12FeCl2 + 50KMnO4 🔥→ 4Fe3O4 + 24KClO4 + 25Mn2O3 + 13K2O
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The reaction of iron(II) chloride and potassium permanganate yields iron(II,III) oxide, potassium perchlorate, manganese(III) oxide, and potassium oxide (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
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of iron(II) chloride and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCl2 | Iron(II) chloride | 12 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 50 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3O4 | Iron(II,III) oxide | 4 | Oxidized | – |
| KClO4 | Potassium perchlorate | 24 | Oxidized | – |
| Mn2O3 | Manganese(III) oxide | 25 | Reduced | – |
| K2O | Potassium oxide | 13 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(II) chloride and potassium permanganate◆
ΔrG 2957.0 kJ/mol K 0.90 × 10−518 pK 518.04
| 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 | 2427.4 | 2957.0 | −1805.5 | 251.9 |
per 1 mol of | 202.28 | 246.42 | −150.46 | 20.99 |
per 1 mol of | 48.548 | 59.140 | −36.110 | 5.038 |
per 1 mol of | 606.85 | 739.25 | −451.38 | 62.98 |
per 1 mol of | 101.14 | 123.21 | −75.229 | 10.50 |
per 1 mol of | 97.096 | 118.28 | −72.220 | 10.08 |
per 1 mol of | 186.72 | 227.46 | −138.88 | 19.38 |
Changes in aqueous solution (1)
- Reaction of iron(II) chloride and potassium permanganate◆
ΔrG 2594.8 kJ/mol K 0.26 × 10−454 pK 454.59
| 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 | – | 2594.8 | – | – |
per 1 mol of | – | 216.23 | – | – |
per 1 mol of | – | 51.896 | – | – |
per 1 mol of | – | 648.70 | – | – |
per 1 mol of | – | 108.12 | – | – |
per 1 mol of | – | 103.79 | – | – |
per 1 mol of | – | 199.60 | – | – |
Changes in aqueous solution (2)
- Reaction of iron(II) chloride and potassium permanganate◆
ΔrG 3341.7 kJ/mol K 0.36 × 10−585 pK 585.44
| 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 | 2461.7 | 3341.7 | −2989.2 | – |
per 1 mol of | 205.14 | 278.47 | −249.10 | – |
per 1 mol of | 49.234 | 66.834 | −59.784 | – |
per 1 mol of | 615.42 | 835.42 | −747.30 | – |
per 1 mol of | 102.57 | 139.24 | −124.55 | – |
per 1 mol of | 98.468 | 133.67 | −119.57 | – |
per 1 mol of | 189.36 | 257.05 | −229.94 | – |
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] |
* (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 |
|---|---|---|---|---|
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| KClO4 (cr) | -432.75[1] | -303.09[1] | 151.0[1] | 112.38[1] |
| KClO4 (ai) | -381.71[1] | -291.79[1] | 284.5[1] | – |
| Mn2O3 (cr) | -959.0[1] | -881.1[1] | 110.5[1] | 107.65[1] |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 J · K−1 · mol−1
- ^ ΔfH°, -432.75 kJ · mol−1
- ^ ΔfG°, -303.09 kJ · mol−1
- ^ S°, 151.0 J · K−1 · mol−1
- ^ Cp°, 112.38 J · K−1 · mol−1
- ^ ΔfH°, -381.71 kJ · mol−1
- ^ ΔfG°, -291.79 kJ · mol−1
- ^ S°, 284.5 J · K−1 · mol−1
- ^ ΔfH°, -959.0 kJ · mol−1
- ^ ΔfG°, -881.1 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, 107.65 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280