3CuI + KMnO4 + 7H+ → 3Cu2+ + MnO2 + 3HI↑ + K+ + 2H2O
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- Reaction of copper(I) iodide and potassium permanganate under acidic condition
- 3CuICopper(I) iodide + KMnO4Potassium permanganate + 7H+Hydrogen ion3Cu2+Copper(II) ion + MnO2Manganese(IV) oxide + 3HI↑Hydrogen 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
Reaction data
Chemical equation
- Reaction of copper(I) iodide and potassium permanganate under acidic condition
- 3CuICopper(I) iodide + KMnO4Potassium permanganate + 7H+Hydrogen ion3Cu2+Copper(II) ion + MnO2Manganese(IV) oxide + 3HI↑Hydrogen 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 formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CuI | Copper(I) iodide | 3 | Reducing | Oxidizable |
KMnO4 | Potassium permanganate | 1 | Oxidizing | Oxidizing under acidic condition |
H+ | Hydrogen ion | 7 | – | Hydrogen ion |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Cu2+ | Copper(II) ion | 3 | Oxidized | – |
MnO2 | Manganese(IV) oxide | 1 | Reduced | – |
HI | Hydrogen iodide | 3 | – | – |
K+ | Potassium ion | 1 | – | – |
H2O | Water | 2 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of copper(I) iodide and potassium permanganate under acidic condition◆
ΔrG −82.1 kJ/mol K 2.42 × 1014 pK −14.38
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 | −82.1 | 32.6 | – |
per 1 mol of | −24.4 | −27.4 | 10.9 | – |
per 1 mol of | −73.1 | −82.1 | 32.6 | – |
per 1 mol of Hydrogen ion | −10.4 | −11.7 | 4.66 | – |
per 1 mol of Copper(II) ion | −24.4 | −27.4 | 10.9 | – |
per 1 mol of | −73.1 | −82.1 | 32.6 | – |
per 1 mol of | −24.4 | −27.4 | 10.9 | – |
per 1 mol of Potassium ion | −73.1 | −82.1 | 32.6 | – |
per 1 mol of | −36.5 | −41.0 | 16.3 | – |
Changes in standard condition (2)
- Reaction of copper(I) iodide and potassium permanganate under acidic condition◆
ΔrG −241.9 kJ/mol K 2.39 × 1042 pK −42.38
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 | – |
per 1 mol of | −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 | – |
per 1 mol of | −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 formula | Standard 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 formula | Standard 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
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -67.8 kJ · mol−1
- ^ ΔfG°, -69.5 kJ · mol−1
- ^ S°, 96.7 J · K−1 · mol−1
- ^ Cp°, 54.06 J · K−1 · mol−1
- ^ ΔfH°, -837.2 kJ · mol−1
- ^ ΔfG°, -737.6 kJ · mol−1
- ^ S°, 171.71 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -793.8 kJ · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ S°, 293.7 J · K−1 · mol−1
- ^ Cp°, -60.2 J · K−1 · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, 3054.07 kJ · mol−1
- ^ ΔfH°, 64.77 kJ · mol−1
- ^ ΔfG°, 65.49 kJ · mol−1
- ^ S°, -99.6 J · K−1 · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · mol−1
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1
- ^ ΔfH°, 514.26 kJ · mol−1
- ^ ΔfH°, -252.38 kJ · mol−1
- ^ ΔfG°, -283.27 kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 21.8 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1