HO2− → O2 + H+ + 2e−
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Oxidation of hydrogenperoxide ion yields , hydrogen ion. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
General equation
- Oxidation of oxidizable species
- ReactantReducing agent ⟶ ProductOxidation product + e−
Oxidation state of each atom
- Oxidation of hydrogenperoxide ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HO2− | Hydrogenperoxide ion | 1 | Reducing | – |
Products
Thermodynamic changes
Changes in standard condition (1)
- Oxidation of hydrogenperoxide ion◆
ΔrG 67.3 kJ/mol K 0.16 × 10−11 pK 11.79 - HO2−Un-ionized aqueous solutionGas + H+Un-ionized aqueous solution + 2e−⟶
| 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 | 160.33 | 67.3 | 181.3 | – |
per 1 mol of Hydrogenperoxide ion | 160.33 | 67.3 | 181.3 | – |
| 160.33 | 67.3 | 181.3 | – | |
per 1 mol of Hydrogen ion | 160.33 | 67.3 | 181.3 | – |
per 1 mol of Electron | 80.165 | 33.6 | 90.65 | – |
Changes in standard condition (2)
- Oxidation of hydrogenperoxide ion◆
ΔrG 83.7 kJ/mol K 0.22 × 10−14 pK 14.66 - HO2−Un-ionized aqueous solutionUn-ionized aqueous solution + H+Un-ionized aqueous solution + 2e−⟶
| 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 | 148.6 | 83.7 | 87.1 | – |
per 1 mol of Hydrogenperoxide ion | 148.6 | 83.7 | 87.1 | – |
| 148.6 | 83.7 | 87.1 | – | |
per 1 mol of Hydrogen ion | 148.6 | 83.7 | 87.1 | – |
per 1 mol of Electron | 74.30 | 41.9 | 43.5 | – |
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 |
|---|---|---|---|---|
| HO2− (ao) | -160.33[1] | -67.3[1] | 23.8[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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
| e− | – | – | – | – |
* (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°, -160.33 kJ · mol−1
- ^ ΔfG°, -67.3 kJ · mol−1
- ^ S°, 23.8 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°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1