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  3. 6NH4I + 6KMnO4 → 6NH3↑ + 5KIO3 + 3Mn(OH)2 + 3MnO + KI

6NH4I + 6KMnO4 → 6NH3↑ + 5KIO3 + 3Mn(OH)2 + 3MnO + KI

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Reaction of ammonium iodide and potassium permanganate
6NH4IAmmonium iodide + 6KMnO4Potassium permanganate
⟶
6NH3↑Ammonia + 5KIO3Potassium iodate + 3Mn(OH)2Manganese(II) hydroxide + 3MnOManganese(II) oxide + KIPotassium iodide

The reaction of ammonium iodide and potassium permanganate yields ammonia, potassium iodate, manganese(II) hydroxide, manganese(II) oxide, and potassium iodide (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 iodide and potassium permanganate
6NH4IAmmonium iodide + 6KMnO4Potassium permanganate
⟶
6NH3↑Ammonia + 5KIO3Potassium iodate + 3Mn(OH)2Manganese(II) hydroxide + 3MnOManganese(II) oxide + KIPotassium iodide

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 iodide and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4IAmmonium iodide6
Reducing
Reducing
KMnO4Potassium permanganate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH3Ammonia6
–
–
KIO3Potassium iodate5
Oxidized
–
Mn(OH)2Manganese(II) hydroxide3
Reduced
–
MnOManganese(II) oxide3
Reduced
–
KIPotassium iodide1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium iodide and potassium permanganate
◆
ΔrG−348.4 kJ/mol
K1.09 × 1061
pK−61.04
6NH4ICrystalline solid + 6KMnO4Crystalline solid
⟶
6NH3↑Gas + 5KIO3Crystalline solid + 3Mn(OH)2Amorphous solidprecipitated + 3MnOCrystalline solid + KICrystalline 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
−121.6−348.4763–
per 1 mol of
−20.27−58.07127–
−20.27−58.07127–
per 1 mol of
−20.27−58.07127–
per 1 mol of
−24.32−69.68153–
−40.53−116.1254–
−40.53−116.1254–
per 1 mol of
−121.6−348.4763–

Changes in aqueous solution (1)

Reaction of ammonium iodide and potassium permanganate
◆
ΔrG−255.0 kJ/mol
K4.72 × 1044
pK−44.67
6NH4IIonized aqueous solution + 6KMnO4Ionized aqueous solution
⟶
6NH3↑Gas + 5KIO3Ionized aqueous solution + 3Mn(OH)2Amorphous solidprecipitated + 3MnOCrystalline solid + KIIonized 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
−305.1−255.0−160.7–
per 1 mol of
−50.85−42.50−26.78–
−50.85−42.50−26.78–
per 1 mol of
−50.85−42.50−26.78–
per 1 mol of
−61.02−51.00−32.14–
−101.7−85.00−53.57–
−101.7−85.00−53.57–
per 1 mol of
−305.1−255.0−160.7–

Changes in aqueous solution (2)

Reaction of ammonium iodide and potassium permanganate
◆
ΔrG−315.3 kJ/mol
K1.73 × 1055
pK−55.24
6NH4IIonized aqueous solution + 6KMnO4Ionized aqueous solution
⟶
6NH3↑Un-ionized aqueous solution + 5KIO3Ionized aqueous solution + 3Mn(OH)2Amorphous solidprecipitated + 3MnOCrystalline solid + KIIonized 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
−510.2−315.3−647.6–
per 1 mol of
−85.03−52.55−107.9–
−85.03−52.55−107.9–
per 1 mol of
−85.03−52.55−107.9–
per 1 mol of
−102.0−63.06−129.5–
−170.1−105.1−215.9–
−170.1−105.1−215.9–
per 1 mol of
−510.2−315.3−647.6–

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
NH4I (cr)-201.42[1]-112.5[1]117[1]–
NH4I (ai)-187.69[1]-130.88[1]224.7[1]-62.3[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
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]–
KIO3 (cr)-501.37[1]-418.35[1]151.46[1]106.48[1]
KIO3 (ai)-473.6[1]-411.2[1]220.9[1]–
Mn(OH)2 (am)
precipitated
-695.4[1]-615.0[1]99.2[1]–
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]–––
KI (cr)-327.900[1]-324.892[1]106.32[1]52.93[1]
KI (g)-125.5[1]-166.1[1]258.3[1]37.11[1]
KI (ai)-307.57[1]-334.85[1]213.8[1]-120.5[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid

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)