5NaSCN + 6KMnO4 → 5NaNO2 + 5MnS + MnCO3 + 3K2CO3 + CO2↑
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The reaction of sodium thiocyanate and potassium permanganate yields sodium nitrite, manganese(II) sulfide, manganese(II) carbonate, potassium carbonate, and carbon dioxide (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 | 5 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 6 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO2 | Sodium nitrite | 5 | Oxidized | – |
| MnS | Manganese(II) sulfide | 5 | Reduced | – |
| MnCO3 | Manganese(II) carbonate | 1 | Reduced | – |
| K2CO3 | Potassium carbonate | 3 | – | – |
| CO2 | Carbon dioxide | 1 | – | – |
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 | −1729.2 | – | – | – |
per 1 mol of | −345.84 | – | – | – |
per 1 mol of | −288.20 | – | – | – |
per 1 mol of | −345.84 | – | – | – |
per 1 mol of | −345.84 | – | – | – |
per 1 mol of | −1729.2 | – | – | – |
per 1 mol of | −576.40 | – | – | – |
per 1 mol of | −1729.2 | – | – | – |
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 | −1718.3 | – | – | – |
per 1 mol of | −343.66 | – | – | – |
per 1 mol of | −286.38 | – | – | – |
per 1 mol of | −343.66 | – | – | – |
per 1 mol of | −343.66 | – | – | – |
per 1 mol of | −1718.3 | – | – | – |
per 1 mol of | −572.77 | – | – | – |
per 1 mol of | −1718.3 | – | – | – |
Changes in standard condition (3)
- 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 | −1727.2 | – | – | – |
per 1 mol of | −345.44 | – | – | – |
per 1 mol of | −287.87 | – | – | – |
per 1 mol of | −345.44 | – | – | – |
per 1 mol of | −345.44 | – | – | – |
per 1 mol of | −1727.2 | – | – | – |
per 1 mol of | −575.73 | – | – | – |
per 1 mol of | −1727.2 | – | – | – |
Changes in standard condition (4)
- 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 | −1716.3 | – | – | – |
per 1 mol of | −343.26 | – | – | – |
per 1 mol of | −286.05 | – | – | – |
per 1 mol of | −343.26 | – | – | – |
per 1 mol of | −343.26 | – | – | – |
per 1 mol of | −1716.3 | – | – | – |
per 1 mol of | −572.10 | – | – | – |
per 1 mol of | −1716.3 | – | – | – |
Changes in aqueous solution (1)
- Reaction of sodium thiocyanate and potassium permanganate◆
ΔrG −1827.7 kJ/mol K 1.58 × 10320 pK −320.20
| 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 | −2047.1 | −1827.7 | −733.9 | – |
per 1 mol of | −409.42 | −365.54 | −146.8 | – |
per 1 mol of | −341.18 | −304.62 | −122.3 | – |
per 1 mol of | −409.42 | −365.54 | −146.8 | – |
per 1 mol of | −409.42 | −365.54 | −146.8 | – |
per 1 mol of | −2047.1 | −1827.7 | −733.9 | – |
per 1 mol of | −682.37 | −609.23 | −244.6 | – |
per 1 mol of | −2047.1 | −1827.7 | −733.9 | – |
Changes in aqueous solution (2)
- Reaction of sodium thiocyanate and potassium permanganate◆
ΔrG −1819.4 kJ/mol K 5.56 × 10318 pK −318.75
| 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 | −2067.4 | −1819.4 | −830.0 | – |
per 1 mol of | −413.48 | −363.88 | −166.0 | – |
per 1 mol of | −344.57 | −303.23 | −138.3 | – |
per 1 mol of | −413.48 | −363.88 | −166.0 | – |
per 1 mol of | −413.48 | −363.88 | −166.0 | – |
per 1 mol of | −2067.4 | −1819.4 | −830.0 | – |
per 1 mol of | −689.13 | −606.47 | −276.7 | – |
per 1 mol of | −2067.4 | −1819.4 | −830.0 | – |
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 |
|---|---|---|---|---|
| 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 |
|---|---|---|---|---|
| NaNO2 (cr) | -358.65[1] | -284.55[1] | 103.8[1] | – |
| NaNO2 (ai) | -344.8[1] | -294.1[1] | 182.0[1] | -51.0[1] |
| MnS (cr) green | -214.2[1] | -218.4[1] | 78.2[1] | 49.96[1] |
| MnS (am) precipitated, pink | -213.8[1] | – | – | – |
| MnCO3 (cr) natural | -894.1[1] | -816.7[1] | 85.8[1] | 81.50[1] |
| MnCO3 (cr) precipitated | -883.2[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] | – |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid, (g):Gas, (ao):Un-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°, -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°, -358.65 kJ · mol−1
- ^ ΔfG°, -284.55 kJ · mol−1
- ^ S°, 103.8 J · K−1 · mol−1
- ^ ΔfH°, -344.8 kJ · mol−1
- ^ ΔfG°, -294.1 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ Cp°, -51.0 J · K−1 · 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°, -894.1 kJ · mol−1
- ^ ΔfG°, -816.7 kJ · mol−1
- ^ S°, 85.8 J · K−1 · mol−1
- ^ Cp°, 81.50 J · K−1 · mol−1
- ^ ΔfH°, -883.2 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
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 J · K−1 · mol−1