5FeF2 + KMnO4 + 17H+ → 5Fe3+ + Mn2+ + KF + 9HF↑ + 4H2O
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- Reaction of iron(II) fluoride and potassium permanganate under acidic condition
- 5FeF2Iron(II) fluoride + KMnO4Potassium permanganate + 17H+Hydrogen ion5Fe3+Iron(III) ion + Mn2+Manganese(II) ion + KFPotassium fluoride + 9HF↑Hydrogen fluoride + 4H2OWater⟶
The reaction of iron(II) fluoride, potassium permanganate, and hydrogen ion yields iron(III) ion, manganese(II) ion, potassium fluoride, hydrogen fluoride, 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) fluoride and potassium permanganate under acidic condition
- 5FeF2Iron(II) fluoride + KMnO4Potassium permanganate + 17H+Hydrogen ion5Fe3+Iron(III) ion + Mn2+Manganese(II) ion + KFPotassium fluoride + 9HF↑Hydrogen fluoride + 4H2OWater⟶
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) fluoride and potassium permanganate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeF2 | Iron(II) fluoride | 5 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 1 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 17 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3+ | Iron(III) ion | 5 | Oxidized | – |
| Mn2+ | Manganese(II) ion | 1 | Reduced | – |
| KF | Potassium fluoride | 1 | – | – |
| HF | Hydrogen fluoride | 9 | – | – |
| H2O | Water | 4 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) 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 | −111.7 | – | – | – |
per 1 mol of | −22.34 | – | – | – |
per 1 mol of | −111.7 | – | – | – |
per 1 mol of Hydrogen ion | −6.571 | – | – | – |
per 1 mol of Iron(III) ion | −22.34 | – | – | – |
per 1 mol of Manganese(II) ion | −111.7 | – | – | – |
per 1 mol of | −111.7 | – | – | – |
per 1 mol of | −12.41 | – | – | – |
per 1 mol of | −27.93 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(II) 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 | −552.5 | – | – | – |
per 1 mol of | −110.5 | – | – | – |
per 1 mol of | −552.5 | – | – | – |
per 1 mol of Hydrogen ion | −32.50 | – | – | – |
per 1 mol of Iron(III) ion | −110.5 | – | – | – |
per 1 mol of Manganese(II) ion | −552.5 | – | – | – |
per 1 mol of | −552.5 | – | – | – |
per 1 mol of | −61.39 | – | – | – |
per 1 mol of | −138.1 | – | – | – |
Changes in standard condition (3)
- Reaction of iron(II) 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 | −552.5 | – | – | – |
per 1 mol of | −110.5 | – | – | – |
per 1 mol of | −552.5 | – | – | – |
per 1 mol of Hydrogen ion | −32.50 | – | – | – |
per 1 mol of Iron(III) ion | −110.5 | – | – | – |
per 1 mol of Manganese(II) ion | −552.5 | – | – | – |
per 1 mol of | −552.5 | – | – | – |
per 1 mol of | −61.39 | – | – | – |
per 1 mol of | −138.1 | – | – | – |
Changes in standard condition (4)
- Reaction of iron(II) fluoride and potassium permanganate under acidic condition◆
ΔrG −147.5 kJ/mol K 6.93 × 1025 pK −25.84
| 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 | −281.2 | −147.5 | −449.4 | – |
per 1 mol of | −56.24 | −29.50 | −89.88 | – |
per 1 mol of | −281.2 | −147.5 | −449.4 | – |
per 1 mol of Hydrogen ion | −16.54 | −8.676 | −26.44 | – |
per 1 mol of Iron(III) ion | −56.24 | −29.50 | −89.88 | – |
per 1 mol of Manganese(II) ion | −281.2 | −147.5 | −449.4 | – |
per 1 mol of | −281.2 | −147.5 | −449.4 | – |
per 1 mol of | −31.24 | −16.39 | −49.93 | – |
per 1 mol of | −70.30 | −36.88 | −112.3 | – |
Changes in standard condition (5)
- Reaction of iron(II) fluoride and potassium permanganate under acidic condition◆
ΔrG −360.1 kJ/mol K 1.22 × 1063 pK −63.09
| 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 | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of | −144.4 | −72.02 | −243.02 | – |
per 1 mol of | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of Hydrogen ion | −42.47 | −21.18 | −71.476 | – |
per 1 mol of Iron(III) ion | −144.4 | −72.02 | −243.02 | – |
per 1 mol of Manganese(II) ion | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of | −80.22 | −40.01 | −135.01 | – |
per 1 mol of | −180.5 | −90.03 | −303.77 | – |
Changes in standard condition (6)
- Reaction of iron(II) fluoride and potassium permanganate under acidic condition◆
ΔrG −360.1 kJ/mol K 1.22 × 1063 pK −63.09
| 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 | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of | −144.4 | −72.02 | −243.02 | – |
per 1 mol of | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of Hydrogen ion | −42.47 | −21.18 | −71.476 | – |
per 1 mol of Iron(III) ion | −144.4 | −72.02 | −243.02 | – |
per 1 mol of Manganese(II) ion | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of | −722.0 | −360.1 | −1215.1 | – |
per 1 mol of | −80.22 | −40.01 | −135.01 | – |
per 1 mol of | −180.5 | −90.03 | −303.77 | – |
Changes in standard condition (7)
- Reaction of iron(II) 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 | −665.5 | – | – | – |
per 1 mol of | −133.1 | – | – | – |
per 1 mol of | −665.5 | – | – | – |
per 1 mol of Hydrogen ion | −39.15 | – | – | – |
per 1 mol of Iron(III) ion | −133.1 | – | – | – |
per 1 mol of Manganese(II) ion | −665.5 | – | – | – |
per 1 mol of | −665.5 | – | – | – |
per 1 mol of | −73.94 | – | – | – |
per 1 mol of | −166.4 | – | – | – |
Changes in standard condition (8)
- Reaction of iron(II) fluoride and potassium permanganate under acidic condition◆
ΔrG −197.8 kJ/mol K 4.50 × 1034 pK −34.65
| 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 | −835.0 | −197.8 | −2137.6 | – |
per 1 mol of | −167.0 | −39.56 | −427.52 | – |
per 1 mol of | −835.0 | −197.8 | −2137.6 | – |
per 1 mol of Hydrogen ion | −49.12 | −11.64 | −125.74 | – |
per 1 mol of Iron(III) ion | −167.0 | −39.56 | −427.52 | – |
per 1 mol of Manganese(II) ion | −835.0 | −197.8 | −2137.6 | – |
per 1 mol of | −835.0 | −197.8 | −2137.6 | – |
per 1 mol of | −92.78 | −21.98 | −237.51 | – |
per 1 mol of | −208.8 | −49.45 | −534.40 | – |
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 |
|---|---|---|---|---|
| FeF2 (cr) | -711.3[1] | -668.6[1] | 86.99[1] | 68.12[1] |
| FeF2 (ai) | -754.4[1] | -636.48[1] | -165.3[1] | – |
| FeF2 (aq) | -745.2[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, (aq):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 |
|---|---|---|---|---|
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[1] | – |
| Mn2+ (g) | 2519.69[1] | – | – | – |
| Mn2+ (ao) | -220.75[1] | -228.1[1] | -73.6[1] | 50[1] |
| KF (cr) | -567.27[1] | -537.75[1] | 66.57[1] | 49.04[1] |
| KF (g) | -325.43[1] | -343.62[1] | 226.41[1] | 35.23[1] |
| KF (ai) | -585.01[1] | -562.06[1] | 88.7[1] | -84.9[1] |
| KF (cr) 2 hydrate | -1163.621[1] | -1021.49[1] | 155.2[1] | – |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[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°, -711.3 kJ · mol−1
- ^ ΔfG°, -668.6 kJ · mol−1
- ^ S°, 86.99 J · K−1 · mol−1
- ^ Cp°, 68.12 J · K−1 · mol−1
- ^ ΔfH°, -754.4 kJ · mol−1
- ^ ΔfG°, -636.48 kJ · mol−1
- ^ S°, -165.3 J · K−1 · mol−1
- ^ ΔfH°, -745.2 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°, 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°, -567.27 kJ · mol−1
- ^ ΔfG°, -537.75 kJ · mol−1
- ^ S°, 66.57 J · K−1 · mol−1
- ^ Cp°, 49.04 J · K−1 · mol−1
- ^ ΔfH°, -325.43 kJ · mol−1
- ^ ΔfG°, -343.62 kJ · mol−1
- ^ S°, 226.41 J · K−1 · mol−1
- ^ Cp°, 35.23 J · K−1 · mol−1
- ^ ΔfH°, -585.01 kJ · mol−1
- ^ ΔfG°, -562.06 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1
- ^ Cp°, -84.9 J · K−1 · mol−1
- ^ ΔfH°, -1163.621 kJ · mol−1
- ^ ΔfG°, -1021.49 kJ · mol−1
- ^ S°, 155.2 J · K−1 · mol−1
- ^ ΔfH°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 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