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(NH4)2SO3 + MnO2 → 2NH3↑ + MnSO4 + H2O

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Reaction of ammonium sulfite and manganese(IV) oxide
(NH4)2SO3Ammonium sulfite + MnO2Manganese(IV) oxide
⟶
2NH3↑Ammonia + MnSO4Manganese(II) sulfate + H2OWater

The reaction of ammonium sulfite and manganese(IV) oxide yields ammonia, manganese(II) sulfate, and water (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 ammonium sulfite and manganese(IV) oxide
(NH4)2SO3Ammonium sulfite + MnO2Manganese(IV) oxide
⟶
2NH3↑Ammonia + MnSO4Manganese(II) sulfate + H2OWater

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 ammonium sulfite and manganese(IV) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO3Ammonium sulfite1
Reducing
Reducing
MnO2Manganese(IV) oxide1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH3Ammonia2
–
–
MnSO4Manganese(II) sulfate1
Redoxed product
–
H2OWater1
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of ammonium sulfite and manganese(IV) oxide
(NH4)2SO3Crystalline solid + MnO2Crystalline solid
⟶
2NH3↑Gas + MnSO4Crystalline solid + H2OLiquid
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
−38.0–––
per 1 mol of
−38.0–––
−38.0–––
per 1 mol of
−19.0–––
−38.0–––
per 1 mol of
−38.0–––

Changes in standard condition (2)

Reaction of ammonium sulfite and manganese(IV) oxide
(NH4)2SO3Crystalline solid + MnO2Amorphous solidprecipitated
⟶
2NH3↑Gas + MnSO4Crystalline solid + H2OLiquid
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
−55.5–––
per 1 mol of
−55.5–––
−55.5–––
per 1 mol of
−27.8–––
−55.5–––
per 1 mol of
−55.5–––

Changes in aqueous solution (1)

Reaction of ammonium sulfite and manganese(IV) oxide
◆
ΔrG−145.6 kJ/mol
K3.22 × 1025
pK−25.51
(NH4)2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2NH3↑Gas + MnSO4Un-ionized aqueous solution + H2OLiquid
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
−73.5−145.6240.7–
per 1 mol of
−73.5−145.6240.7–
−73.5−145.6240.7–
per 1 mol of
−36.8−72.80120.3–
−73.5−145.6240.7–
per 1 mol of
−73.5−145.6240.7–

Changes in aqueous solution (2)

Reaction of ammonium sulfite and manganese(IV) oxide
◆
ΔrG−132.6 kJ/mol
K1.70 × 1023
pK−23.23
(NH4)2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2NH3↑Gas + MnSO4Ionized aqueous solution + H2OLiquid
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
−87.7−132.6150.7–
per 1 mol of
−87.7−132.6150.7–
−87.7−132.6150.7–
per 1 mol of
−43.9−66.3075.35–
−87.7−132.6150.7–
per 1 mol of
−87.7−132.6150.7–

Changes in aqueous solution (3)

Reaction of ammonium sulfite and manganese(IV) oxide
◆
ΔrG−145.6 kJ/mol
K3.22 × 1025
pK−25.51
(NH4)2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2NH3↑Gas + MnSO4Un-ionized aqueous solution + H2OLiquid
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
−73.5−145.6240.7–
per 1 mol of
−73.5−145.6240.7–
−73.5−145.6240.7–
per 1 mol of
−36.8−72.80120.3–
−73.5−145.6240.7–
per 1 mol of
−73.5−145.6240.7–

Changes in aqueous solution (4)

Reaction of ammonium sulfite and manganese(IV) oxide
◆
ΔrG−165.7 kJ/mol
K1.07 × 1029
pK−29.03
(NH4)2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2NH3↑Un-ionized aqueous solution + MnSO4Un-ionized aqueous solution + H2OLiquid
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
−141.9−165.778.4–
per 1 mol of
−141.9−165.778.4–
−141.9−165.778.4–
per 1 mol of
−70.95−82.8539.2–
−141.9−165.778.4–
per 1 mol of
−141.9−165.778.4–

Changes in aqueous solution (5)

Reaction of ammonium sulfite and manganese(IV) oxide
◆
ΔrG−152.7 kJ/mol
K5.65 × 1026
pK−26.75
(NH4)2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2NH3↑Un-ionized aqueous solution + MnSO4Ionized aqueous solution + H2OLiquid
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
−156.1−152.7−11.6–
per 1 mol of
−156.1−152.7−11.6–
−156.1−152.7−11.6–
per 1 mol of
−78.05−76.35−5.80–
−156.1−152.7−11.6–
per 1 mol of
−156.1−152.7−11.6–

Changes in aqueous solution (6)

Reaction of ammonium sulfite and manganese(IV) oxide
◆
ΔrG−165.7 kJ/mol
K1.07 × 1029
pK−29.03
(NH4)2SO3Ionized aqueous solution + MnO2Crystalline solid
⟶
2NH3↑Un-ionized aqueous solution + MnSO4Un-ionized aqueous solution + H2OLiquid
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
−141.9−165.778.4–
per 1 mol of
−141.9−165.778.4–
−141.9−165.778.4–
per 1 mol of
−70.95−82.8539.2–
−141.9−165.778.4–
per 1 mol of
−141.9−165.778.4–

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
(NH4)2SO3 (cr)-885.3[1]–––
(NH4)2SO3 (ai)-900.4[1]-645.0[1]197.5[1]–
(NH4)2SO3 (cr)
1 hydrate
-1187.4[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
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]–
MnSO4 (cr)-1065.25[1]-957.36[1]112.1[1]100.50[1]
MnSO4 (ai)-1130.1[1]-972.7[1]-53.6[1]-243[1]
MnSO4 (ao)-1115.9[1]-985.7[1]36.4[1]–
MnSO4 (cr)
1 hydrate
α
-1376.5[1]–––
MnSO4 (cr)
1 hydrate
β
-1348.1[1]–––
MnSO4 (cr)
4 hydrate
-2258.1[1]–––
MnSO4 (cr)
5 hydrate
-2553.1[1]––326[1]
MnSO4 (cr)
7 hydrate
-3139.3[1]–––
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid

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)