4NaSCN + 8KMnO4 → 4NaNO3 + MnSO4 + 4MnO + 3MnS + 4K2CO3
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The reaction of sodium thiocyanate and potassium permanganate yields sodium nitrate, manganese(II) sulfate, manganese(II) oxide, manganese(II) sulfide, and potassium carbonate (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 thiocyanate 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 thiocyanate and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaSCN | Sodium thiocyanate | 4 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 8 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO3 | Sodium nitrate | 4 | Oxidized | – |
| MnSO4 | Manganese(II) sulfate | 1 | Redoxed product | – |
| MnO | Manganese(II) oxide | 4 | Reduced | – |
| MnS | Manganese(II) sulfide | 3 | Reduced | – |
| K2CO3 | Potassium carbonate | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium thiocyanate 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 | −2344.6 | – | – | – |
per 1 mol of | −586.15 | – | – | – |
per 1 mol of | −293.07 | – | – | – |
per 1 mol of | −586.15 | – | – | – |
per 1 mol of | −2344.6 | – | – | – |
per 1 mol of | −586.15 | – | – | – |
per 1 mol of | −781.53 | – | – | – |
per 1 mol of | −586.15 | – | – | – |
Changes in standard condition (2)
- Reaction of sodium thiocyanate 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 | −2343.4 | – | – | – |
per 1 mol of | −585.85 | – | – | – |
per 1 mol of | −292.93 | – | – | – |
per 1 mol of | −585.85 | – | – | – |
per 1 mol of | −2343.4 | – | – | – |
per 1 mol of | −585.85 | – | – | – |
per 1 mol of | −781.13 | – | – | – |
per 1 mol of | −585.85 | – | – | – |
Changes in aqueous solution (1)
- Reaction of sodium thiocyanate and potassium permanganate◆
ΔrG −2441.8 kJ/mol K 6.09 × 10427 pK −427.78
| 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 | −2811.8 | −2441.8 | −1239.0 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
per 1 mol of | −351.48 | −305.23 | −154.88 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
per 1 mol of | −2811.8 | −2441.8 | −1239.0 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
per 1 mol of | −937.27 | −813.93 | −413.00 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
Changes in aqueous solution (2)
- Reaction of sodium thiocyanate and potassium permanganate◆
ΔrG −2428.8 kJ/mol K 3.22 × 10425 pK −425.51
| 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 | −2826.0 | −2428.8 | −1329.0 | – |
per 1 mol of | −706.50 | −607.20 | −332.25 | – |
per 1 mol of | −353.25 | −303.60 | −166.13 | – |
per 1 mol of | −706.50 | −607.20 | −332.25 | – |
per 1 mol of | −2826.0 | −2428.8 | −1329.0 | – |
per 1 mol of | −706.50 | −607.20 | −332.25 | – |
per 1 mol of | −942.00 | −809.60 | −443.00 | – |
per 1 mol of | −706.50 | −607.20 | −332.25 | – |
Changes in aqueous solution (3)
- Reaction of sodium thiocyanate and potassium permanganate◆
ΔrG −2441.8 kJ/mol K 6.09 × 10427 pK −427.78
| 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 | −2811.8 | −2441.8 | −1239.0 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
per 1 mol of | −351.48 | −305.23 | −154.88 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
per 1 mol of | −2811.8 | −2441.8 | −1239.0 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
per 1 mol of | −937.27 | −813.93 | −413.00 | – |
per 1 mol of | −702.95 | −610.45 | −309.75 | – |
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 |
|---|---|---|---|---|
| NaSCN (cr) | -170.50[1] | – | – | – |
| NaSCN (ai) | -163.68[1] | -169.18[1] | 203.3[1] | 6.3[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 |
|---|---|---|---|---|
| NaNO3 (cr) | -467.85[1] | -367.00[1] | 116.52[1] | 92.88[1] |
| NaNO3 (ai) | -447.48[1] | -373.15[1] | 205.4[1] | -40.2[1] |
| MnSO4 (cr) | -1065.25[1] | -957.36[1] | 112.1[1] | 100.50[1] |
| MnSO4 (ai) | -1130.1[1] | -972.7[1] | -53.6[1] | -243[1] |
| MnSO4 (ao) | -1115.9[1] | -985.7[1] | 36.4[1] | – |
| MnSO4 (cr) 1 hydrate α | -1376.5[1] | – | – | – |
| MnSO4 (cr) 1 hydrate β | -1348.1[1] | – | – | – |
| MnSO4 (cr) 4 hydrate | -2258.1[1] | – | – | – |
| MnSO4 (cr) 5 hydrate | -2553.1[1] | – | – | 326[1] |
| MnSO4 (cr) 7 hydrate | -3139.3[1] | – | – | – |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[1] | – | – | – |
| MnS (cr) green | -214.2[1] | -218.4[1] | 78.2[1] | 49.96[1] |
| MnS (am) precipitated, pink | -213.8[1] | – | – | – |
| K2CO3 (cr) | -1151.02[1] | -1063.5[1] | 155.52[1] | 114.43[1] |
| K2CO3 (ai) | -1181.90[1] | -1094.36[1] | 148.1[1] | – |
| K2CO3 (cr) 1.5 hydrate | -1609.2[1] | -1432.5[1] | 203.3[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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°, -170.50 kJ · mol−1
- ^ ΔfH°, -163.68 kJ · mol−1
- ^ ΔfG°, -169.18 kJ · mol−1
- ^ S°, 203.3 J · K−1 · mol−1
- ^ Cp°, 6.3 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°, -467.85 kJ · mol−1
- ^ ΔfG°, -367.00 kJ · mol−1
- ^ S°, 116.52 J · K−1 · mol−1
- ^ Cp°, 92.88 J · K−1 · mol−1
- ^ ΔfH°, -447.48 kJ · mol−1
- ^ ΔfG°, -373.15 kJ · mol−1
- ^ S°, 205.4 J · K−1 · mol−1
- ^ Cp°, -40.2 J · K−1 · mol−1
- ^ ΔfH°, -1065.25 kJ · mol−1
- ^ ΔfG°, -957.36 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 100.50 J · K−1 · mol−1
- ^ ΔfH°, -1130.1 kJ · mol−1
- ^ ΔfG°, -972.7 kJ · mol−1
- ^ S°, -53.6 J · K−1 · mol−1
- ^ Cp°, -243. J · K−1 · mol−1
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfG°, -985.7 kJ · mol−1
- ^ S°, 36.4 J · K−1 · mol−1
- ^ ΔfH°, -1376.5 kJ · mol−1
- ^ ΔfH°, -1348.1 kJ · mol−1
- ^ ΔfH°, -2258.1 kJ · mol−1
- ^ ΔfH°, -2553.1 kJ · mol−1
- ^ Cp°, 326. J · K−1 · mol−1
- ^ ΔfH°, -3139.3 kJ · 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°, -214.2 kJ · mol−1
- ^ ΔfG°, -218.4 kJ · mol−1
- ^ S°, 78.2 J · K−1 · mol−1
- ^ Cp°, 49.96 J · K−1 · mol−1
- ^ ΔfH°, -213.8 kJ · mol−1
- ^ ΔfH°, -1151.02 kJ · mol−1
- ^ ΔfG°, -1063.5 kJ · mol−1
- ^ S°, 155.52 J · K−1 · mol−1
- ^ Cp°, 114.43 J · K−1 · mol−1
- ^ ΔfH°, -1181.90 kJ · mol−1
- ^ ΔfG°, -1094.36 kJ · mol−1
- ^ S°, 148.1 J · K−1 · mol−1
- ^ ΔfH°, -1609.2 kJ · mol−1
- ^ ΔfG°, -1432.5 kJ · mol−1
- ^ S°, 203.3 J · K−1 · mol−1