3NH4ClO3 🔥|️☀️→ 3NH3↑ + 3HClO + 2O3↑
Last updated:
- Decomposition of ammonium chlorate
Decomposition of ammonium chlorate yields ammonia, hypochlorous acid, and (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 ammonium 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
- Photolytic decomposition with redox
- Photolytically decomposable substanceSelf redox agent️☀️⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of ammonium chlorate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4ClO3 | Ammonium chlorate | 3 | Self redox agent | Thermally decomposable Oxoacid salt Photolytically decomposable |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH3 | Ammonia | 3 | – | – |
| HClO | Hypochlorous acid | 3 | Reduced | – |
| 2 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Decomposition of ammonium chlorate◆
ΔrG 299.1 kJ/mol K 0.40 × 10−52 pK 52.40
| 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 | 493.8 | 299.1 | 654 | – |
per 1 mol of | 164.6 | 99.70 | 218 | – |
per 1 mol of | 164.6 | 99.70 | 218 | – |
per 1 mol of | 164.6 | 99.70 | 218 | – |
| 246.9 | 149.6 | 327 | – |
Changes in aqueous solution (2)
- Decomposition of ammonium chlorate◆
ΔrG 320.9 kJ/mol K 0.60 × 10−56 pK 56.22
| 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 | 460.2 | 320.9 | 468 | – |
per 1 mol of | 153.4 | 107.0 | 156 | – |
per 1 mol of | 153.4 | 107.0 | 156 | – |
per 1 mol of | 153.4 | 107.0 | 156 | – |
| 230.1 | 160.4 | 234 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium chlorate◆
ΔrG 269.0 kJ/mol K 0.75 × 10−47 pK 47.13
| 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 | 391.3 | 269.0 | 411 | – |
per 1 mol of | 130.4 | 89.67 | 137 | – |
per 1 mol of | 130.4 | 89.67 | 137 | – |
per 1 mol of | 130.4 | 89.67 | 137 | – |
| 195.7 | 134.5 | 206 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium chlorate◆
ΔrG 290.8 kJ/mol K 0.11 × 10−50 pK 50.95
| 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 | 357.7 | 290.8 | 225 | – |
per 1 mol of | 119.2 | 96.93 | 75.0 | – |
per 1 mol of | 119.2 | 96.93 | 75.0 | – |
per 1 mol of | 119.2 | 96.93 | 75.0 | – |
| 178.8 | 145.4 | 113 | – |
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 |
|---|---|---|---|---|
| NH4ClO3 (ai) | -236.48[1] | -87.26[1] | 275.7[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 |
|---|---|---|---|---|
| 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] | – |
| HClO (g) | -78.7[1] | -66.1[1] | 236.67[1] | 37.15[1] |
| HClO (ao) | -120.9[1] | -79.9[1] | 142[1] | – |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (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°, -236.48 kJ · mol−1
- ^ ΔfG°, -87.26 kJ · mol−1
- ^ S°, 275.7 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°, -78.7 kJ · mol−1
- ^ ΔfG°, -66.1 kJ · mol−1
- ^ S°, 236.67 J · K−1 · mol−1
- ^ Cp°, 37.15 J · K−1 · mol−1
- ^ ΔfH°, -120.9 kJ · mol−1
- ^ ΔfG°, -79.9 kJ · mol−1
- ^ S°, 142. J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1