3Na2S2O3 + 8KMnO4 → 3Na2SO4 + 3K2SO4 + 8MnO2 + K2O
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The reaction of sodium thiosulfate and potassium permanganate yields sodium sulfate, potassium sulfate, manganese(IV) 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 sodium thiosulfate and potassium permanganate
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of sodium thiosulfate and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2S2O3 | Sodium thiosulfate | 3 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 8 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2SO4 | Sodium sulfate | 3 | Oxidized | – |
| K2SO4 | Potassium sulfate | 3 | Oxidized | – |
| MnO2 | Manganese(IV) oxide | 8 | Reduced | – |
| K2O | Potassium oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium thiosulfate and potassium permanganate◆
ΔrG −2833.0 kJ/mol K 2.09 × 10496 pK −496.32
| 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 | −2929.8 | −2833.0 | −345 | – |
per 1 mol of | −976.60 | −944.33 | −115 | – |
per 1 mol of | −366.23 | −354.13 | −43.1 | – |
per 1 mol of | −976.60 | −944.33 | −115 | – |
per 1 mol of | −976.60 | −944.33 | −115 | – |
per 1 mol of | −366.23 | −354.13 | −43.1 | – |
per 1 mol of | −2929.8 | −2833.0 | −345 | – |
Changes in standard condition (2)
- Reaction of sodium thiosulfate and potassium permanganate
| 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 | −2789.5 | – | – | – |
per 1 mol of | −929.83 | – | – | – |
per 1 mol of | −348.69 | – | – | – |
per 1 mol of | −929.83 | – | – | – |
per 1 mol of | −929.83 | – | – | – |
per 1 mol of | −348.69 | – | – | – |
per 1 mol of | −2789.5 | – | – | – |
Changes in standard condition (3)
- Reaction of sodium thiosulfate and potassium permanganate
| 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 | – | – | −329 | – |
per 1 mol of | – | – | −110 | – |
per 1 mol of | – | – | −41.1 | – |
per 1 mol of | – | – | −110 | – |
per 1 mol of | – | – | −110 | – |
per 1 mol of | – | – | −41.1 | – |
per 1 mol of | – | – | −329 | – |
Changes in standard condition (4)
- Reaction of sodium thiosulfate and potassium permanganate
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution
- Reaction of sodium thiosulfate and potassium permanganate◆
ΔrG −2799.5 kJ/mol K 2.83 × 10490 pK −490.45
| 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 | −3184.7 | −2799.5 | −1293.8 | – |
per 1 mol of | −1061.6 | −933.17 | −431.27 | – |
per 1 mol of | −398.09 | −349.94 | −161.72 | – |
per 1 mol of | −1061.6 | −933.17 | −431.27 | – |
per 1 mol of | −1061.6 | −933.17 | −431.27 | – |
per 1 mol of | −398.09 | −349.94 | −161.72 | – |
per 1 mol of | −3184.7 | −2799.5 | −1293.8 | – |
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 |
|---|---|---|---|---|
| Na2S2O3 (cr) | -1123.0[1] | -1028.0[1] | 155[1] | – |
| Na2S2O3 (ai) | -1132.40[1] | -1046.0[1] | 184.1[1] | – |
| Na2S2O3 (cr) 5 hydrate | -2607.93[1] | -2229.8[1] | 372[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, (ai):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 |
|---|---|---|---|---|
| Na2SO4 (cr) orthorhombic | -1387.08[1] | -1270.16[1] | 149.58[1] | 128.20[1] |
| Na2SO4 (cr) metastable | – | – | 154.934[1] | 129.29[1] |
| Na2SO4 (ai) | -1389.51[1] | -1268.36[1] | 138.1[1] | -201[1] |
| Na2SO4 (cr) 10 hydrate | -4327.26[1] | -3646.85[1] | 592.0[1] | – |
| K2SO4 (cr) | -1437.79[1] | -1321.37[1] | 175.56[1] | 131.46[1] |
| K2SO4 (g) | -1096[1] | -1033[1] | 364[1] | 108.8[1] |
| K2SO4 (ai) | -1414.02[1] | -1311.07[1] | 225.1[1] | -251[1] |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[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, (am):Amorphous solid
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°, -1123.0 kJ · mol−1
- ^ ΔfG°, -1028.0 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -1132.40 kJ · mol−1
- ^ ΔfG°, -1046.0 kJ · mol−1
- ^ S°, 184.1 J · K−1 · mol−1
- ^ ΔfH°, -2607.93 kJ · mol−1
- ^ ΔfG°, -2229.8 kJ · mol−1
- ^ S°, 372. 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°, -1387.08 kJ · mol−1
- ^ ΔfG°, -1270.16 kJ · mol−1
- ^ S°, 149.58 J · K−1 · mol−1
- ^ Cp°, 128.20 J · K−1 · mol−1
- ^ S°, 154.934 J · K−1 · mol−1
- ^ Cp°, 129.29 J · K−1 · mol−1
- ^ ΔfH°, -1389.51 kJ · mol−1
- ^ ΔfG°, -1268.36 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ Cp°, -201. J · K−1 · mol−1
- ^ ΔfH°, -4327.26 kJ · mol−1
- ^ ΔfG°, -3646.85 kJ · mol−1
- ^ S°, 592.0 J · K−1 · mol−1
- ^ ΔfH°, -1437.79 kJ · mol−1
- ^ ΔfG°, -1321.37 kJ · mol−1
- ^ S°, 175.56 J · K−1 · mol−1
- ^ Cp°, 131.46 J · K−1 · mol−1
- ^ ΔfH°, -1096. kJ · mol−1
- ^ ΔfG°, -1033. kJ · mol−1
- ^ S°, 364. J · K−1 · mol−1
- ^ Cp°, 108.8 J · K−1 · mol−1
- ^ ΔfH°, -1414.02 kJ · mol−1
- ^ ΔfG°, -1311.07 kJ · mol−1
- ^ S°, 225.1 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · 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