Se + 2KMnO4 → K2SeO4 + 2MnO2
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- Reaction of and potassium permanganate
The reaction of and potassium permanganate yields potassium selenate 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 oxidizable species and oxidizing species
- Oxidizable 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 |
---|---|---|---|---|
1 | Reducing | Oxidizable | ||
KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
K2SeO4 | Potassium selenate | 1 | Oxidized | – |
MnO2 | Manganese(IV) oxide | 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and potassium permanganate◆
ΔrG −457.9 kJ/mol K 1.66 × 1080 pK −80.22
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 | −475.7 | −457.9 | −58 | – |
−475.7 | −457.9 | −58 | – | |
per 1 mol of | −237.8 | −228.9 | −29 | – |
per 1 mol of | −475.7 | −457.9 | −58 | – |
per 1 mol of | −237.8 | −228.9 | −29 | – |
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 | −440.6 | – | – | – |
−440.6 | – | – | – | |
per 1 mol of | −220.3 | – | – | – |
per 1 mol of | −440.6 | – | – | – |
per 1 mol of | −220.3 | – | – | – |
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 | −482.4 | – | – | – |
−482.4 | – | – | – | |
per 1 mol of | −241.2 | – | – | – |
per 1 mol of | −482.4 | – | – | – |
per 1 mol of | −241.2 | – | – | – |
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 | −447.3 | – | – | – |
−447.3 | – | – | – | |
per 1 mol of | −223.7 | – | – | – |
per 1 mol of | −447.3 | – | – | – |
per 1 mol of | −223.7 | – | – | – |
Changes in aqueous solution
- Reaction of and potassium permanganate◆
ΔrG −477.2 kJ/mol K 4.00 × 1083 pK −83.60
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 | −556.2 | −477.2 | −264.7 | – |
−556.2 | −477.2 | −264.7 | – | |
per 1 mol of | −278.1 | −238.6 | −132.3 | – |
per 1 mol of | −556.2 | −477.2 | −264.7 | – |
per 1 mol of | −278.1 | −238.6 | −132.3 | – |
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) hexagonal, gray | 0[1] | 0[1] | 42.442[1] | 25.363[1] |
(cr) monoclinic, red | 6.7[1] | – | – | – |
(vit) | 5.0[1] | – | – | – |
(g) | 227.07[1] | 187.03[1] | 176.72[1] | 20.820[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, (vit):Vitreous liquid, (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 |
---|---|---|---|---|
K2SeO4 (cr) | -1110.02[1] | -1002.8[1] | 222[1] | – |
K2SeO4 (ai) | -1103.7[1] | -1007.9[1] | 259.0[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, (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°, 42.442 J · K−1 · mol−1
- ^ Cp°, 25.363 J · K−1 · mol−1
- ^ ΔfH°, 6.7 kJ · mol−1
- ^ ΔfH°, 5.0 kJ · mol−1
- ^ ΔfH°, 227.07 kJ · mol−1
- ^ ΔfG°, 187.03 kJ · mol−1
- ^ S°, 176.72 J · K−1 · mol−1
- ^ Cp°, 20.820 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°, -1110.02 kJ · mol−1
- ^ ΔfG°, -1002.8 kJ · mol−1
- ^ S°, 222. J · K−1 · mol−1
- ^ ΔfH°, -1103.7 kJ · mol−1
- ^ ΔfG°, -1007.9 kJ · mol−1
- ^ S°, 259.0 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