6NaSCN + 10KMnO4 → 6NaNO3 + S + 6MnCO3 + 4MnO + 5K2S
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The reaction of sodium thiocyanate and potassium permanganate yields sodium nitrate, , manganese(II) carbonate, 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 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 | 6 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 10 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO3 | Sodium nitrate | 6 | Oxidized | – |
| 1 | Oxidized | – | ||
| MnCO3 | Manganese(II) carbonate | 6 | Reduced | – |
| MnO | Manganese(II) oxide | 4 | Reduced | – |
| K2S | Potassium sulfide | 5 | – | – |
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 | −2221.1 | – | – | – |
per 1 mol of | −370.18 | – | – | – |
per 1 mol of | −222.11 | – | – | – |
per 1 mol of | −370.18 | – | – | – |
| −2221.1 | – | – | – | |
per 1 mol of | −370.18 | – | – | – |
per 1 mol of | −555.27 | – | – | – |
per 1 mol of | −444.22 | – | – | – |
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 | −2155.7 | – | – | – |
per 1 mol of | −359.28 | – | – | – |
per 1 mol of | −215.57 | – | – | – |
per 1 mol of | −359.28 | – | – | – |
| −2155.7 | – | – | – | |
per 1 mol of | −359.28 | – | – | – |
per 1 mol of | −538.92 | – | – | – |
per 1 mol of | −431.14 | – | – | – |
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 | −2220.8 | – | – | – |
per 1 mol of | −370.13 | – | – | – |
per 1 mol of | −222.08 | – | – | – |
per 1 mol of | −370.13 | – | – | – |
| −2220.8 | – | – | – | |
per 1 mol of | −370.13 | – | – | – |
per 1 mol of | −555.20 | – | – | – |
per 1 mol of | −444.16 | – | – | – |
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 | −2155.4 | – | – | – |
per 1 mol of | −359.23 | – | – | – |
per 1 mol of | −215.54 | – | – | – |
per 1 mol of | −359.23 | – | – | – |
| −2155.4 | – | – | – | |
per 1 mol of | −359.23 | – | – | – |
per 1 mol of | −538.85 | – | – | – |
per 1 mol of | −431.08 | – | – | – |
Changes in aqueous solution
- Reaction of sodium thiocyanate and potassium permanganate◆
ΔrG −2674.1 kJ/mol K 3.03 × 10468 pK −468.48
| 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 | −3027.8 | −2674.1 | −1187.0 | – |
per 1 mol of | −504.63 | −445.68 | −197.83 | – |
per 1 mol of | −302.78 | −267.41 | −118.70 | – |
per 1 mol of | −504.63 | −445.68 | −197.83 | – |
| −3027.8 | −2674.1 | −1187.0 | – | |
per 1 mol of | −504.63 | −445.68 | −197.83 | – |
per 1 mol of | −756.95 | −668.52 | −296.75 | – |
per 1 mol of | −605.56 | −534.82 | −237.40 | – |
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] |
| (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] |
| MnCO3 (cr) natural | -894.1[1] | -816.7[1] | 85.8[1] | 81.50[1] |
| MnCO3 (cr) precipitated | -883.2[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, (ai):Ionized aqueous solution, (g):Gas
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°, 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°, -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°, -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