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ZnI2 + 4KMnO4 + H2O → ZnO + 2KIO3 + 4MnO2 + 2KOH

The reaction of zinc iodide, potassium permanganate, and water yields zinc oxide, potassium iodate, manganese(IV) oxide, and potassium hydroxide (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 oxidizable species and oxidizing species under neutral condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of zinc iodide and potassium permanganate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnI2Zinc iodide1
Reducing
Oxidizable
KMnO4Potassium permanganate4
Oxidizing
Oxidizing
H2OWater1
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnOZinc oxide1
KIO3Potassium iodate2
Oxidized
MnO2Manganese(IV) oxide4
Reduced
KOHPotassium hydroxide2

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc iodide and potassium permanganate under neutral condition
ΔrG−377.2 kJ/mol
K1.21 × 1066
pK−66.08
ZnI2Crystalline solid + 4KMnO4Crystalline solid + H2OLiquid
ZnOCrystalline solid + 2KIO3Crystalline solid + 4MnO2Crystalline solid + 2KOHCrystalline 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
−438.0−377.2−201.3
per 1 mol of
−438.0−377.2−201.3
−109.5−94.30−50.33
per 1 mol of
−438.0−377.2−201.3
per 1 mol of
−438.0−377.2−201.3
per 1 mol of
−219.0−188.6−100.7
−109.5−94.30−50.33
−219.0−188.6−100.7

Changes in standard condition (2)

Reaction of zinc iodide and potassium permanganate under neutral condition
ZnI2Crystalline solid + 4KMnO4Crystalline solid + H2OLiquid
ZnOCrystalline solid + 2KIO3Crystalline solid + 4MnO2Amorphous solidprecipitated + 2KOHCrystalline 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
−367.9
per 1 mol of
−367.9
−91.97
per 1 mol of
−367.9
per 1 mol of
−367.9
per 1 mol of
−183.9
−91.97
−183.9

Changes in aqueous solution (1)

Reaction of zinc iodide and potassium permanganate under neutral condition
ΔrG−472.9 kJ/mol
K7.05 × 1082
pK−82.85
ZnI2Ionized aqueous solution + 4KMnO4Ionized aqueous solution + H2OLiquid
ZnOCrystalline solid + 2KIO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized 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
−615.1−472.9−474.4
per 1 mol of
−615.1−472.9−474.4
−153.8−118.2−118.6
per 1 mol of
−615.1−472.9−474.4
per 1 mol of
−615.1−472.9−474.4
per 1 mol of
−307.6−236.4−237.2
−153.8−118.2−118.6
−307.6−236.4−237.2

Changes in aqueous solution (2)

Reaction of zinc iodide and potassium permanganate under neutral condition
ΔrG−482.5 kJ/mol
K3.39 × 1084
pK−84.53
ZnI2Un-ionized aqueous solution + 4KMnO4Ionized aqueous solution + H2OLiquid
ZnOCrystalline solid + 2KIO3Ionized aqueous solution + 4MnO2Crystalline solid + 2KOHIonized 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
−482.5
per 1 mol of
−482.5
−120.6
per 1 mol of
−482.5
per 1 mol of
−482.5
per 1 mol of
−241.3
−120.6
−241.3

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
ZnI2 (cr)-208.03[1]-208.95[1]161.1[1]
ZnI2 (ai)-264.26[1]-250.20[1]110.5[1]-238[1]
ZnI2 (ao)-240.6[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]
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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas

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
ZnO (cr)-348.28[1]-318.30[1]43.64[1]40.25[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]
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[1]
KOH (cr)-424.764[1]-379.08[1]78.9[1]64.9[1]
KOH (g)-231.0[1]-232.6[1]238.3[1]49.20[1]
KOH (ai)-482.37[1]-440.50[1]91.6[1]-126.8[1]
KOH (cr)
1 hydrate
-748.9[1]-645.1[1]117.2[1]
KOH (cr)
2 hydrate
-1051.0[1]-887.3[1]150.6[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid, (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)