15FeI2 + 2KMnO4 + 16H+ → 10FeI3 + 2Mn2+ + 2K+ + 8H2O + 5Fe2+
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- Reaction of iron(II) iodide and potassium permanganate under acidic condition
- 15FeI2Iron(II) iodide + 2KMnO4Potassium permanganate + 16H+Hydrogen ion10FeI3Iron(III) iodide + 2Mn2+Manganese(II) ion + 2K+Potassium ion + 8H2OWater + 5Fe2+Iron(II) ion⟶
The reaction of iron(II) iodide, potassium permanganate, and hydrogen ion yields iron(III) iodide, manganese(II) ion, potassium ion, water, and iron(II) ion (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 iron(II) iodide and potassium permanganate under acidic condition
- 15FeI2Iron(II) iodide + 2KMnO4Potassium permanganate + 16H+Hydrogen ion10FeI3Iron(III) iodide + 2Mn2+Manganese(II) ion + 2K+Potassium ion + 8H2OWater + 5Fe2+Iron(II) ion⟶
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 iron(II) iodide and potassium permanganate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeI2 | Iron(II) iodide | 15 | 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 |
|---|---|---|---|---|
| FeI3 | Iron(III) iodide | 10 | Oxidized | – |
| Mn2+ | Manganese(II) ion | 2 | Reduced | – |
| K+ | Potassium ion | 2 | – | – |
| H2O | Water | 8 | – | Water |
| Fe2+ | Iron(II) ion | 5 | – | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of iron(II) iodide and potassium permanganate under acidic condition◆
ΔrG −716.5 kJ/mol K 3.35 × 10125 pK −125.53
| 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 | −1238.8 | −716.5 | −1752.3 | – |
per 1 mol of | −82.587 | −47.77 | −116.82 | – |
per 1 mol of | −619.40 | −358.3 | −876.15 | – |
per 1 mol of Hydrogen ion | −77.425 | −44.78 | −109.52 | – |
per 1 mol of | −123.88 | −71.65 | −175.23 | – |
per 1 mol of Manganese(II) ion | −619.40 | −358.3 | −876.15 | – |
per 1 mol of Potassium ion | −619.40 | −358.3 | −876.15 | – |
per 1 mol of | −154.85 | −89.56 | −219.04 | – |
per 1 mol of Iron(II) ion | −247.76 | −143.3 | −350.46 | – |
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 |
|---|---|---|---|---|
| FeI2 (cr) | -113.0[1] | – | – | – |
| FeI2 (g) | 60.7[1] | – | – | – |
| FeI2 (ai) | -199.6[1] | -182.05[1] | 84.9[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, (g):Gas, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| FeI3 (g) | 71[1] | – | – | – |
| FeI3 (ai) | -214.2[1] | -159.4[1] | 18.0[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] |
| Fe2+ (g) | 2749.93[1] | – | – | – |
| Fe2+ (ao) | -89.1[1] | -78.90[1] | -137.7[1] | – |
* (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline 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°, -113.0 kJ · mol−1
- ^ ΔfH°, 60.7 kJ · mol−1
- ^ ΔfH°, -199.6 kJ · mol−1
- ^ ΔfG°, -182.05 kJ · mol−1
- ^ S°, 84.9 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°, 71. kJ · mol−1
- ^ ΔfH°, -214.2 kJ · mol−1
- ^ ΔfG°, -159.4 kJ · mol−1
- ^ S°, 18.0 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
- ^ ΔfH°, 2749.93 kJ · mol−1
- ^ ΔfH°, -89.1 kJ · mol−1
- ^ ΔfG°, -78.90 kJ · mol−1
- ^ S°, -137.7 J · K−1 · mol−1