2NaHSO4 + 2e− → 2NaSO4− + H2↑
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- Reduction of sodium hydrogensulfate
Reduction of sodium hydrogensulfate yields sodium sulfate ion and (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
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 | 2 | Oxidizing | – |
| e− | Electron | 2 | – | Electron |
Products
Thermodynamic changes
Changes in standard condition (1)
- Reduction of sodium hydrogensulfate◆
ΔrG 14.38 kJ/mol K 0.30 × 10−2 pK 2.52
| 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 | −34.48 | 14.38 | −33.3 | – |
per 1 mol of | −17.24 | 7.190 | −16.6 | – |
per 1 mol of Electron | −17.24 | 7.190 | −16.6 | – |
per 1 mol of Sodium sulfate ion | −17.24 | 7.190 | −16.6 | – |
| −34.48 | 14.38 | −33.3 | – |
Changes in standard condition (2)
- Reduction of sodium hydrogensulfate◆
ΔrG 32.0 kJ/mol K 0.25 × 10−5 pK 5.61 - 2NaHSO4Ionized aqueous solution + 2e−2NaSO4−Un-ionized aqueous solution + ↑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 | −38.7 | 32.0 | 413 | – |
per 1 mol of | −19.4 | 16.0 | 207 | – |
per 1 mol of Electron | −19.4 | 16.0 | 207 | – |
per 1 mol of Sodium sulfate ion | −19.4 | 16.0 | 207 | – |
| −38.7 | 32.0 | 413 | – |
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 |
|---|---|---|---|---|
| NaSO4− (ao) | -1144.70[1] | -1010.61[1] | 108.8[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (ao):Un-ionized aqueous solution, (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°, -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°, -1144.70 kJ · mol−1
- ^ ΔfG°, -1010.61 kJ · mol−1
- ^ S°, 108.8 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1