6NH4ClO3 🔥|️☀️→ 6NO2↑ + 3Cl2O↑ + 12H2↑ + O3↑
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- Decomposition of ammonium chlorate
Decomposition of ammonium chlorate yields nitrogen dioxide, dichlorine monoxide, , 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 | 6 | Self redox agent | Thermally decomposable Oxoacid salt Photolytically decomposable |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NO2 | Nitrogen dioxide | 6 | Oxidized | – |
| Cl2O | Dichlorine monoxide | 3 | Reduced | – |
| 12 | Reduced | – | ||
| 1 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Decomposition of ammonium chlorate◆
ΔrG 1288.3 kJ/mol K 0.20 × 10−225 pK 225.70
| 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 | 2001.6 | 1288.3 | 2391.9 | – |
per 1 mol of | 333.60 | 214.72 | 398.65 | – |
per 1 mol of | 333.60 | 214.72 | 398.65 | – |
per 1 mol of | 667.20 | 429.43 | 797.30 | – |
| 166.80 | 107.36 | 199.33 | – | |
| 2001.6 | 1288.3 | 2391.9 | – |
Changes in aqueous solution (2)
- Decomposition of ammonium chlorate◆
ΔrG 1299.2 kJ/mol K 0.25 × 10−227 pK 227.61
| 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 | 1984.8 | 1299.2 | 2299 | – |
per 1 mol of | 330.80 | 216.53 | 383.2 | – |
per 1 mol of | 330.80 | 216.53 | 383.2 | – |
per 1 mol of | 661.60 | 433.07 | 766.3 | – |
| 165.40 | 108.27 | 191.6 | – | |
| 1984.8 | 1299.2 | 2299 | – |
Changes in aqueous solution (3)
- Decomposition of ammonium chlorate◆
ΔrG 1499.5 kJ/mol K 0.20 × 10−262 pK 262.70
| 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 | 1951.2 | 1499.5 | 7748 | – |
per 1 mol of | 325.20 | 249.92 | 1291 | – |
per 1 mol of | 325.20 | 249.92 | 1291 | – |
per 1 mol of | 650.40 | 499.83 | 2583 | – |
| 162.60 | 124.96 | 645.7 | – | |
| 1951.2 | 1499.5 | 7748 | – |
Changes in aqueous solution (4)
- Decomposition of ammonium chlorate◆
ΔrG 1510.4 kJ/mol K 0.25 × 10−264 pK 264.61
| 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 | 1934.4 | 1510.4 | 7655 | – |
per 1 mol of | 322.40 | 251.73 | 1276 | – |
per 1 mol of | 322.40 | 251.73 | 1276 | – |
per 1 mol of | 644.80 | 503.47 | 2552 | – |
| 161.20 | 125.87 | 637.9 | – | |
| 1934.4 | 1510.4 | 7655 | – |
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 |
|---|---|---|---|---|
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[1] |
| Cl2O (g) | 80.3[1] | 97.9[1] | 266.21[1] | 45.40[1] |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[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°, 33.18 kJ · mol−1
- ^ ΔfG°, 51.31 kJ · mol−1
- ^ S°, 240.06 J · K−1 · mol−1
- ^ Cp°, 37.20 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 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