HSCN + KMnO4 → NO↑ + MnCO3 + KHS
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The reaction of thiocyanic acid and potassium permanganate yields nitrogen monoxide, manganese(II) carbonate, and potassium hydrogensulfide (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 thiocyanic acid 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 thiocyanic acid and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HSCN | Thiocyanic acid | 1 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 1 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO | Nitrogen monoxide | 1 | Oxidized | – |
| MnCO3 | Manganese(II) carbonate | 1 | Reduced | – |
| KHS | Potassium hydrogensulfide | 1 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of thiocyanic acid and potassium permanganate◆
ΔrG −363.6 kJ/mol K 5.01 × 1063 pK −63.70
| 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 | −356.4 | −363.6 | 23.9 | – |
per 1 mol of | −356.4 | −363.6 | 23.9 | – |
per 1 mol of | −356.4 | −363.6 | 23.9 | – |
per 1 mol of | −356.4 | −363.6 | 23.9 | – |
per 1 mol of | −356.4 | −363.6 | 23.9 | – |
per 1 mol of | −356.4 | −363.6 | 23.9 | – |
Changes in aqueous solution (2)
- Reaction of thiocyanic acid and potassium permanganate◆
ΔrG −368.4 kJ/mol K 3.47 × 1064 pK −64.54
| 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 | – | −368.4 | – | – |
per 1 mol of | – | −368.4 | – | – |
per 1 mol of | – | −368.4 | – | – |
per 1 mol of | – | −368.4 | – | – |
per 1 mol of | – | −368.4 | – | – |
per 1 mol of | – | −368.4 | – | – |
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 |
|---|---|---|---|---|
| HSCN (ai) | 76.44[1] | 92.71[1] | 144.3[1] | -40.2[1] |
| HSCN (ao) | – | 97.56[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] |
* (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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 |
|---|---|---|---|---|
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| MnCO3 (cr) natural | -894.1[1] | -816.7[1] | 85.8[1] | 81.50[1] |
| MnCO3 (cr) precipitated | -883.2[1] | – | – | – |
| KHS (cr) | -265.10[1] | – | – | 75.31[1] |
| KHS (ai) | -269.9[1] | -271.19[1] | 165.3[1] | – |
| KHS (cr) 0.25 hydrate | -337.2[1] | – | – | – |
* (g):Gas, (cr):Crystalline solid, (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°, 76.44 kJ · mol−1
- ^ ΔfG°, 92.71 kJ · mol−1
- ^ S°, 144.3 J · K−1 · mol−1
- ^ Cp°, -40.2 J · K−1 · mol−1
- ^ ΔfG°, 97.56 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°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · 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°, -265.10 kJ · mol−1
- ^ Cp°, 75.31 J · K−1 · mol−1
- ^ ΔfH°, -269.9 kJ · mol−1
- ^ ΔfG°, -271.19 kJ · mol−1
- ^ S°, 165.3 J · K−1 · mol−1
- ^ ΔfH°, -337.2 kJ · mol−1