Zn(SCN)2 + 4KMnO4 → ZnS + SO2↑ + N2↑ + 4MnO2 + 2K2CO3
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The reaction of zinc thiocyanate and potassium permanganate yields zinc sulfide, sulfur dioxide, , manganese(IV) oxide, 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 zinc 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 zinc thiocyanate and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn(SCN)2 | Zinc thiocyanate | 1 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnS | Zinc sulfide | 1 | – | – |
| SO2 | Sulfur dioxide | 1 | Oxidized | – |
| 1 | Oxidized | – | ||
| MnO2 | Manganese(IV) oxide | 4 | Reduced | – |
| K2CO3 | Potassium carbonate | 2 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of zinc thiocyanate and potassium permanganate◆
ΔrG −1661.9 kJ/mol K 1.42 × 10291 pK −291.15
| 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 | – | −1661.9 | – | – |
per 1 mol of | – | −1661.9 | – | – |
per 1 mol of | – | −415.48 | – | – |
per 1 mol of | – | −1661.9 | – | – |
per 1 mol of | – | −1661.9 | – | – |
| – | −1661.9 | – | – | |
per 1 mol of | – | −415.48 | – | – |
per 1 mol of | – | −830.95 | – | – |
Changes in aqueous solution (2)
- Reaction of zinc thiocyanate and potassium permanganate◆
ΔrG −1662.3 kJ/mol K 1.67 × 10291 pK −291.22
| 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 | – | −1662.3 | – | – |
per 1 mol of | – | −1662.3 | – | – |
per 1 mol of | – | −415.57 | – | – |
per 1 mol of | – | −1662.3 | – | – |
per 1 mol of | – | −1662.3 | – | – |
| – | −1662.3 | – | – | |
per 1 mol of | – | −415.57 | – | – |
per 1 mol of | – | −831.15 | – | – |
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 |
|---|---|---|---|---|
| Zn(SCN)2 (ao) | – | 33.1[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] |
* (ao):Un-ionized aqueous solution, (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 |
|---|---|---|---|---|
| ZnS (cr) | -205.98[1] | -201.29[1] | 57.7[1] | 46.0[1] |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[1] | – |
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[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, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (am):Amorphous 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)
- ^ ΔfG°, 33.1 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°, -205.98 kJ · mol−1
- ^ ΔfG°, -201.29 kJ · mol−1
- ^ S°, 57.7 J · K−1 · mol−1
- ^ Cp°, 46.0 J · K−1 · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 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°, -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