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3CuI + KMnO4 + 7H+ → 3Cu2+ + MnO2 + 3HI↑ + K+ + 2H2O

Reaction of copper(I) iodide and potassium permanganate under acidic condition
3CuICopper(I) iodide + KMnO4Potassium permanganate + 7H+Hydrogen ion
3Cu2+Copper(II) ion + MnO2Manganese(IV) oxide + 3HIHydrogen iodide + K+Potassium ion + 2H2OWater

The reaction of copper(I) iodide, potassium permanganate, and hydrogen ion yields copper(II) ion, manganese(IV) oxide, hydrogen iodide, 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 copper(I) iodide and potassium permanganate under acidic condition
3CuICopper(I) iodide + KMnO4Potassium permanganate + 7H+Hydrogen ion
3Cu2+Copper(II) ion + MnO2Manganese(IV) oxide + 3HIHydrogen iodide + K+Potassium ion + 2H2OWater

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 copper(I) iodide and potassium permanganate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuICopper(I) iodide3
Reducing
Oxidizable
KMnO4Potassium permanganate1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion7
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2+Copper(II) ion3
Oxidized
MnO2Manganese(IV) oxide1
Reduced
HIHydrogen iodide3
K+Potassium ion1
H2OWater2
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper(I) iodide and potassium permanganate under acidic condition
ΔrG−82.1 kJ/mol
K2.42 × 1014
pK−14.38
3CuICrystalline solid + KMnO4Ionized aqueous solution + 7H+Un-ionized aqueous solution
3Cu2+Un-ionized aqueous solution + MnO2Crystalline solid + 3HIGas + K+Un-ionized aqueous solution + 2H2OLiquid
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
−73.1−82.132.6
per 1 mol of
−24.4−27.410.9
−73.1−82.132.6
per 1 mol of
Hydrogen ion
−10.4−11.74.66
per 1 mol of
Copper(II) ion
−24.4−27.410.9
−73.1−82.132.6
per 1 mol of
−24.4−27.410.9
per 1 mol of
Potassium ion
−73.1−82.132.6
per 1 mol of
−36.5−41.016.3

Changes in standard condition (2)

Reaction of copper(I) iodide and potassium permanganate under acidic condition
ΔrG−241.9 kJ/mol
K2.39 × 1042
pK−42.38
3CuICrystalline solid + KMnO4Ionized aqueous solution + 7H+Un-ionized aqueous solution
3Cu2+Un-ionized aqueous solution + MnO2Crystalline solid + 3HIIonized aqueous solution + K+Un-ionized aqueous solution + 2H2OLiquid
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
−318.1−241.9−253.3
per 1 mol of
−106.0−80.63−84.43
−318.1−241.9−253.3
per 1 mol of
Hydrogen ion
−45.44−34.56−36.19
per 1 mol of
Copper(II) ion
−106.0−80.63−84.43
−318.1−241.9−253.3
per 1 mol of
−106.0−80.63−84.43
per 1 mol of
Potassium ion
−318.1−241.9−253.3
per 1 mol of
−159.1−121.0−126.7

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
CuI (cr)-67.8[1]-69.5[1]96.7[1]54.06[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, (g):Gas, (ao):Un-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
Cu2+ (g)3054.07[1]
Cu2+ (ao)64.77[1]65.49[1]-99.6[1]
MnO2 (cr)-520.03[1]-465.14[1]53.05[1]54.14[1]
MnO2 (am)
precipitated
-502.5[1]
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[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, (am):Amorphous 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)