2HClO 💧⚡→ Cl2↑ + O2↑ + H2↑
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- Electrolysis of aqueous hypochlorous acid without water as reactant
Electrolysis of aqueous hypochlorous acid yields , , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous hypochlorous acid without water as reactant
General equation
- Electrolysis of aqueous solution without water as reactant
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous hypochlorous acid without water as reactant
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO | Hypochlorous acid | 2 | Self redox agent | Soluble in water |
Products
Thermodynamic changes
Changes in standard condition (1)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 159.8 kJ/mol K 0.10 × 10−27 pK 28.00
| 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 | 241.8 | 159.8 | 275 | – |
per 1 mol of | 120.9 | 79.90 | 138 | – |
| 241.8 | 159.8 | 275 | – | |
| 241.8 | 159.8 | 275 | – | |
| 241.8 | 159.8 | 275 | – |
Changes in standard condition (2)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 177.4 kJ/mol K 0.83 × 10−31 pK 31.08
| 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 | 237.6 | 177.4 | 721 | – |
per 1 mol of | 118.8 | 88.70 | 361 | – |
| 237.6 | 177.4 | 721 | – | |
| 237.6 | 177.4 | 721 | – | |
| 237.6 | 177.4 | 721 | – |
Changes in standard condition (3)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 176.2 kJ/mol K 0.14 × 10−30 pK 30.87
| 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 | 230.1 | 176.2 | 181 | – |
per 1 mol of | 115.0 | 88.10 | 90.5 | – |
| 230.1 | 176.2 | 181 | – | |
| 230.1 | 176.2 | 181 | – | |
| 230.1 | 176.2 | 181 | – |
Changes in standard condition (4)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 193.8 kJ/mol K 0.11 × 10−33 pK 33.95 - 2HClOUn-ionized aqueous solution↑Gas + ↑Un-ionized aqueous solution + ↑Un-ionized aqueous solution💧⚡⟶
| 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 | 225.9 | 193.8 | 627 | – |
per 1 mol of | 113.0 | 96.90 | 314 | – |
| 225.9 | 193.8 | 627 | – | |
| 225.9 | 193.8 | 627 | – | |
| 225.9 | 193.8 | 627 | – |
Changes in standard condition (5)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 166.7 kJ/mol K 0.62 × 10−29 pK 29.20
| 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 | 218.4 | 166.7 | 173 | – |
per 1 mol of | 109.2 | 83.35 | 86.5 | – |
| 218.4 | 166.7 | 173 | – | |
| 218.4 | 166.7 | 173 | – | |
| 218.4 | 166.7 | 173 | – |
Changes in standard condition (6)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 184.3 kJ/mol K 0.52 × 10−32 pK 32.29 - 2HClOUn-ionized aqueous solution↑Un-ionized aqueous solution + ↑Gas + ↑Un-ionized aqueous solution💧⚡⟶
| 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 | 214.2 | 184.3 | 619 | – |
per 1 mol of | 107.1 | 92.15 | 310 | – |
| 214.2 | 184.3 | 619 | – | |
| 214.2 | 184.3 | 619 | – | |
| 214.2 | 184.3 | 619 | – |
Changes in standard condition (7)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 183.1 kJ/mol K 0.84 × 10−32 pK 32.08 - 2HClOUn-ionized aqueous solution↑Un-ionized aqueous solution + ↑Un-ionized aqueous solution + ↑Gas💧⚡⟶
| 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 | 206.7 | 183.1 | 79 | – |
per 1 mol of | 103.3 | 91.55 | 40 | – |
| 206.7 | 183.1 | 79 | – | |
| 206.7 | 183.1 | 79 | – | |
| 206.7 | 183.1 | 79 | – |
Changes in standard condition (8)
- Electrolysis of aqueous hypochlorous acid without water as reactant◆
ΔrG 200.7 kJ/mol K 0.69 × 10−35 pK 35.16 - 2HClOUn-ionized aqueous solution↑Un-ionized aqueous solution + ↑Un-ionized aqueous solution + ↑Un-ionized aqueous solution💧⚡⟶
| 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 | 202.5 | 200.7 | 525 | – |
per 1 mol of | 101.3 | 100.3 | 263 | – |
| 202.5 | 200.7 | 525 | – | |
| 202.5 | 200.7 | 525 | – | |
| 202.5 | 200.7 | 525 | – |
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 |
|---|---|---|---|---|
| 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):Gas, (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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[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°, -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°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. 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
- ^ 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