9FeCl2 + 5KMnO4 + 32H+ → 9Fe3+ + 8HClO + 5MnCl2 + 5K+ + 12H2O
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- Reaction of iron(II) chloride and potassium permanganate under acidic condition
- 9FeCl2Iron(II) chloride + 5KMnO4Potassium permanganate + 32H+Hydrogen ion9Fe3+Iron(III) ion + 8HClOHypochlorous acid + 5MnCl2Manganese(II) chloride + 5K+Potassium ion + 12H2OWater⟶
The reaction of iron(II) chloride, potassium permanganate, and hydrogen ion yields iron(III) ion, hypochlorous acid, 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 iron(II) chloride and potassium permanganate under acidic condition
- 9FeCl2Iron(II) chloride + 5KMnO4Potassium permanganate + 32H+Hydrogen ion9Fe3+Iron(III) ion + 8HClOHypochlorous acid + 5MnCl2Manganese(II) chloride + 5K+Potassium ion + 12H2OWater⟶
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) chloride and potassium permanganate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCl2 | Iron(II) chloride | 9 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 5 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 32 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3+ | Iron(III) ion | 9 | Oxidized | – |
| HClO | Hypochlorous acid | 8 | Oxidized | – |
| MnCl2 | Manganese(II) chloride | 5 | Reduced | – |
| K+ | Potassium ion | 5 | – | – |
| H2O | Water | 12 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) chloride and potassium permanganate under acidic condition◆
ΔrG −1233.0 kJ/mol K 1.03 × 10216 pK −216.01
| 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 | – | −1233.0 | – | – |
per 1 mol of | – | −137.00 | – | – |
per 1 mol of | – | −246.60 | – | – |
per 1 mol of Hydrogen ion | – | −38.531 | – | – |
per 1 mol of Iron(III) ion | – | −137.00 | – | – |
per 1 mol of | – | −154.13 | – | – |
per 1 mol of | – | −246.60 | – | – |
per 1 mol of Potassium ion | – | −246.60 | – | – |
per 1 mol of | – | −102.75 | – | – |
Changes in standard condition (2)
- Reaction of iron(II) chloride and potassium permanganate under acidic condition◆
ΔrG −1239.0 kJ/mol K 1.16 × 10217 pK −217.06
| 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 | – | −1239.0 | – | – |
per 1 mol of | – | −137.67 | – | – |
per 1 mol of | – | −247.80 | – | – |
per 1 mol of Hydrogen ion | – | −38.719 | – | – |
per 1 mol of Iron(III) ion | – | −137.67 | – | – |
per 1 mol of | – | −154.88 | – | – |
per 1 mol of | – | −247.80 | – | – |
per 1 mol of Potassium ion | – | −247.80 | – | – |
per 1 mol of | – | −103.25 | – | – |
Changes in standard condition (3)
- Reaction of iron(II) chloride and potassium permanganate under acidic condition◆
ΔrG −672.8 kJ/mol K 7.40 × 10117 pK −117.87
| 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 | −1091.2 | −672.8 | −1407 | – |
per 1 mol of | −121.24 | −74.76 | −156.3 | – |
per 1 mol of | −218.24 | −134.6 | −281.4 | – |
per 1 mol of Hydrogen ion | −34.100 | −21.02 | −43.97 | – |
per 1 mol of Iron(III) ion | −121.24 | −74.76 | −156.3 | – |
per 1 mol of | −136.40 | −84.10 | −175.9 | – |
per 1 mol of | −218.24 | −134.6 | −281.4 | – |
per 1 mol of Potassium ion | −218.24 | −134.6 | −281.4 | – |
per 1 mol of | −90.933 | −56.07 | −117.3 | – |
Changes in standard condition (4)
- Reaction of iron(II) chloride and potassium permanganate under acidic condition◆
ΔrG −678.8 kJ/mol K 8.33 × 10118 pK −118.92
| 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 | – | −678.8 | – | – |
per 1 mol of | – | −75.42 | – | – |
per 1 mol of | – | −135.8 | – | – |
per 1 mol of Hydrogen ion | – | −21.21 | – | – |
per 1 mol of Iron(III) ion | – | −75.42 | – | – |
per 1 mol of | – | −84.85 | – | – |
per 1 mol of | – | −135.8 | – | – |
per 1 mol of Potassium ion | – | −135.8 | – | – |
per 1 mol of | – | −56.57 | – | – |
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 |
|---|---|---|---|---|
| FeCl2 (cr) | -341.79[1] | -302.30[1] | 117.95[1] | 76.65[1] |
| FeCl2 (g) | -148.5[1] | – | – | – |
| FeCl2 (ai) | -423.4[1] | -341.34[1] | -24.7[1] | – |
| FeCl2 (ao) | – | -279.1[1] | – | – |
| FeCl2 (cr) 2 hydrate | -953.1[1] | – | – | – |
| FeCl2 (cr) 4 hydrate | -1549.3[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 |
|---|---|---|---|---|
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[1] | – |
| HClO (g) | -78.7[1] | -66.1[1] | 236.67[1] | 37.15[1] |
| HClO (ao) | -120.9[1] | -79.9[1] | 142[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°, -341.79 kJ · mol−1
- ^ ΔfG°, -302.30 kJ · mol−1
- ^ S°, 117.95 J · K−1 · mol−1
- ^ Cp°, 76.65 J · K−1 · mol−1
- ^ ΔfH°, -148.5 kJ · mol−1
- ^ ΔfH°, -423.4 kJ · mol−1
- ^ ΔfG°, -341.34 kJ · mol−1
- ^ S°, -24.7 J · K−1 · mol−1
- ^ ΔfG°, -279.1 kJ · mol−1
- ^ ΔfH°, -953.1 kJ · mol−1
- ^ ΔfH°, -1549.3 kJ · 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°, 5712.8 kJ · mol−1
- ^ ΔfH°, -48.5 kJ · mol−1
- ^ ΔfG°, -4.7 kJ · mol−1
- ^ S°, -315.9 J · K−1 · mol−1
- ^ ΔfH°, -78.7 kJ · mol−1
- ^ ΔfG°, -66.1 kJ · mol−1
- ^ S°, 236.67 J · K−1 · mol−1
- ^ Cp°, 37.15 J · K−1 · mol−1
- ^ ΔfH°, -120.9 kJ · mol−1
- ^ ΔfG°, -79.9 kJ · mol−1
- ^ S°, 142. 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