NH4ClO3 🔥|️☀️→ NH2OH + HClO2
Last updated:
- Decomposition of ammonium chlorate
Decomposition of ammonium chlorate yields hydroxylamine and chlorous acid (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 | 1 | Self redox agent | Thermally decomposable Oxoacid salt Photolytically decomposable |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH2OH | Hydroxylamine | 1 | Oxidized | – |
| HClO2 | Chlorous acid | 1 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution
- Decomposition of ammonium chlorate
| 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 | 86.3 | – | – | – |
per 1 mol of | 86.3 | – | – | – |
per 1 mol of Hydroxylamine | 86.3 | – | – | – |
per 1 mol of | 86.3 | – | – | – |
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 |
|---|---|---|---|---|
| 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 |
|---|---|---|---|---|
| NH2OH (cr) | -114.2[1] | – | – | – |
| NH2OH (aq) | -98.3[1] | – | – | – |
| HClO2 (ao) | -51.9[1] | 5.9[1] | 188.3[1] | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (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)