2Ag2SO4 🔥⚡→ 2Ag2O + 2S + 3O2↑
Last updated:
- Molten salt electrolysis of silver(I) sulfate
Molten salt electrolysis of silver(I) sulfate yields silver(I) oxide, , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Molten salt electrolysis of silver(I) sulfate
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of silver(I) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ag2SO4 | Silver(I) sulfate | 2 | Self redox agent | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ag2O | Silver(I) oxide | 2 | – | – |
| 2 | Reduced | – | ||
| 3 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Molten salt electrolysis of silver(I) sulfate◆
ΔrG 1214.42 kJ/mol K 0.17 × 10−212 pK 212.76
| 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 | 1369.66 | 1214.42 | 520.8 | 2.31 |
per 1 mol of | 684.830 | 607.210 | 260.4 | 1.16 |
per 1 mol of | 684.830 | 607.210 | 260.4 | 1.16 |
| 684.830 | 607.210 | 260.4 | 1.16 | |
| 456.553 | 404.807 | 173.6 | 0.770 |
Changes in standard condition (2)
- Molten salt electrolysis of silver(I) sulfate
| 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 | 1370.32 | – | – | – |
per 1 mol of | 685.160 | – | – | – |
per 1 mol of | 685.160 | – | – | – |
| 685.160 | – | – | – | |
| 456.773 | – | – | – |
Changes in aqueous solution (1)
- Molten salt electrolysis of silver(I) sulfate◆
ΔrG 1158.20 kJ/mol K 0.12 × 10−202 pK 202.91
| 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 | 1334.10 | 1158.20 | 590.2 | 767 |
per 1 mol of | 667.050 | 579.100 | 295.1 | 384 |
per 1 mol of | 667.050 | 579.100 | 295.1 | 384 |
| 667.050 | 579.100 | 295.1 | 384 | |
| 444.700 | 386.067 | 196.7 | 256 |
Changes in aqueous solution (2)
- Molten salt electrolysis of silver(I) sulfate◆
ΔrG 1207.4 kJ/mol K 0.30 × 10−211 pK 211.53
| 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 | 1299.0 | 1207.4 | 307.5 | – |
per 1 mol of | 649.50 | 603.70 | 153.8 | – |
per 1 mol of | 649.50 | 603.70 | 153.8 | – |
| 649.50 | 603.70 | 153.8 | – | |
| 433.00 | 402.47 | 102.5 | – |
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 |
|---|---|---|---|---|
| Ag2SO4 (cr) | -715.88[1] | -618.41[1] | 200.4[1] | 131.38[1] |
| Ag2SO4 (ai) | -698.10[1] | -590.30[1] | 165.7[1] | -251[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 |
|---|---|---|---|---|
| Ag2O (cr) | -31.05[1] | -11.20[1] | 121.3[1] | 65.86[1] |
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (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°, -715.88 kJ · mol−1
- ^ ΔfG°, -618.41 kJ · mol−1
- ^ S°, 200.4 J · K−1 · mol−1
- ^ Cp°, 131.38 J · K−1 · mol−1
- ^ ΔfH°, -698.10 kJ · mol−1
- ^ ΔfG°, -590.30 kJ · mol−1
- ^ S°, 165.7 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfH°, -31.05 kJ · mol−1
- ^ ΔfG°, -11.20 kJ · mol−1
- ^ S°, 121.3 J · K−1 · mol−1
- ^ Cp°, 65.86 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1