2KClO 🔥|️☀️→ KClO2 + KCl
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- Decomposition of potassium hypochlorite
Decomposition of potassium hypochlorite yields potassium chlorite and potassium chloride (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
- Thermal decomposition with redox
- Thermal decomposition of oxoacid salt with redox
- Photolytic decomposition with redox
Table of contents
Reaction data
Chemical equation
- Decomposition of potassium hypochlorite
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Photolytic decomposition with redox
- Photolytically decomposable substanceSelf redox agent️☀️⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of potassium hypochlorite
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO | Potassium hypochlorite | 2 | – | Thermally decomposable Oxoacid salt Photolytically decomposable |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO2 | Potassium chlorite | 1 | Oxidized | – |
| KCl | Potassium chloride | 1 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution
- Decomposition of potassium hypochlorite◆
ΔrG −40.6 kJ/mol K 1.30 × 107 pK −7.11
| 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 | −19.5 | −40.6 | 71 | – |
per 1 mol of | −9.75 | −20.3 | 36 | – |
per 1 mol of | −19.5 | −40.6 | 71 | – |
per 1 mol of | −19.5 | −40.6 | 71 | – |
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 |
|---|---|---|---|---|
| KClO (ai) | -359.4[1] | -320.0[1] | 146[1] | – |
* (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 |
|---|---|---|---|---|
| KClO2 (ai) | -318.8[1] | -266.1[1] | 203.8[1] | – |
| KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
| KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
| KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[1] |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (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°, -359.4 kJ · mol−1
- ^ ΔfG°, -320.0 kJ · mol−1
- ^ S°, 146. 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°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1