6Na2S + 2KMnO4 🔥→ 6Na2O + 5S + 2MnO + K2S
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- Reaction of sodium sulfide and potassium permanganate
The reaction of sodium sulfide and potassium permanganate yields sodium oxide, , manganese(II) oxide, and potassium sulfide (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 sulfide 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 sulfide and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2S | Sodium sulfide | 6 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2O | Sodium oxide | 6 | – | – |
| 5 | Oxidized | – | ||
| MnO | Manganese(II) oxide | 2 | Reduced | – |
| K2S | Potassium sulfide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium sulfide and potassium permanganate◆
ΔrG 231.4 kJ/mol K 0.29 × 10−40 pK 40.54
| 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 | 226.7 | 231.4 | −12 | – |
per 1 mol of | 37.78 | 38.57 | −2.0 | – |
per 1 mol of | 113.3 | 115.7 | −6.0 | – |
per 1 mol of | 37.78 | 38.57 | −2.0 | – |
| 45.34 | 46.28 | −2.4 | – | |
per 1 mol of | 113.3 | 115.7 | −6.0 | – |
per 1 mol of | 226.7 | 231.4 | −12 | – |
Changes in standard condition (2)
- Reaction of sodium sulfide 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 | 228.4 | – | – | – |
per 1 mol of | 38.07 | – | – | – |
per 1 mol of | 114.2 | – | – | – |
per 1 mol of | 38.07 | – | – | – |
| 45.68 | – | – | – | |
per 1 mol of | 114.2 | – | – | – |
per 1 mol of | 228.4 | – | – | – |
Changes in aqueous solution
- Reaction of sodium sulfide and potassium permanganate◆
ΔrG 630.3 kJ/mol K 0.38 × 10−110 pK 110.42
| 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 | 544.1 | 630.3 | −288.0 | – |
per 1 mol of | 90.68 | 105.0 | −48.00 | – |
per 1 mol of | 272.1 | 315.1 | −144.0 | – |
per 1 mol of | 90.68 | 105.0 | −48.00 | – |
| 108.8 | 126.1 | −57.60 | – | |
per 1 mol of | 272.1 | 315.1 | −144.0 | – |
per 1 mol of | 544.1 | 630.3 | −288.0 | – |
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 |
|---|---|---|---|---|
| Na2S (cr) | -364.8[1] | -349.8[1] | 83.7[1] | – |
| Na2S (ai) | -447.3[1] | -438.1[1] | 103.3[1] | – |
| Na2S (cr) 4.5 hydrate | -1725.9[1] | – | – | – |
| Na2S (cr) 5 hydrate | -1886.6[1] | – | – | – |
| Na2S (cr) 9 hydrate | -3074.0[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 |
|---|---|---|---|---|
| Na2O (cr) | -414.22[1] | -375.46[1] | 75.06[1] | 69.12[1] |
| Na2O (g) | -35.6[1] | -52.3[1] | 261.2[1] | 55.2[1] |
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[1] | – | – | – |
| K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
| K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
| K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
| K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
* (cr):Crystalline 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°, -364.8 kJ · mol−1
- ^ ΔfG°, -349.8 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1
- ^ ΔfH°, -447.3 kJ · mol−1
- ^ ΔfG°, -438.1 kJ · mol−1
- ^ S°, 103.3 J · K−1 · mol−1
- ^ ΔfH°, -1725.9 kJ · mol−1
- ^ ΔfH°, -1886.6 kJ · mol−1
- ^ ΔfH°, -3074.0 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°, -414.22 kJ · mol−1
- ^ ΔfG°, -375.46 kJ · mol−1
- ^ S°, 75.06 J · K−1 · mol−1
- ^ Cp°, 69.12 J · K−1 · mol−1
- ^ ΔfH°, -35.6 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 261.2 J · K−1 · mol−1
- ^ Cp°, 55.2 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 kJ · mol−1
- ^ ΔfH°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1