3P + 3KMnO4 → Mn3(PO4)2 + K3PO4
Last updated:
The reaction of and potassium permanganate yields manganese(II) phosphate and potassium phosphate (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 | 3 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn3(PO4)2 | Manganese(II) phosphate | 1 | Redoxed product | – |
| K3PO4 | Potassium phosphate | 1 | Oxidized | – |
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 | −2555.3 | – | – | – |
| −851.77 | – | – | – | |
per 1 mol of | −851.77 | – | – | – |
per 1 mol of | −2555.3 | – | – | – |
per 1 mol of | −2555.3 | – | – | – |
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 | −2502.5 | – | – | – |
| −834.17 | – | – | – | |
per 1 mol of | −834.17 | – | – | – |
per 1 mol of | −2502.5 | – | – | – |
per 1 mol of | −2502.5 | – | – | – |
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 | −2437.4 | – | – | – |
| −812.47 | – | – | – | |
per 1 mol of | −812.47 | – | – | – |
per 1 mol of | −2437.4 | – | – | – |
per 1 mol of | −2437.4 | – | – | – |
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 | −2532.8 | – | – | – |
| −844.27 | – | – | – | |
per 1 mol of | −844.27 | – | – | – |
per 1 mol of | −2532.8 | – | – | – |
per 1 mol of | −2532.8 | – | – | – |
Changes in aqueous solution
- 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 | −2770.0 | – | – | – |
| −923.33 | – | – | – | |
per 1 mol of | −923.33 | – | – | – |
per 1 mol of | −2770.0 | – | – | – |
per 1 mol of | −2770.0 | – | – | – |
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) white | 0[1] | 0[1] | 41.09[1] | 23.84[1] |
| (cr) red, triclinic | -17.6[1] | -12.1[1] | 22.80[1] | 21.21[1] |
| (cr) black | -39.3[1] | – | – | – |
| (am) red | -7.5[1] | – | – | – |
| (g) | 314.64[1] | 278.25[1] | 163.193[1] | 20.786[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, (am):Amorphous 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 |
|---|---|---|---|---|
| Mn3(PO4)2 (cr) | -3116.7[1] | – | – | – |
| K3PO4 (cr) | -1950.2[1] | – | – | – |
| K3PO4 (ai) | -2034.7[1] | -1868.7[1] | 87.2[1] | – |
* (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.09 J · K−1 · mol−1
- ^ Cp°, 23.84 J · K−1 · mol−1
- ^ ΔfH°, -17.6 kJ · mol−1
- ^ ΔfG°, -12.1 kJ · mol−1
- ^ S°, 22.80 J · K−1 · mol−1
- ^ Cp°, 21.21 J · K−1 · mol−1
- ^ ΔfH°, -39.3 kJ · mol−1
- ^ ΔfH°, -7.5 kJ · mol−1
- ^ ΔfH°, 314.64 kJ · mol−1
- ^ ΔfG°, 278.25 kJ · mol−1
- ^ S°, 163.193 J · K−1 · mol−1
- ^ Cp°, 20.786 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°, -3116.7 kJ · mol−1
- ^ ΔfH°, -1950.2 kJ · mol−1
- ^ ΔfH°, -2034.7 kJ · mol−1
- ^ ΔfG°, -1868.7 kJ · mol−1
- ^ S°, 87.2 J · K−1 · mol−1