5CuCl + 2KMnO4 + 12H+ → 5Cu2+ + ClO2↑ + 2MnCl2 + 2K+ + 6H2O
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- Reaction of copper(I) chloride and potassium permanganate under acidic condition
- 5CuClCopper(I) chloride + 2KMnO4Potassium permanganate + 12H+Hydrogen ion5Cu2+Copper(II) ion + ClO2↑Chlorine dioxide + 2MnCl2Manganese(II) chloride + 2K+Potassium ion + 6H2OWater⟶
The reaction of copper(I) chloride, potassium permanganate, and hydrogen ion yields copper(II) ion, chlorine dioxide, manganese(II) chloride, 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) chloride and potassium permanganate under acidic condition
- 5CuClCopper(I) chloride + 2KMnO4Potassium permanganate + 12H+Hydrogen ion5Cu2+Copper(II) ion + ClO2↑Chlorine dioxide + 2MnCl2Manganese(II) chloride + 2K+Potassium ion + 6H2OWater⟶
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) chloride and potassium permanganate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuCl | Copper(I) chloride | 5 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 12 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cu2+ | Copper(II) ion | 5 | Oxidized | – |
| ClO2 | Chlorine dioxide | 1 | Oxidized | – |
| MnCl2 | Manganese(II) chloride | 2 | Reduced | – |
| K+ | Potassium ion | 2 | – | – |
| H2O | Water | 6 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of copper(I) chloride and potassium permanganate under acidic condition◆
ΔrG −462.7 kJ/mol K 1.15 × 1081 pK −81.06
| 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 | −629.9 | −462.7 | −557.3 | – |
per 1 mol of | −126.0 | −92.54 | −111.5 | – |
per 1 mol of | −314.9 | −231.3 | −278.6 | – |
per 1 mol of Hydrogen ion | −52.49 | −38.56 | −46.44 | – |
per 1 mol of Copper(II) ion | −126.0 | −92.54 | −111.5 | – |
per 1 mol of | −629.9 | −462.7 | −557.3 | – |
per 1 mol of | −314.9 | −231.3 | −278.6 | – |
per 1 mol of Potassium ion | −314.9 | −231.3 | −278.6 | – |
per 1 mol of | −105.0 | −77.12 | −92.88 | – |
Changes in standard condition (2)
- Reaction of copper(I) chloride and potassium permanganate under acidic condition◆
ΔrG −465.1 kJ/mol K 3.03 × 1081 pK −81.48
| 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 | – | −465.1 | – | – |
per 1 mol of | – | −93.02 | – | – |
per 1 mol of | – | −232.6 | – | – |
per 1 mol of Hydrogen ion | – | −38.76 | – | – |
per 1 mol of Copper(II) ion | – | −93.02 | – | – |
per 1 mol of | – | −465.1 | – | – |
per 1 mol of | – | −232.6 | – | – |
per 1 mol of Potassium ion | – | −232.6 | – | – |
per 1 mol of | – | −77.52 | – | – |
Changes in standard condition (3)
- Reaction of copper(I) chloride and potassium permanganate under acidic condition◆
ΔrG −463.1 kJ/mol K 1.35 × 1081 pK −81.13
| 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 | −657.5 | −463.1 | −649.3 | – |
per 1 mol of | −131.5 | −92.62 | −129.9 | – |
per 1 mol of | −328.8 | −231.6 | −324.6 | – |
per 1 mol of Hydrogen ion | −54.79 | −38.59 | −54.11 | – |
per 1 mol of Copper(II) ion | −131.5 | −92.62 | −129.9 | – |
per 1 mol of | −657.5 | −463.1 | −649.3 | – |
per 1 mol of | −328.8 | −231.6 | −324.6 | – |
per 1 mol of Potassium ion | −328.8 | −231.6 | −324.6 | – |
per 1 mol of | −109.6 | −77.18 | −108.2 | – |
Changes in standard condition (4)
- Reaction of copper(I) chloride and potassium permanganate under acidic condition◆
ΔrG −465.5 kJ/mol K 3.57 × 1081 pK −81.55
| 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 | – | −465.5 | – | – |
per 1 mol of | – | −93.10 | – | – |
per 1 mol of | – | −232.8 | – | – |
per 1 mol of Hydrogen ion | – | −38.79 | – | – |
per 1 mol of Copper(II) ion | – | −93.10 | – | – |
per 1 mol of | – | −465.5 | – | – |
per 1 mol of | – | −232.8 | – | – |
per 1 mol of Potassium ion | – | −232.8 | – | – |
per 1 mol of | – | −77.58 | – | – |
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 |
|---|---|---|---|---|
| CuCl (cr) | -137.2[1] | -119.86[1] | 86.2[1] | 48.5[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] | – |
| ClO2 (g) | 102.5[1] | 120.5[1] | 256.84[1] | 41.97[1] |
| ClO2 (ao) | 74.9[1] | 120.1[1] | 164.8[1] | – |
| MnCl2 (cr) | -481.29[1] | -440.50[1] | 118.24[1] | 72.93[1] |
| MnCl2 (g) | -263.6[1] | – | – | – |
| MnCl2 (ai) | -555.05[1] | -490.8[1] | 38.9[1] | -222[1] |
| MnCl2 (ao) | – | -492.0[1] | – | – |
| MnCl2 (cr) 1 hydrate | -789.9[1] | -696.1[1] | 174.1[1] | – |
| MnCl2 (cr) 2 hydrate | -1092.0[1] | -942.1[1] | 218.8[1] | – |
| MnCl2 (cr) 4 hydrate | -1687.4[1] | -1423.6[1] | 303.3[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, (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°, -137.2 kJ · mol−1
- ^ ΔfG°, -119.86 kJ · mol−1
- ^ S°, 86.2 J · K−1 · mol−1
- ^ Cp°, 48.5 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°, 102.5 kJ · mol−1
- ^ ΔfG°, 120.5 kJ · mol−1
- ^ S°, 256.84 J · K−1 · mol−1
- ^ Cp°, 41.97 J · K−1 · mol−1
- ^ ΔfH°, 74.9 kJ · mol−1
- ^ ΔfG°, 120.1 kJ · mol−1
- ^ S°, 164.8 J · K−1 · mol−1
- ^ ΔfH°, -481.29 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 118.24 J · K−1 · mol−1
- ^ Cp°, 72.93 J · K−1 · mol−1
- ^ ΔfH°, -263.6 kJ · mol−1
- ^ ΔfH°, -555.05 kJ · mol−1
- ^ ΔfG°, -490.8 kJ · mol−1
- ^ S°, 38.9 J · K−1 · mol−1
- ^ Cp°, -222. J · K−1 · mol−1
- ^ ΔfG°, -492.0 kJ · mol−1
- ^ ΔfH°, -789.9 kJ · mol−1
- ^ ΔfG°, -696.1 kJ · mol−1
- ^ S°, 174.1 J · K−1 · mol−1
- ^ ΔfH°, -1092.0 kJ · mol−1
- ^ ΔfG°, -942.1 kJ · mol−1
- ^ S°, 218.8 J · K−1 · mol−1
- ^ ΔfH°, -1687.4 kJ · mol−1
- ^ ΔfG°, -1423.6 kJ · mol−1
- ^ S°, 303.3 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