13NaHSO4 + 8e− → NaHS + 12NaSO4− + 4H3O+
Last updated:
- Reduction of sodium hydrogensulfate
- 13NaHSO4Sodium hydrogensulfate + 8e−ElectronNaHSSodium hydrogensulfide + 12NaSO4−Sodium sulfate ion + 4H3O+Hydronium ion⟶
Reduction of sodium hydrogensulfate yields sodium hydrogensulfide, sodium sulfate ion, and 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
- Reduction of sodium hydrogensulfate
- 13NaHSO4Sodium hydrogensulfate + 8e−ElectronNaHSSodium hydrogensulfide + 12NaSO4−Sodium sulfate ion + 4H3O+Hydronium ion⟶
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of sodium hydrogensulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHSO4 | Sodium hydrogensulfate | 13 | Oxidizing | – |
| e− | Electron | 8 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHS | Sodium hydrogensulfide | 1 | Reduced | – |
| NaSO4− | Sodium sulfate ion | 12 | – | – |
| H3O+ | Hydronium ion | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of sodium hydrogensulfate◆
ΔrG −94.25 kJ/mol K 3.25 × 1016 pK −16.51
| 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 | −480.47 | −94.25 | −773.4 | – |
per 1 mol of | −36.959 | −7.250 | −59.49 | – |
per 1 mol of Electron | −60.059 | −11.78 | −96.67 | – |
per 1 mol of | −480.47 | −94.25 | −773.4 | – |
per 1 mol of Sodium sulfate ion | −40.039 | −7.854 | −64.45 | – |
per 1 mol of Hydronium ion | −120.12 | −23.56 | −193.3 | – |
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 |
|---|---|---|---|---|
| NaHSO4 (cr) | -1125.5[1] | -992.8[1] | 113.0[1] | – |
| NaHSO4 (ai) | -1127.46[1] | -1017.80[1] | 190.8[1] | -38[1] |
| NaHSO4 (cr) 1 hydrate | -1421.7[1] | -1231.6[1] | 155[1] | – |
| e− | – | – | – | – |
* (cr):Crystalline solid, (ai):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 |
|---|---|---|---|---|
| NaHS (cr) | -237.23[1] | – | – | – |
| NaHS (ai) | -257.73[1] | -249.81[1] | 121.8[1] | – |
| NaHS (cr) 2 hydrate | -838.47[1] | – | – | – |
| NaSO4− (ao) | -1144.70[1] | -1010.61[1] | 108.8[1] | – |
| H3O+ (ao) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -1125.5 kJ · mol−1
- ^ ΔfG°, -992.8 kJ · mol−1
- ^ S°, 113.0 J · K−1 · mol−1
- ^ ΔfH°, -1127.46 kJ · mol−1
- ^ ΔfG°, -1017.80 kJ · mol−1
- ^ S°, 190.8 J · K−1 · mol−1
- ^ Cp°, -38. J · K−1 · mol−1
- ^ ΔfH°, -1421.7 kJ · mol−1
- ^ ΔfG°, -1231.6 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -237.23 kJ · mol−1
- ^ ΔfH°, -257.73 kJ · mol−1
- ^ ΔfG°, -249.81 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -838.47 kJ · mol−1
- ^ ΔfH°, -1144.70 kJ · mol−1
- ^ ΔfG°, -1010.61 kJ · mol−1
- ^ S°, 108.8 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