2NH4I + 8KMnO4 → N2↑ + I2 + 4K2MnO4 + 4H2MnO4
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- Reaction of ammonium iodide and potassium permanganate
- 2NH4IAmmonium iodide + 8KMnO4Potassium permanganate↑ + + 4K2MnO4Potassium manganate + 4H2MnO4Manganic acid⟶
The reaction of ammonium iodide and potassium permanganate yields , , potassium manganate, and manganic acid (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 ammonium iodide and potassium permanganate
- 2NH4IAmmonium iodide + 8KMnO4Potassium permanganate↑ + + 4K2MnO4Potassium manganate + 4H2MnO4Manganic acid⟶
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 ammonium iodide and potassium permanganate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4I | Ammonium iodide | 2 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 8 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Oxidized | – | ||
| 1 | Oxidized | – | ||
| K2MnO4 | Potassium manganate | 4 | Reduced | – |
| H2MnO4 | Manganic acid | 4 | Reduced | – |
Thermodynamic changes
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 |
|---|---|---|---|---|
| NH4I (cr) | -201.42[1] | -112.5[1] | 117[1] | – |
| NH4I (ai) | -187.69[1] | -130.88[1] | 224.7[1] | -62.3[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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
| (cr) | 0[1] | 0[1] | 116.135[1] | 54.438[1] |
| (g) | 62.438[1] | 19.327[1] | 260.69[1] | 36.90[1] |
| (ao) | 22.6[1] | 16.40[1] | 137.2[1] | – |
| K2MnO4 | – | – | – | – |
| H2MnO4 | – | – | – | – |
* (g):Gas, (cr):Crystalline solid, (ao):Un-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°, -201.42 kJ · mol−1
- ^ ΔfG°, -112.5 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -187.69 kJ · mol−1
- ^ ΔfG°, -130.88 kJ · mol−1
- ^ S°, 224.7 J · K−1 · mol−1
- ^ Cp°, -62.3 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°, 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 116.135 J · K−1 · mol−1
- ^ Cp°, 54.438 J · K−1 · mol−1
- ^ ΔfH°, 62.438 kJ · mol−1
- ^ ΔfG°, 19.327 kJ · mol−1
- ^ S°, 260.69 J · K−1 · mol−1
- ^ Cp°, 36.90 J · K−1 · mol−1
- ^ ΔfH°, 22.6 kJ · mol−1
- ^ ΔfG°, 16.40 kJ · mol−1
- ^ S°, 137.2 J · K−1 · mol−1