sulfite and manganese(IV) oxide
2K2SO3Potassium sulfite + MnO2Manganese(IV) oxide
⟶
2K2SO4Potassium sulfate + MnManganese

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium sulfite and manganese(IV) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K2SO3Potassium sulfite2
Reducing
Reducing
MnO2Manganese(IV) oxide1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate2
Oxidized
–
MnManganese1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Crystalline solid + MnO2Crystalline solid
⟶
2K2SO4Crystalline solid + MnCrystalline solidα
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
−104.6–––
per 1 mol of
−52.30–––
−104.6–––
per 1 mol of
−52.30–––
per 1 mol of
−104.6–––

Changes in standard condition (2)

Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Crystalline solid + MnO2Crystalline solid
⟶
2K2SO4Crystalline solid + MnCrystalline solidβ
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 standard condition (3)

Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Crystalline solid + MnO2Crystalline solid
⟶
2K2SO4Crystalline solid + MnCrystalline solidγ
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
−103.0–––
per 1 mol of
−51.50–––
−103.0–––
per 1 mol of
−51.50–––
per 1 mol of
−103.0–––

Changes in standard condition (4)

Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Crystalline solid + MnO2Amorphous solidprecipitated
⟶
2K2SO4Crystalline solid + MnCrystalline solidα
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
−122.1–––
per 1 mol of
−61.05–––
−122.1–––
per 1 mol of
−61.05–––
per 1 mol of
−122.1–––

Changes in standard condition (5)

Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Crystalline solid + MnO2Amorphous solidprecipitated
⟶
2K2SO4Crystalline solid + MnCrystalline solidβ
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 standard condition (6)

Reaction of potassium sulfite and manganese(IV) oxide
2K2SO3Crystalline solid + MnO2Amorphous solidprecipitated
⟶
2K2SO4Crystalline solid + MnCrystalline solidγ
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
−120.5–––
per 1 mol of
−60.25–––
−120.5–––
per 1 mol of
−60.25–––
per 1 mol of
−120.5–––

Changes in aqueous solution

Reaction of potassium sulfite and manganese(IV) oxide
◆
ΔrG−50.8 kJ/mol
K7.94 × 108
pK−8.90
2K2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2K2SO4Ionized aqueous solution + MnCrystalline solidα
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
−27.8−50.877–
per 1 mol of
−13.9−25.439–
−27.8−50.877–
per 1 mol of
−13.9−25.439–
per 1 mol of
−27.8−50.877–

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
K2SO3 (cr)-1125.5[1]–––
K2SO3 (ai)-1140.1[1]-1053.1[1]176[1]–
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[1]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid

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
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]
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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

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)