12NaI + 6KMnO4 + 3H2O 🔥→ 6Na2MnO4 + KIO3 + 5KI + 6HI↑
Last updated:
- Reaction of sodium iodide and potassium permanganate under neutral condition
The reaction of sodium iodide, potassium permanganate, and water yields sodium manganate, potassium iodate, potassium iodide, and hydrogen 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 sodium 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 sodium iodide and potassium permanganate under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaI | Sodium iodide | 12 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 6 | Oxidizing | Oxidizing |
| H2O | Water | 3 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2MnO4 | Sodium manganate | 6 | Reduced | – |
| KIO3 | Potassium iodate | 1 | Oxidized | – |
| KI | Potassium iodide | 5 | – | – |
| HI | Hydrogen iodide | 6 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium 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 | 416.1 | – | – | – |
per 1 mol of | 34.68 | – | – | – |
per 1 mol of | 69.35 | – | – | – |
per 1 mol of | 138.7 | – | – | – |
per 1 mol of | 69.35 | – | – | – |
per 1 mol of | 416.1 | – | – | – |
per 1 mol of | 83.22 | – | – | – |
per 1 mol of | 69.35 | – | – | – |
Changes in aqueous solution (1)
- Reaction of sodium iodide and potassium permanganate under neutral condition◆
ΔrG 633.2 kJ/mol K 0.12 × 10−110 pK 110.93
| 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 | 507 | 633.2 | −430 | – |
per 1 mol of | 42.3 | 52.77 | −35.8 | – |
per 1 mol of | 84.5 | 105.5 | −71.7 | – |
per 1 mol of | 169 | 211.1 | −143 | – |
per 1 mol of | 84.5 | 105.5 | −71.7 | – |
per 1 mol of | 507 | 633.2 | −430 | – |
per 1 mol of | 101 | 126.6 | −86.0 | – |
per 1 mol of | 84.5 | 105.5 | −71.7 | – |
Changes in aqueous solution (2)
- Reaction of sodium iodide and potassium permanganate under neutral condition◆
ΔrG 313.6 kJ/mol K 0.11 × 10−54 pK 54.94
| 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 | 17 | 313.6 | −1002 | – |
per 1 mol of | 1.4 | 26.13 | −83.50 | – |
per 1 mol of | 2.8 | 52.27 | −167.0 | – |
per 1 mol of | 5.7 | 104.5 | −334.0 | – |
per 1 mol of | 2.8 | 52.27 | −167.0 | – |
per 1 mol of | 17 | 313.6 | −1002 | – |
per 1 mol of | 3.4 | 62.72 | −200.4 | – |
per 1 mol of | 2.8 | 52.27 | −167.0 | – |
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 |
|---|---|---|---|---|
| NaI (cr) | -287.78[1] | -286.06[1] | 98.53[1] | 52.09[1] |
| NaI (g) | -79.5[1] | -121.0[1] | 248.978[1] | 36.65[1] |
| NaI (ai) | -295.31[1] | -313.47[1] | 170.3[1] | -95.8[1] |
| NaI (cr) 1 hydrate | -883.096[1] | -771.10[1] | 196.2[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] |
| 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 |
|---|---|---|---|---|
| Na2MnO4 (cr) | -1156.0[1] | – | – | – |
| Na2MnO4 (ai) | -1134[1] | -1024.6[1] | 176[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] | – |
| 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] |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[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°, -287.78 kJ · mol−1
- ^ ΔfG°, -286.06 kJ · mol−1
- ^ S°, 98.53 J · K−1 · mol−1
- ^ Cp°, 52.09 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -121.0 kJ · mol−1
- ^ S°, 248.978 J · K−1 · mol−1
- ^ Cp°, 36.65 J · K−1 · mol−1
- ^ ΔfH°, -295.31 kJ · mol−1
- ^ ΔfG°, -313.47 kJ · mol−1
- ^ S°, 170.3 J · K−1 · mol−1
- ^ Cp°, -95.8 J · K−1 · mol−1
- ^ ΔfH°, -883.096 kJ · mol−1
- ^ ΔfG°, -771.10 kJ · mol−1
- ^ S°, 196.2 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°, -1156.0 kJ · mol−1
- ^ ΔfH°, -1134. kJ · mol−1
- ^ ΔfG°, -1024.6 kJ · mol−1
- ^ S°, 176. 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°, -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
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1