5ZnI2 + 2KMnO4 + 6H2O → 5Zn(OH)2 + 5I2 + 2MnO + 2KOH
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- Reaction of zinc iodide and potassium permanganate under neutral condition
The reaction of zinc iodide, potassium permanganate, and water yields zinc hydroxide, , manganese(II) 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 zinc iodide and potassium permanganate under neutral condition
General equation
- Reaction of oxidizable species and oxidizing species under neutral condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of zinc iodide and potassium permanganate under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnI2 | Zinc iodide | 5 | Reducing | Oxidizable |
| KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
| H2O | Water | 6 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn(OH)2 | Zinc hydroxide | 5 | – | – |
| 5 | Oxidized | – | ||
| MnO | Manganese(II) oxide | 2 | Reduced | – |
| KOH | Potassium hydroxide | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −310.3 kJ/mol K 2.30 × 1054 pK −54.36
| 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 | – | −310.3 | – | – |
per 1 mol of | – | −62.06 | – | – |
per 1 mol of | – | −155.2 | – | – |
per 1 mol of | – | −51.72 | – | – |
per 1 mol of | – | −62.06 | – | – |
| – | −62.06 | – | – | |
per 1 mol of | – | −155.2 | – | – |
per 1 mol of | – | −155.2 | – | – |
Changes in standard condition (2)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −308.8 kJ/mol K 1.26 × 1054 pK −54.10
| 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 | −400.0 | −308.8 | −304.5 | – |
per 1 mol of | −80.00 | −61.76 | −60.90 | – |
per 1 mol of | −200.0 | −154.4 | −152.3 | – |
per 1 mol of | −66.67 | −51.47 | −50.75 | – |
per 1 mol of | −80.00 | −61.76 | −60.90 | – |
| −80.00 | −61.76 | −60.90 | – | |
per 1 mol of | −200.0 | −154.4 | −152.3 | – |
per 1 mol of | −200.0 | −154.4 | −152.3 | – |
Changes in standard condition (3)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −316.6 kJ/mol K 2.92 × 1055 pK −55.47
| 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 | −406.7 | −316.6 | −302.5 | – |
per 1 mol of | −81.34 | −63.32 | −60.50 | – |
per 1 mol of | −203.3 | −158.3 | −151.3 | – |
per 1 mol of | −67.78 | −52.77 | −50.42 | – |
per 1 mol of | −81.34 | −63.32 | −60.50 | – |
| −81.34 | −63.32 | −60.50 | – | |
per 1 mol of | −203.3 | −158.3 | −151.3 | – |
per 1 mol of | −203.3 | −158.3 | −151.3 | – |
Changes in standard condition (4)
- Reaction of zinc iodide and potassium permanganate under neutral condition
| 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 | −401.4 | – | – | – |
per 1 mol of | −80.28 | – | – | – |
per 1 mol of | −200.7 | – | – | – |
per 1 mol of | −66.90 | – | – | – |
per 1 mol of | −80.28 | – | – | – |
| −80.28 | – | – | – | |
per 1 mol of | −200.7 | – | – | – |
per 1 mol of | −200.7 | – | – | – |
Changes in aqueous solution (1)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −3.7 kJ/mol K 4.45 × 100 pK −0.65
| 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 | – | −3.7 | – | – |
per 1 mol of | – | −0.74 | – | – |
per 1 mol of | – | −1.9 | – | – |
per 1 mol of | – | −0.62 | – | – |
per 1 mol of | – | −0.74 | – | – |
| – | −0.74 | – | – | |
per 1 mol of | – | −1.9 | – | – |
per 1 mol of | – | −1.9 | – | – |
Changes in aqueous solution (2)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −159.1 kJ/mol K 7.47 × 1027 pK −27.87
| 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 | – | −159.1 | – | – |
per 1 mol of | – | −31.82 | – | – |
per 1 mol of | – | −79.55 | – | – |
per 1 mol of | – | −26.52 | – | – |
per 1 mol of | – | −31.82 | – | – |
| – | −31.82 | – | – | |
per 1 mol of | – | −79.55 | – | – |
per 1 mol of | – | −79.55 | – | – |
Changes in aqueous solution (3)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −157.6 kJ/mol K 4.08 × 1027 pK −27.61
| 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 | −207.9 | −157.6 | −164.7 | – |
per 1 mol of | −41.58 | −31.52 | −32.94 | – |
per 1 mol of | −104.0 | −78.80 | −82.35 | – |
per 1 mol of | −34.65 | −26.27 | −27.45 | – |
per 1 mol of | −41.58 | −31.52 | −32.94 | – |
| −41.58 | −31.52 | −32.94 | – | |
per 1 mol of | −104.0 | −78.80 | −82.35 | – |
per 1 mol of | −104.0 | −78.80 | −82.35 | – |
Changes in aqueous solution (4)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −165.4 kJ/mol K 9.48 × 1028 pK −28.98
| 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 | −214.6 | −165.4 | −162.7 | – |
per 1 mol of | −42.92 | −33.08 | −32.54 | – |
per 1 mol of | −107.3 | −82.70 | −81.35 | – |
per 1 mol of | −35.77 | −27.57 | −27.12 | – |
per 1 mol of | −42.92 | −33.08 | −32.54 | – |
| −42.92 | −33.08 | −32.54 | – | |
per 1 mol of | −107.3 | −82.70 | −81.35 | – |
per 1 mol of | −107.3 | −82.70 | −81.35 | – |
Changes in aqueous solution (5)
- Reaction of zinc iodide and potassium permanganate under neutral condition
| 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 | −209.3 | – | – | – |
per 1 mol of | −41.86 | – | – | – |
per 1 mol of | −104.7 | – | – | – |
per 1 mol of | −34.88 | – | – | – |
per 1 mol of | −41.86 | – | – | – |
| −41.86 | – | – | – | |
per 1 mol of | −104.7 | – | – | – |
per 1 mol of | −104.7 | – | – | – |
Changes in aqueous solution (6)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −51.7 kJ/mol K 1.14 × 109 pK −9.06
| 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 | – | −51.7 | – | – |
per 1 mol of | – | −10.3 | – | – |
per 1 mol of | – | −25.9 | – | – |
per 1 mol of | – | −8.62 | – | – |
per 1 mol of | – | −10.3 | – | – |
| – | −10.3 | – | – | |
per 1 mol of | – | −25.9 | – | – |
per 1 mol of | – | −25.9 | – | – |
Changes in aqueous solution (7)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −207.1 kJ/mol K 1.92 × 1036 pK −36.28
| 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 | – | −207.1 | – | – |
per 1 mol of | – | −41.42 | – | – |
per 1 mol of | – | −103.5 | – | – |
per 1 mol of | – | −34.52 | – | – |
per 1 mol of | – | −41.42 | – | – |
| – | −41.42 | – | – | |
per 1 mol of | – | −103.5 | – | – |
per 1 mol of | – | −103.5 | – | – |
Changes in aqueous solution (8)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −205.6 kJ/mol K 1.05 × 1036 pK −36.02
| 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 | – | −205.6 | – | – |
per 1 mol of | – | −41.12 | – | – |
per 1 mol of | – | −102.8 | – | – |
per 1 mol of | – | −34.27 | – | – |
per 1 mol of | – | −41.12 | – | – |
| – | −41.12 | – | – | |
per 1 mol of | – | −102.8 | – | – |
per 1 mol of | – | −102.8 | – | – |
Changes in aqueous solution (9)
- Reaction of zinc iodide and potassium permanganate under neutral condition◆
ΔrG −213.4 kJ/mol K 2.43 × 1037 pK −37.39
| 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 | – | −213.4 | – | – |
per 1 mol of | – | −42.68 | – | – |
per 1 mol of | – | −106.7 | – | – |
per 1 mol of | – | −35.57 | – | – |
per 1 mol of | – | −42.68 | – | – |
| – | −42.68 | – | – | |
per 1 mol of | – | −106.7 | – | – |
per 1 mol of | – | −106.7 | – | – |
Changes in aqueous solution (10)
- Reaction of zinc iodide and potassium permanganate under neutral condition
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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 |
|---|---|---|---|---|
| ZnI2 (cr) | -208.03[1] | -208.95[1] | 161.1[1] | – |
| ZnI2 (ai) | -264.26[1] | -250.20[1] | 110.5[1] | -238[1] |
| ZnI2 (ao) | – | -240.6[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] |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| Zn(OH)2 (cr) γ | – | -553.81[1] | – | – |
| Zn(OH)2 (cr) β | -641.91[1] | -553.52[1] | 81.2[1] | – |
| Zn(OH)2 (cr) ε | -643.25[1] | -555.07[1] | 81.6[1] | 72.4[1] |
| Zn(OH)2 (cr) precipitated | -642.2[1] | – | – | – |
| Zn(OH)2 (ai) | -613.88[1] | -461.56[1] | -133.5[1] | -251[1] |
| Zn(OH)2 (ao) | – | -522.73[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] | – |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[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] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas
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°, -208.03 kJ · mol−1
- ^ ΔfG°, -208.95 kJ · mol−1
- ^ S°, 161.1 J · K−1 · mol−1
- ^ ΔfH°, -264.26 kJ · mol−1
- ^ ΔfG°, -250.20 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, -238. J · K−1 · mol−1
- ^ ΔfG°, -240.6 kJ · 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°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfG°, -553.81 kJ · mol−1
- ^ ΔfH°, -641.91 kJ · mol−1
- ^ ΔfG°, -553.52 kJ · mol−1
- ^ S°, 81.2 J · K−1 · mol−1
- ^ ΔfH°, -643.25 kJ · mol−1
- ^ ΔfG°, -555.07 kJ · mol−1
- ^ S°, 81.6 J · K−1 · mol−1
- ^ Cp°, 72.4 J · K−1 · mol−1
- ^ ΔfH°, -642.2 kJ · mol−1
- ^ ΔfH°, -613.88 kJ · mol−1
- ^ ΔfG°, -461.56 kJ · mol−1
- ^ S°, -133.5 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfG°, -522.73 kJ · 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
- ^ ΔfH°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 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