3MgI2 + 6KMnO4 + 3H2O → 3Mg(OH)2 + 4KIO3 + 3Mn2O3 + 2KI
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- Reaction of magnesium iodide and potassium permanganate under neutral condition
The reaction of magnesium iodide, potassium permanganate, and water yields magnesium hydroxide, potassium iodate, manganese(III) oxide, and potassium iodide (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 magnesium iodide and potassium permanganate under neutral condition
General equation
- Reaction of oxidizable species and oxidizing species under neutral condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of magnesium iodide and potassium permanganate under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgI2 | Magnesium iodide | 3 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 6 | Oxidizing | Oxidizing |
| H2O | Water | 3 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg(OH)2 | Magnesium hydroxide | 3 | – | – |
| KIO3 | Potassium iodate | 4 | Oxidized | – |
| Mn2O3 | Manganese(III) oxide | 3 | Reduced | – |
| KI | Potassium iodide | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of magnesium iodide and potassium permanganate under neutral condition◆
ΔrG −1255.4 kJ/mol K 8.64 × 10219 pK −219.94
| 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 | −1339.2 | −1255.4 | −289.6 | – |
per 1 mol of | −446.40 | −418.47 | −96.53 | – |
per 1 mol of | −223.20 | −209.23 | −48.27 | – |
per 1 mol of | −446.40 | −418.47 | −96.53 | – |
per 1 mol of | −446.40 | −418.47 | −96.53 | – |
per 1 mol of | −334.80 | −313.85 | −72.40 | – |
per 1 mol of | −446.40 | −418.47 | −96.53 | – |
per 1 mol of | −669.60 | −627.70 | −144.8 | – |
Changes in standard condition (2)
- Reaction of magnesium iodide and potassium permanganate under neutral 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 | −1327.1 | – | – | – |
per 1 mol of | −442.37 | – | – | – |
per 1 mol of | −221.18 | – | – | – |
per 1 mol of | −442.37 | – | – | – |
per 1 mol of | −442.37 | – | – | – |
per 1 mol of | −331.77 | – | – | – |
per 1 mol of | −442.37 | – | – | – |
per 1 mol of | −663.55 | – | – | – |
Changes in aqueous solution (1)
- Reaction of magnesium iodide and potassium permanganate under neutral condition◆
ΔrG −689.6 kJ/mol K 6.50 × 10120 pK −120.81
| 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 | −808.2 | −689.6 | −393.2 | – |
per 1 mol of | −269.4 | −229.9 | −131.1 | – |
per 1 mol of | −134.7 | −114.9 | −65.53 | – |
per 1 mol of | −269.4 | −229.9 | −131.1 | – |
per 1 mol of | −269.4 | −229.9 | −131.1 | – |
per 1 mol of | −202.1 | −172.4 | −98.30 | – |
per 1 mol of | −269.4 | −229.9 | −131.1 | – |
per 1 mol of | −404.1 | −344.8 | −196.6 | – |
Changes in aqueous solution (2)
- Reaction of magnesium iodide and potassium permanganate under neutral 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 | −796.1 | – | – | – |
per 1 mol of | −265.4 | – | – | – |
per 1 mol of | −132.7 | – | – | – |
per 1 mol of | −265.4 | – | – | – |
per 1 mol of | −265.4 | – | – | – |
per 1 mol of | −199.0 | – | – | – |
per 1 mol of | −265.4 | – | – | – |
per 1 mol of | −398.1 | – | – | – |
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 |
|---|---|---|---|---|
| MgI2 (cr) | -364.0[1] | -358.2[1] | 129.7[1] | – |
| MgI2 (g) | -172[1] | – | – | – |
| MgI2 (ai) | -577.22[1] | -558.1[1] | 84.5[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] |
| 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, (ai):Ionized aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| Mg(OH)2 (cr) | -924.54[1] | -833.51[1] | 63.18[1] | 77.03[1] |
| Mg(OH)2 (am) precipitated | -920.5[1] | – | – | – |
| Mg(OH)2 (g) | -561[1] | – | – | – |
| Mg(OH)2 (ai) | -926.84[1] | -769.4[1] | -159.4[1] | – |
| KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
| KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[1] | – |
| Mn2O3 (cr) | -959.0[1] | -881.1[1] | 110.5[1] | 107.65[1] |
| KI (cr) | -327.900[1] | -324.892[1] | 106.32[1] | 52.93[1] |
| KI (g) | -125.5[1] | -166.1[1] | 258.3[1] | 37.11[1] |
| KI (ai) | -307.57[1] | -334.85[1] | 213.8[1] | -120.5[1] |
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution
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°, -364.0 kJ · mol−1
- ^ ΔfG°, -358.2 kJ · mol−1
- ^ S°, 129.7 J · K−1 · mol−1
- ^ ΔfH°, -172. kJ · mol−1
- ^ ΔfH°, -577.22 kJ · mol−1
- ^ ΔfG°, -558.1 kJ · mol−1
- ^ S°, 84.5 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°, -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°, -924.54 kJ · mol−1
- ^ ΔfG°, -833.51 kJ · mol−1
- ^ S°, 63.18 J · K−1 · mol−1
- ^ Cp°, 77.03 J · K−1 · mol−1
- ^ ΔfH°, -920.5 kJ · mol−1
- ^ ΔfH°, -561. kJ · mol−1
- ^ ΔfH°, -926.84 kJ · mol−1
- ^ ΔfG°, -769.4 kJ · mol−1
- ^ S°, -159.4 J · K−1 · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 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°, -327.900 kJ · mol−1
- ^ ΔfG°, -324.892 kJ · mol−1
- ^ S°, 106.32 J · K−1 · mol−1
- ^ Cp°, 52.93 J · K−1 · mol−1
- ^ ΔfH°, -125.5 kJ · mol−1
- ^ ΔfG°, -166.1 kJ · mol−1
- ^ S°, 258.3 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -307.57 kJ · mol−1
- ^ ΔfG°, -334.85 kJ · mol−1
- ^ S°, 213.8 J · K−1 · mol−1
- ^ Cp°, -120.5 J · K−1 · mol−1