3HClO2 🔥|🕒→ 3HClO + O3↑
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- Decomposition of chlorous acid
Decomposition of chlorous acid yields 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 chlorous acid
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Spontaneous decomposition with redox
- Spontaneously decomposable substanceSelf redox agent🕒⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of chlorous acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO2 | Chlorous acid | 3 | Self redox agent | Thermally decomposable Spontaneously decomposable |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO | Hypochlorous acid | 3 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of chlorous acid◆
ΔrG −94.2 kJ/mol K 3.19 × 1016 pK −16.50
| 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 | −64.3 | −94.2 | 100 | – |
per 1 mol of | −21.4 | −31.4 | 33.3 | – |
per 1 mol of | −21.4 | −31.4 | 33.3 | – |
| −64.3 | −94.2 | 100 | – |
Changes in standard condition (2)
- Decomposition of chlorous acid◆
ΔrG −83.3 kJ/mol K 3.92 × 1014 pK −14.59
| 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 | −81.1 | −83.3 | 7 | – |
per 1 mol of | −27.0 | −27.8 | 2 | – |
per 1 mol of | −27.0 | −27.8 | 2 | – |
| −81.1 | −83.3 | 7 | – |
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 |
|---|---|---|---|---|
| HClO2 (ao) | -51.9[1] | 5.9[1] | 188.3[1] | – |
* (ao):Un-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 |
|---|---|---|---|---|
| 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°, -51.9 kJ · mol−1
- ^ ΔfG°, 5.9 kJ · mol−1
- ^ S°, 188.3 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