NH4ClO4 🔥→ NH2OH + HClO + O2↑
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- Decomposition of ammonium perchlorate
Decomposition of ammonium perchlorate yields hydroxylamine, hypochlorous acid, 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 ammonium perchlorate
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 ammonium perchlorate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NH4ClO4 | Ammonium perchlorate | 1 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NH2OH | Hydroxylamine | 1 | Oxidized | – |
HClO | Hypochlorous acid | 1 | Reduced | – |
1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of ammonium perchlorate
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 | 42.6 | – | – | – |
per 1 mol of | 42.6 | – | – | – |
per 1 mol of Hydroxylamine | 42.6 | – | – | – |
per 1 mol of | 42.6 | – | – | – |
42.6 | – | – | – |
Changes in standard condition (2)
- Decomposition of ammonium perchlorate
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 | 30.9 | – | – | – |
per 1 mol of | 30.9 | – | – | – |
per 1 mol of Hydroxylamine | 30.9 | – | – | – |
per 1 mol of | 30.9 | – | – | – |
30.9 | – | – | – |
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 |
---|---|---|---|---|
NH4ClO4 (cr) | -295.31[1] | -88.75[1] | 186.2[1] | – |
NH4ClO4 (ai) | -261.83[1] | -87.83[1] | 295.4[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 |
---|---|---|---|---|
NH2OH (cr) | -114.2[1] | – | – | – |
NH2OH (aq) | -98.3[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) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
(ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (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°, -295.31 kJ · mol−1
- ^ ΔfG°, -88.75 kJ · mol−1
- ^ S°, 186.2 J · K−1 · mol−1
- ^ ΔfH°, -261.83 kJ · mol−1
- ^ ΔfG°, -87.83 kJ · mol−1
- ^ S°, 295.4 J · K−1 · mol−1
- ^ ΔfH°, -114.2 kJ · mol−1
- ^ ΔfH°, -98.3 kJ · 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°, 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