12HSO3− + 10e− → S22− + 6H2O + 10SO32−
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Reduction of hydrogensulfurous ion yields disulfide ion, water, and sulfurous ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of hydrogensulfurous ion
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of hydrogensulfurous ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HSO3− | Hydrogensulfurous ion | 12 | Oxidizing | – |
| e− | Electron | 10 | – | Electron |
Products
Thermodynamic changes
Changes in standard condition
- Reduction of hydrogensulfurous ion◆
ΔrG 124.5 kJ/mol K 0.15 × 10−21 pK 21.81 - 12HSO3−Un-ionized aqueous solution + 10e−S22−Un-ionized aqueous solution + 6H2OLiquid + 10SO32−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 | −525.2 | 124.5 | −1518 | – |
per 1 mol of Hydrogensulfurous ion | −43.77 | 10.38 | −126.5 | – |
per 1 mol of Electron | −52.52 | 12.45 | −151.8 | – |
per 1 mol of Disulfide ion | −525.2 | 124.5 | −1518 | – |
per 1 mol of | −87.53 | 20.75 | −253.0 | – |
per 1 mol of Sulfurous ion | −52.52 | 12.45 | −151.8 | – |
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 |
|---|---|---|---|---|
| HSO3− (ao) | -626.22[1] | -527.73[1] | 139.7[1] | – |
| e− | – | – | – | – |
* (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 |
|---|---|---|---|---|
| S22− (ao) | 30.1[1] | 79.5[1] | 28.5[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
| SO32− (ao) | -635.5[1] | -486.5[1] | -29[1] | – |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (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°, -626.22 kJ · mol−1
- ^ ΔfG°, -527.73 kJ · mol−1
- ^ S°, 139.7 J · K−1 · mol−1
- ^ ΔfH°, 30.1 kJ · mol−1
- ^ ΔfG°, 79.5 kJ · mol−1
- ^ S°, 28.5 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
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, -635.5 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, -29. J · K−1 · mol−1