(NH4)2SO3 💧⚡→ NH4NO2 + H2S↑ + H2O
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- Electrolysis of aqueous ammonium sulfite without water as reactant
Electrolysis of aqueous ammonium sulfite yields ammonium nitrite, hydrogen sulfide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous ammonium sulfite without water as reactant
General equation
- Electrolysis of aqueous solution without water as reactant
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous ammonium sulfite without water as reactant
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2SO3 | Ammonium sulfite | 1 | Self redox agent | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO2 | Ammonium nitrite | 1 | Oxidized | – |
| H2S | Hydrogen sulfide | 1 | Reduced | – |
| H2O | Water | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous ammonium sulfite without water as reactant
| 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 | 322.3 | – | – | – |
per 1 mol of | 322.3 | – | – | – |
per 1 mol of | 322.3 | – | – | – |
per 1 mol of | 322.3 | – | – | – |
per 1 mol of | 322.3 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous ammonium sulfite without water as reactant◆
ΔrG 262.7 kJ/mol K 0.95 × 10−46 pK 46.02
| 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 | 356.7 | 262.7 | 314.6 | – |
per 1 mol of | 356.7 | 262.7 | 314.6 | – |
per 1 mol of | 356.7 | 262.7 | 314.6 | – |
per 1 mol of | 356.7 | 262.7 | 314.6 | – |
per 1 mol of | 356.7 | 262.7 | 314.6 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous ammonium sulfite without water as reactant◆
ΔrG 268.4 kJ/mol K 0.95 × 10−47 pK 47.02
| 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 | 337.7 | 268.4 | 230 | – |
per 1 mol of | 337.7 | 268.4 | 230 | – |
per 1 mol of | 337.7 | 268.4 | 230 | – |
per 1 mol of | 337.7 | 268.4 | 230 | – |
per 1 mol of | 337.7 | 268.4 | 230 | – |
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 |
|---|---|---|---|---|
| (NH4)2SO3 (cr) | -885.3[1] | – | – | – |
| (NH4)2SO3 (ai) | -900.4[1] | -645.0[1] | 197.5[1] | – |
| (NH4)2SO3 (cr) 1 hydrate | -1187.4[1] | – | – | – |
* (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 |
|---|---|---|---|---|
| NH4NO2 (cr) | -256.5[1] | – | – | – |
| NH4NO2 (ai) | -237.2[1] | -111.6[1] | 236.4[1] | -17.6[1] |
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -885.3 kJ · mol−1
- ^ ΔfH°, -900.4 kJ · mol−1
- ^ ΔfG°, -645.0 kJ · mol−1
- ^ S°, 197.5 J · K−1 · mol−1
- ^ ΔfH°, -1187.4 kJ · mol−1
- ^ ΔfH°, -256.5 kJ · mol−1
- ^ ΔfH°, -237.2 kJ · mol−1
- ^ ΔfG°, -111.6 kJ · mol−1
- ^ S°, 236.4 J · K−1 · mol−1
- ^ Cp°, -17.6 J · K−1 · mol−1
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. 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