10HCrO4− → HO2− + 5Cr2O72− + 3H3O+ + 2e−
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- Oxidation of hydrogenchromate ion
- 10HCrO4−Hydrogenchromate ionHO2−Hydrogenperoxide ion + 5Cr2O72−Dichromate ion + 3H3O+Hydronium ion + 2e−Electron⟶
Oxidation of hydrogenchromate ion yields hydrogenperoxide ion, dichromate ion, hydronium ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Oxidation of hydrogenchromate ion
- 10HCrO4−Hydrogenchromate ionHO2−Hydrogenperoxide ion + 5Cr2O72−Dichromate ion + 3H3O+Hydronium ion + 2e−Electron⟶
General equation
- Oxidation of oxidizable species
- ReactantReducing agent ⟶ ProductOxidation product + e−
Oxidation state of each atom
- Oxidation of hydrogenchromate ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCrO4− | Hydrogenchromate ion | 10 | Reducing | – |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HO2− | Hydrogenperoxide ion | 1 | Oxidized | – |
| Cr2O72− | Dichromate ion | 5 | – | – |
| H3O+ | Hydronium ion | 3 | – | – |
| e− | Electron | 2 | – | Electron |
Thermodynamic changes
Changes in standard condition
- Oxidation of hydrogenchromate ion◆
ΔrG 362.8 kJ/mol K 0.28 × 10−63 pK 63.56 - 10HCrO4−Un-ionized aqueous solutionHO2−Un-ionized aqueous solution + 5Cr2O72−Un-ionized aqueous solution + 3H3O+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 | 312.7 | 362.8 | −298.0 | – |
per 1 mol of Hydrogenchromate ion | 31.27 | 36.28 | −29.80 | – |
per 1 mol of Hydrogenperoxide ion | 312.7 | 362.8 | −298.0 | – |
per 1 mol of Dichromate ion | 62.54 | 72.56 | −59.60 | – |
per 1 mol of Hydronium ion | 104.2 | 120.9 | −99.33 | – |
per 1 mol of Electron | 156.3 | 181.4 | −149.0 | – |
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 |
|---|---|---|---|---|
| HCrO4− (ao) | -878.2[1] | -764.7[1] | 184.1[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 |
|---|---|---|---|---|
| HO2− (ao) | -160.33[1] | -67.3[1] | 23.8[1] | – |
| Cr2O72− (ao) | -1490.3[1] | -1301.1[1] | 261.9[1] | – |
| H3O+ (ao) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| e− | – | – | – | – |
* (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°, -878.2 kJ · mol−1
- ^ ΔfG°, -764.7 kJ · mol−1
- ^ S°, 184.1 J · K−1 · mol−1
- ^ ΔfH°, -160.33 kJ · mol−1
- ^ ΔfG°, -67.3 kJ · mol−1
- ^ S°, 23.8 J · K−1 · mol−1
- ^ ΔfH°, -1490.3 kJ · mol−1
- ^ ΔfG°, -1301.1 kJ · mol−1
- ^ S°, 261.9 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1