NH4I + 2KMnO4 → NH3↑ + KIO3 + 2MnO2 + KOH
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The reaction of ammonium iodide and potassium permanganate yields ammonia, potassium iodate, manganese(IV) oxide, and potassium hydroxide (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
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 | 1 | Reducing | Reducing |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH3 | Ammonia | 1 | – | – |
| KIO3 | Potassium iodate | 1 | Oxidized | – |
| MnO2 | Manganese(IV) oxide | 2 | Reduced | – |
| KOH | Potassium hydroxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of ammonium iodide and potassium permanganate◆
ΔrG −156.5 kJ/mol K 2.62 × 1027 pK −27.42
| 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 | −136.5 | −156.5 | 68 | – |
per 1 mol of | −136.5 | −156.5 | 68 | – |
per 1 mol of | −68.25 | −78.25 | 34 | – |
per 1 mol of | −136.5 | −156.5 | 68 | – |
per 1 mol of | −136.5 | −156.5 | 68 | – |
per 1 mol of | −68.25 | −78.25 | 34 | – |
per 1 mol of | −136.5 | −156.5 | 68 | – |
Changes in standard condition (2)
- Reaction of ammonium iodide 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 | −101.4 | – | – | – |
per 1 mol of | −101.4 | – | – | – |
per 1 mol of | −50.70 | – | – | – |
per 1 mol of | −101.4 | – | – | – |
per 1 mol of | −101.4 | – | – | – |
per 1 mol of | −50.70 | – | – | – |
per 1 mol of | −101.4 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium iodide and potassium permanganate◆
ΔrG −206.6 kJ/mol K 1.57 × 1036 pK −36.19
| 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 | −266.9 | −206.6 | −201.1 | – |
per 1 mol of | −266.9 | −206.6 | −201.1 | – |
per 1 mol of | −133.4 | −103.3 | −100.5 | – |
per 1 mol of | −266.9 | −206.6 | −201.1 | – |
per 1 mol of | −266.9 | −206.6 | −201.1 | – |
per 1 mol of | −133.4 | −103.3 | −100.5 | – |
per 1 mol of | −266.9 | −206.6 | −201.1 | – |
Changes in aqueous solution (2)
- Reaction of ammonium iodide and potassium permanganate◆
ΔrG −216.6 kJ/mol K 8.84 × 1037 pK −37.95
| 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 | −301.0 | −216.6 | −282.2 | – |
per 1 mol of | −301.0 | −216.6 | −282.2 | – |
per 1 mol of | −150.5 | −108.3 | −141.1 | – |
per 1 mol of | −301.0 | −216.6 | −282.2 | – |
per 1 mol of | −301.0 | −216.6 | −282.2 | – |
per 1 mol of | −150.5 | −108.3 | −141.1 | – |
per 1 mol of | −301.0 | −216.6 | −282.2 | – |
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 |
|---|---|---|---|---|
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[1] | – |
| KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
| KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[1] | – |
| MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
| MnO2 (am) precipitated | -502.5[1] | – | – | – |
| KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
| KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
| KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
| KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
| KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (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°, -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°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 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
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1