3KI + 6KClO2 + 7H+ → 2KIO3 + 7K+ + 3Cl2O↑ + 3H2O + HI↑
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- Reaction of potassium iodide and potassium chlorite under acidic condition
- 3KIPotassium iodide + 6KClO2Potassium chlorite + 7H+Hydrogen ion2KIO3Potassium iodate + 7K+Potassium ion + 3Cl2O↑Dichlorine monoxide + 3H2OWater + HI↑Hydrogen iodide⟶
The reaction of potassium iodide, potassium chlorite, and hydrogen ion yields potassium iodate, potassium ion, dichlorine monoxide, water, and hydrogen iodide (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 potassium iodide and potassium chlorite under acidic condition
- 3KIPotassium iodide + 6KClO2Potassium chlorite + 7H+Hydrogen ion2KIO3Potassium iodate + 7K+Potassium ion + 3Cl2O↑Dichlorine monoxide + 3H2OWater + HI↑Hydrogen iodide⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of potassium iodide and potassium chlorite under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 3 | Reducing | Oxidizable |
| KClO2 | Potassium chlorite | 6 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 7 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 2 | Oxidized | – |
| K+ | Potassium ion | 7 | – | – |
| Cl2O | Dichlorine monoxide | 3 | Reduced | – |
| H2O | Water | 3 | – | Water |
| HI | Hydrogen iodide | 1 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium iodide and potassium chlorite under acidic condition◆
ΔrG −620.1 kJ/mol K 4.33 × 10108 pK −108.64
| 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 | −468.5 | −620.1 | 510.1 | – |
per 1 mol of | −156.2 | −206.7 | 170.0 | – |
per 1 mol of | −78.08 | −103.4 | 85.02 | – |
per 1 mol of Hydrogen ion | −66.93 | −88.59 | 72.87 | – |
per 1 mol of | −234.3 | −310.1 | 255.1 | – |
per 1 mol of Potassium ion | −66.93 | −88.59 | 72.87 | – |
per 1 mol of | −156.2 | −206.7 | 170.0 | – |
per 1 mol of | −156.2 | −206.7 | 170.0 | – |
per 1 mol of | −468.5 | −620.1 | 510.1 | – |
Changes in aqueous solution (2)
- Reaction of potassium iodide and potassium chlorite under acidic condition◆
ΔrG −673.4 kJ/mol K 9.43 × 10117 pK −117.97
| 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 | −550.1 | −673.4 | 414.8 | – |
per 1 mol of | −183.4 | −224.5 | 138.3 | – |
per 1 mol of | −91.68 | −112.2 | 69.13 | – |
per 1 mol of Hydrogen ion | −78.59 | −96.20 | 59.26 | – |
per 1 mol of | −275.1 | −336.7 | 207.4 | – |
per 1 mol of Potassium ion | −78.59 | −96.20 | 59.26 | – |
per 1 mol of | −183.4 | −224.5 | 138.3 | – |
per 1 mol of | −183.4 | −224.5 | 138.3 | – |
per 1 mol of | −550.1 | −673.4 | 414.8 | – |
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 |
|---|---|---|---|---|
| KI (cr) | -327.900[1] | -324.892[1] | 106.32[1] | 52.93[1] |
| KI (g) | -125.5[1] | -166.1[1] | 258.3[1] | 37.11[1] |
| KI (ai) | -307.57[1] | -334.85[1] | 213.8[1] | -120.5[1] |
| KClO2 (ai) | -318.8[1] | -266.1[1] | 203.8[1] | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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 |
|---|---|---|---|---|
| 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] | – |
| K+ (g) | 514.26[1] | – | – | – |
| K+ (ao) | -252.38[1] | -283.27[1] | 102.5[1] | 21.8[1] |
| Cl2O (g) | 80.3[1] | 97.9[1] | 266.21[1] | 45.40[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] |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -327.900 kJ · mol−1
- ^ ΔfG°, -324.892 kJ · mol−1
- ^ S°, 106.32 J · K−1 · mol−1
- ^ Cp°, 52.93 J · K−1 · mol−1
- ^ ΔfH°, -125.5 kJ · mol−1
- ^ ΔfG°, -166.1 kJ · mol−1
- ^ S°, 258.3 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -307.57 kJ · mol−1
- ^ ΔfG°, -334.85 kJ · mol−1
- ^ S°, 213.8 J · K−1 · mol−1
- ^ Cp°, -120.5 J · K−1 · mol−1
- ^ ΔfH°, -318.8 kJ · mol−1
- ^ ΔfG°, -266.1 kJ · mol−1
- ^ S°, 203.8 J · K−1 · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 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°, 514.26 kJ · mol−1
- ^ ΔfH°, -252.38 kJ · mol−1
- ^ ΔfG°, -283.27 kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 21.8 J · K−1 · mol−1
- ^ ΔfH°, 80.3 kJ · mol−1
- ^ ΔfG°, 97.9 kJ · mol−1
- ^ S°, 266.21 J · K−1 · mol−1
- ^ Cp°, 45.40 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
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1