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5NH4ClO3 + 7KMnO4 → 5NO↑ + 5KClO4 + 7MnO + K2O + 10H2O

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Reaction of ammonium chlorate and potassium permanganate
5NH4ClO3Ammonium chlorate + 7KMnO4Potassium permanganate
⟶
5NO↑Nitrogen monoxide + 5KClO4Potassium perchlorate + 7MnOManganese(II) oxide + K2OPotassium oxide + 10H2OWater

The reaction of ammonium chlorate and potassium permanganate yields nitrogen monoxide, potassium perchlorate, manganese(II) oxide, potassium oxide, 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 chlorate and potassium permanganate
5NH4ClO3Ammonium chlorate + 7KMnO4Potassium permanganate
⟶
5NO↑Nitrogen monoxide + 5KClO4Potassium perchlorate + 7MnOManganese(II) oxide + K2OPotassium oxide + 10H2OWater

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 ammonium chlorate and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4ClO3Ammonium chlorate5
Reducing
Reducing
KMnO4Potassium permanganate7
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NONitrogen monoxide5
Oxidized
–
KClO4Potassium perchlorate5
Oxidized
–
MnOManganese(II) oxide7
Reduced
–
K2OPotassium oxide1
–
–
H2OWater10
–
–

Thermodynamic changes

Changes in aqueous solution

Reaction of ammonium chlorate and potassium permanganate
◆
ΔrG−710.1 kJ/mol
K2.54 × 10124
pK−124.40
5NH4ClO3Ionized aqueous solution + 7KMnO4Ionized aqueous solution
⟶
5NO↑Gas + 5KClO4Ionized aqueous solution + 7MnOCrystalline solid + K2OCrystalline solid + 10H2OLiquid
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
−634.6−710.1253.1–
per 1 mol of
−126.9−142.050.62–
−90.66−101.436.16–
per 1 mol of
−126.9−142.050.62–
−126.9−142.050.62–
−90.66−101.436.16–
per 1 mol of
−634.6−710.1253.1–
per 1 mol of
−63.46−71.0125.31–

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
NH4ClO3 (ai)-236.48[1]-87.26[1]275.7[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]
* (ai):Ionized aqueous solution, (cr):Crystalline 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
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
KClO4 (cr)-432.75[1]-303.09[1]151.0[1]112.38[1]
KClO4 (ai)-381.71[1]-291.79[1]284.5[1]–
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]–––
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[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, (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)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education