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  3. 5ZnI2 + 12KMnO4 + 36H^+ → 5Zn^2+ + 10KIO3 + 12Mn^2+ + 2K^+ + 18H2O

5ZnI2 + 12KMnO4 + 36H+ → 5Zn2+ + 10KIO3 + 12Mn2+ + 2K+ + 18H2O

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Reaction of zinc iodide and potassium permanganate under acidic condition
5ZnI2Zinc iodide + 12KMnO4Potassium permanganate + 36H+Hydrogen ion
⟶
5Zn2+Zinc ion + 10KIO3Potassium iodate + 12Mn2+Manganese(II) ion + 2K+Potassium ion + 18H2OWater

The reaction of zinc iodide, potassium permanganate, and hydrogen ion yields zinc ion, potassium iodate, manganese(II) ion, potassium ion, 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 zinc iodide and potassium permanganate under acidic condition
5ZnI2Zinc iodide + 12KMnO4Potassium permanganate + 36H+Hydrogen ion
⟶
5Zn2+Zinc ion + 10KIO3Potassium iodate + 12Mn2+Manganese(II) ion + 2K+Potassium ion + 18H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
⟶
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of zinc iodide and potassium permanganate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnI2Zinc iodide5
Reducing
Oxidizable
KMnO4Potassium permanganate12
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion36
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Zn2+Zinc ion5
–
–
KIO3Potassium iodate10
Oxidized
–
Mn2+Manganese(II) ion12
Reduced
–
K+Potassium ion2
–
–
H2OWater18
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc iodide and potassium permanganate under acidic condition
◆
ΔrG−2402.4 kJ/mol
K7.63 × 10420
pK−420.88
5ZnI2Ionized aqueous solution + 12KMnO4Ionized aqueous solution + 36H+Un-ionized aqueous solution
⟶
5Zn2+Un-ionized aqueous solution + 10KIO3Ionized aqueous solution + 12Mn2+Un-ionized aqueous solution + 2K+Un-ionized aqueous solution + 18H2OLiquid
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
−2957.3−2402.4−1848.2–
per 1 mol of
−591.46−480.48−369.64–
−246.44−200.20−154.02–
per 1 mol of
Hydrogen ion
−82.147−66.733−51.339–
per 1 mol of
Zinc ion
−591.46−480.48−369.64–
per 1 mol of
−295.73−240.24−184.82–
per 1 mol of
Manganese(II) ion
−246.44−200.20−154.02–
per 1 mol of
Potassium ion
−1478.7−1201.2−924.10–
per 1 mol of
−164.29−133.47−102.68–

Changes in standard condition (2)

Reaction of zinc iodide and potassium permanganate under acidic condition
◆
ΔrG−2450.4 kJ/mol
K1.96 × 10429
pK−429.29
5ZnI2Un-ionized aqueous solution + 12KMnO4Ionized aqueous solution + 36H+Un-ionized aqueous solution
⟶
5Zn2+Un-ionized aqueous solution + 10KIO3Ionized aqueous solution + 12Mn2+Un-ionized aqueous solution + 2K+Un-ionized aqueous solution + 18H2OLiquid
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
–−2450.4––
per 1 mol of
–−490.08––
–−204.20––
per 1 mol of
Hydrogen ion
–−68.067––
per 1 mol of
Zinc ion
–−490.08––
per 1 mol of
–−245.04––
per 1 mol of
Manganese(II) ion
–−204.20––
per 1 mol of
Potassium ion
–−1225.2––
per 1 mol of
–−136.13––

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]
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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
Zn2+ (g)2782.78[1]–––
Zn2+ (ao)-153.89[1]-147.06[1]-112.1[1]46[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]–
Mn2+ (g)2519.69[1]–––
Mn2+ (ao)-220.75[1]-228.1[1]-73.6[1]50[1]
K+ (g)514.26[1]–––
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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)