10CuF + 2KMnO4 + 16H+ → 5CuF2 + 5Cu2+ + 2Mn2+ + 2K+ + 8H2O
Last updated:
- Reaction of copper(I) fluoride and potassium permanganate under acidic condition
- 10CuFCopper(I) fluoride + 2KMnO4Potassium permanganate + 16H+Hydrogen ion5CuF2Copper(II) fluoride + 5Cu2+Copper(II) ion + 2Mn2+Manganese(II) ion + 2K+Potassium ion + 8H2OWater⟶
The reaction of copper(I) fluoride, potassium permanganate, and hydrogen ion yields copper(II) fluoride, copper(II) ion, 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
Reaction data
Chemical equation
- Reaction of copper(I) fluoride and potassium permanganate under acidic condition
- 10CuFCopper(I) fluoride + 2KMnO4Potassium permanganate + 16H+Hydrogen ion5CuF2Copper(II) fluoride + 5Cu2+Copper(II) ion + 2Mn2+Manganese(II) ion + 2K+Potassium ion + 8H2OWater⟶
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) fluoride and potassium permanganate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuF | Copper(I) fluoride | 10 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 16 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuF2 | Copper(II) fluoride | 5 | Oxidized | – |
| Cu2+ | Copper(II) ion | 5 | Oxidized | – |
| Mn2+ | Manganese(II) ion | 2 | Reduced | – |
| K+ | Potassium ion | 2 | – | – |
| H2O | Water | 8 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of copper(I) fluoride and potassium permanganate under acidic condition
| 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 | −1235 | – | – | – |
per 1 mol of | −123.5 | – | – | – |
per 1 mol of | −617.5 | – | – | – |
per 1 mol of Hydrogen ion | −77.19 | – | – | – |
per 1 mol of | −247.0 | – | – | – |
per 1 mol of Copper(II) ion | −247.0 | – | – | – |
per 1 mol of Manganese(II) ion | −617.5 | – | – | – |
per 1 mol of Potassium ion | −617.5 | – | – | – |
per 1 mol of | −154.4 | – | – | – |
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 |
|---|---|---|---|---|
| CuF (s) | -280 | -260 | 64.9 | – |
| 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] |
* (s):Solid, (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 |
|---|---|---|---|---|
| CuF2 (cr) | -542.7[1] | – | – | – |
| CuF2 (cr) 2 hydrate | – | -981.4[1] | – | – |
| Cu2+ (g) | 3054.07[1] | – | – | – |
| Cu2+ (ao) | 64.77[1] | 65.49[1] | -99.6[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] |
* (cr):Crystalline solid, (g):Gas, (ao):Un-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°, -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°, -542.7 kJ · mol−1
- ^ ΔfG°, -981.4 kJ · 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°, 2519.69 kJ · mol−1
- ^ ΔfH°, -220.75 kJ · mol−1
- ^ ΔfG°, -228.1 kJ · mol−1
- ^ S°, -73.6 J · K−1 · mol−1
- ^ Cp°, 50. 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