3HClO4 ⚡→ 3HClO3 + O3↑
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- Electrolysis of perchloric acid
Electrolysis of perchloric acid yields 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
- Electrolysis of perchloric acid
General equation
- Electrolysis of liquid substance
- LiquidSelf redox agent⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of perchloric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO4 | Perchloric acid | 3 | Self redox agent | Liquid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO3 | Chloric acid | 3 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Electrolysis of perchloric acid◆
ΔrG 164.9 kJ/mol K 0.13 × 10−28 pK 28.89
| 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 | 218.8 | 164.9 | 179.8 | – |
per 1 mol of | 72.93 | 54.97 | 59.93 | – |
per 1 mol of | 72.93 | 54.97 | 59.93 | – |
| 218.8 | 164.9 | 179.8 | – |
Changes in standard condition (2)
- Electrolysis of perchloric acid◆
ΔrG 175.8 kJ/mol K 0.16 × 10−30 pK 30.80
| 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 | 202.0 | 175.8 | 87 | – |
per 1 mol of | 67.33 | 58.60 | 29 | – |
per 1 mol of | 67.33 | 58.60 | 29 | – |
| 202.0 | 175.8 | 87 | – |
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 |
|---|---|---|---|---|
| HClO4 (l) | -40.58[1] | – | – | – |
| HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
| HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
| HClO4 (l) 2 hydrate | -677.98[1] | – | – | – |
* (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid
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 |
|---|---|---|---|---|
| HClO3 (ai) | -103.97[1] | -7.95[1] | 162.3[1] | – |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (ai):Ionized 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°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · mol−1
- ^ ΔfH°, -103.97 kJ · mol−1
- ^ ΔfG°, -7.95 kJ · mol−1
- ^ S°, 162.3 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