2NH4ClO4 🔥→ 2NH3↑ + 2HClO3 + O2↑
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- Decomposition of ammonium perchlorate
Decomposition of ammonium perchlorate yields ammonia, chloric 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 | 2 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH3 | Ammonia | 2 | – | – |
| HClO3 | Chloric acid | 2 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of ammonium perchlorate◆
ΔrG 126.86 kJ/mol K 0.60 × 10−22 pK 22.22
| 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 | 223.50 | 126.86 | 323.8 | – |
per 1 mol of | 111.75 | 63.430 | 161.9 | – |
per 1 mol of | 111.75 | 63.430 | 161.9 | – |
per 1 mol of | 111.75 | 63.430 | 161.9 | – |
| 223.50 | 126.86 | 323.8 | – |
Changes in standard condition (2)
- Decomposition of ammonium perchlorate◆
ΔrG 143.3 kJ/mol K 0.79 × 10−25 pK 25.11
| 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 | 211.8 | 143.3 | 229.6 | – |
per 1 mol of | 105.9 | 71.65 | 114.8 | – |
per 1 mol of | 105.9 | 71.65 | 114.8 | – |
per 1 mol of | 105.9 | 71.65 | 114.8 | – |
| 211.8 | 143.3 | 229.6 | – |
Changes in standard condition (3)
- Decomposition of ammonium perchlorate◆
ΔrG 106.76 kJ/mol K 0.20 × 10−18 pK 18.70
| 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 | 155.14 | 106.76 | 161.5 | – |
per 1 mol of | 77.570 | 53.380 | 80.75 | – |
per 1 mol of | 77.570 | 53.380 | 80.75 | – |
per 1 mol of | 77.570 | 53.380 | 80.75 | – |
| 155.14 | 106.76 | 161.5 | – |
Changes in standard condition (4)
- Decomposition of ammonium perchlorate◆
ΔrG 123.2 kJ/mol K 0.26 × 10−21 pK 21.58
| 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 | 143.4 | 123.2 | 67.3 | – |
per 1 mol of | 71.70 | 61.60 | 33.6 | – |
per 1 mol of | 71.70 | 61.60 | 33.6 | – |
per 1 mol of | 71.70 | 61.60 | 33.6 | – |
| 143.4 | 123.2 | 67.3 | – |
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 |
|---|---|---|---|---|
| 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 |
|---|---|---|---|---|
| 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] | – |
| HClO3 (ai) | -103.97[1] | -7.95[1] | 162.3[1] | – |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (ai):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°, -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°, -103.97 kJ · mol−1
- ^ ΔfG°, -7.95 kJ · mol−1
- ^ S°, 162.3 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