3S + 4KMnO4 → 2K2SO3 + SO2↑ + 4MnO2
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- Reaction of and potassium permanganate
The reaction of and potassium permanganate yields potassium sulfite, sulfur dioxide, and manganese(IV) oxide (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 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 and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Reducing | Reducing | ||
| KMnO4 | Potassium permanganate | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SO3 | Potassium sulfite | 2 | Oxidized | – |
| SO2 | Sulfur dioxide | 1 | Oxidized | – |
| MnO2 | Manganese(IV) oxide | 4 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of 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 | −1279.2 | – | – | – |
| −426.40 | – | – | – | |
per 1 mol of | −319.80 | – | – | – |
per 1 mol of | −639.60 | – | – | – |
per 1 mol of | −1279.2 | – | – | – |
per 1 mol of | −319.80 | – | – | – |
Changes in standard condition (2)
- Reaction of 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 | −1209.0 | – | – | – |
| −403.00 | – | – | – | |
per 1 mol of | −302.25 | – | – | – |
per 1 mol of | −604.50 | – | – | – |
per 1 mol of | −1209.0 | – | – | – |
per 1 mol of | −302.25 | – | – | – |
Changes in standard condition (3)
- Reaction of 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 | −1280.1 | – | – | – |
| −426.70 | – | – | – | |
per 1 mol of | −320.02 | – | – | – |
per 1 mol of | −640.05 | – | – | – |
per 1 mol of | −1280.1 | – | – | – |
per 1 mol of | −320.02 | – | – | – |
Changes in standard condition (4)
- Reaction of 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 | −1210.0 | – | – | – |
| −403.33 | – | – | – | |
per 1 mol of | −302.50 | – | – | – |
per 1 mol of | −605.00 | – | – | – |
per 1 mol of | −1210.0 | – | – | – |
per 1 mol of | −302.50 | – | – | – |
Changes in aqueous solution (1)
- Reaction of and potassium permanganate◆
ΔrG −1345.0 kJ/mol K 4.30 × 10235 pK −235.63
| 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 | −1482.0 | −1345.0 | −458 | – |
| −494.00 | −448.33 | −153 | – | |
per 1 mol of | −370.50 | −336.25 | −115 | – |
per 1 mol of | −741.00 | −672.50 | −229 | – |
per 1 mol of | −1482.0 | −1345.0 | −458 | – |
per 1 mol of | −370.50 | −336.25 | −115 | – |
Changes in aqueous solution (2)
- Reaction of and potassium permanganate◆
ΔrG −1345.4 kJ/mol K 5.06 × 10235 pK −235.70
| 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 | −1508.1 | −1345.4 | −544 | – |
| −502.70 | −448.47 | −181 | – | |
per 1 mol of | −377.02 | −336.35 | −136 | – |
per 1 mol of | −754.05 | −672.70 | −272 | – |
per 1 mol of | −1508.1 | −1345.4 | −544 | – |
per 1 mol of | −377.02 | −336.35 | −136 | – |
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 |
|---|---|---|---|---|
| (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] |
| 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, (g):Gas, (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 |
|---|---|---|---|---|
| K2SO3 (cr) | -1125.5[1] | – | – | – |
| K2SO3 (ai) | -1140.1[1] | -1053.1[1] | 176[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] | – |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (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°, 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°, -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°, -1125.5 kJ · mol−1
- ^ ΔfH°, -1140.1 kJ · mol−1
- ^ ΔfG°, -1053.1 kJ · mol−1
- ^ S°, 176. 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°, -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