2HCrO4− → HO2− + 2CrO3 + H+ + 2e−
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- Oxidation of hydrogenchromate ion
- 2HCrO4−Hydrogenchromate ionHO2−Hydrogenperoxide ion + 2CrO3Chromium(VI) oxide + H+Hydrogen ion + 2e−Electron⟶
Oxidation of hydrogenchromate ion yields hydrogenperoxide ion, chromium(VI) oxide, hydrogen 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
- 2HCrO4−Hydrogenchromate ionHO2−Hydrogenperoxide ion + 2CrO3Chromium(VI) oxide + H+Hydrogen 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 | 2 | Reducing | – |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HO2− | Hydrogenperoxide ion | 1 | Oxidized | – |
| CrO3 | Chromium(VI) oxide | 2 | – | – |
| H+ | Hydrogen ion | 1 | – | – |
| e− | Electron | 2 | – | Electron |
Thermodynamic changes
Changes in standard condition
- Oxidation of hydrogenchromate ion
- 2HCrO4−Un-ionized aqueous solutionHO2−Un-ionized aqueous solution + 2CrO3Crystalline solid + 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 | 417.1 | – | – | – |
per 1 mol of Hydrogenchromate ion | 208.6 | – | – | – |
per 1 mol of Hydrogenperoxide ion | 417.1 | – | – | – |
per 1 mol of | 208.6 | – | – | – |
per 1 mol of Hydrogen ion | 417.1 | – | – | – |
per 1 mol of Electron | 208.6 | – | – | – |
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] | – |
| CrO3 (cr) | -589.5[1] | – | – | – |
| CrO3 (g) | -385.8[1] | – | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
| e− | – | – | – | – |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (g):Gas
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°, -589.5 kJ · mol−1
- ^ ΔfH°, -385.8 kJ · 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