2KClO3 🔥→ K2O + Cl2O↑ + 2O2↑
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- Decomposition of potassium chlorate
Decomposition of potassium chlorate yields potassium oxide, dichlorine monoxide, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of potassium chlorate
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
Oxidation state of each atom
- Decomposition of potassium chlorate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO3 | Potassium chlorate | 2 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 1 | – | – |
| Cl2O | Dichlorine monoxide | 1 | Reduced | – |
| 2 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Decomposition of potassium chlorate◆
ΔrG 368.3 kJ/mol K 0.30 × 10−64 pK 64.52
| 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 | 514.3 | 368.3 | 484.4 | −12.7 |
per 1 mol of | 257.1 | 184.2 | 242.2 | −6.35 |
per 1 mol of | 514.3 | 368.3 | 484.4 | −12.7 |
per 1 mol of | 514.3 | 368.3 | 484.4 | −12.7 |
| 257.1 | 184.2 | 242.2 | −6.35 |
Changes in aqueous solution (1)
- Decomposition of potassium chlorate◆
ΔrG 358.2 kJ/mol K 0.18 × 10−62 pK 62.75
| 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 | 431.5 | 358.2 | 241.0 | – |
per 1 mol of | 215.8 | 179.1 | 120.5 | – |
per 1 mol of | 431.5 | 358.2 | 241.0 | – |
per 1 mol of | 431.5 | 358.2 | 241.0 | – |
| 215.8 | 179.1 | 120.5 | – |
Changes in aqueous solution (2)
- Decomposition of potassium chlorate◆
ΔrG 391.0 kJ/mol K 0.32 × 10−68 pK 68.50
| 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 | 408.1 | 391.0 | 52.5 | – |
per 1 mol of | 204.1 | 195.5 | 26.3 | – |
per 1 mol of | 408.1 | 391.0 | 52.5 | – |
per 1 mol of | 408.1 | 391.0 | 52.5 | – |
| 204.1 | 195.5 | 26.3 | – |
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 |
|---|---|---|---|---|
| KClO3 (cr) | -397.73[1] | -296.25[1] | 143.1[1] | 100.25[1] |
| KClO3 (ai) | -356.35[1] | -291.22[1] | 264.8[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 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| Cl2O (g) | 80.3[1] | 97.9[1] | 266.21[1] | 45.40[1] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (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°, -397.73 kJ · mol−1
- ^ ΔfG°, -296.25 kJ · mol−1
- ^ S°, 143.1 J · K−1 · mol−1
- ^ Cp°, 100.25 J · K−1 · mol−1
- ^ ΔfH°, -356.35 kJ · mol−1
- ^ ΔfG°, -291.22 kJ · mol−1
- ^ S°, 264.8 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280