3CuI + 7KMnO4 + 13H+ → 3Cu2+ + 3HIO3 + 7MnO2 + 7K+ + 5H2O
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- Reaction of copper(I) iodide and potassium permanganate under acidic condition
- 3CuICopper(I) iodide + 7KMnO4Potassium permanganate + 13H+Hydrogen ion3Cu2+Copper(II) ion + 3HIO3Iodic acid + 7MnO2Manganese(IV) oxide + 7K+Potassium ion + 5H2OWater⟶
The reaction of copper(I) iodide, potassium permanganate, and hydrogen ion yields copper(II) ion, iodic acid, manganese(IV) oxide, 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 + 7KMnO4Potassium permanganate + 13H+Hydrogen ion3Cu2+Copper(II) ion + 3HIO3Iodic acid + 7MnO2Manganese(IV) oxide + 7K+Potassium ion + 5H2OWater⟶
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 | 7 | Oxidizing | Oxidizing under acidic condition |
H+ | Hydrogen ion | 13 | – | Hydrogen ion |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Cu2+ | Copper(II) ion | 3 | Oxidized | – |
HIO3 | Iodic acid | 3 | Oxidized | – |
MnO2 | Manganese(IV) oxide | 7 | Reduced | – |
K+ | Potassium ion | 7 | – | – |
H2O | Water | 5 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of copper(I) iodide and potassium permanganate under acidic condition◆
ΔrG −1303.8 kJ/mol K 2.61 × 10228 pK −228.42
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 | −1515.6 | −1303.8 | −705.7 | – |
per 1 mol of | −505.20 | −434.60 | −235.2 | – |
per 1 mol of | −216.51 | −186.26 | −100.8 | – |
per 1 mol of Hydrogen ion | −116.58 | −100.29 | −54.28 | – |
per 1 mol of Copper(II) ion | −505.20 | −434.60 | −235.2 | – |
per 1 mol of | −505.20 | −434.60 | −235.2 | – |
per 1 mol of | −216.51 | −186.26 | −100.8 | – |
per 1 mol of Potassium ion | −216.51 | −186.26 | −100.8 | – |
per 1 mol of | −303.12 | −260.76 | −141.1 | – |
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] | – |
HIO3 (cr) | -230.1[1] | – | – | – |
HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
MnO2 (am) precipitated | -502.5[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, (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°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 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°, 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