MnSO4 🔥⚡→ Mn + S + 2O2↑
Last updated:
- Molten salt electrolysis of manganese(II) sulfate
Molten salt electrolysis of manganese(II) sulfate yields , , 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 manganese(II) sulfate
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of manganese(II) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnSO4 | Manganese(II) sulfate | 1 | Self redox agent | Salt |
Products
Thermodynamic changes
Changes in standard condition (1)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 957.36 kJ/mol K 0.19 × 10−167 pK 167.72
| 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 | 1065.25 | 957.36 | 362.0 | 7.17 |
per 1 mol of | 1065.25 | 957.36 | 362.0 | 7.17 |
| 1065.25 | 957.36 | 362.0 | 7.17 | |
| 1065.25 | 957.36 | 362.0 | 7.17 | |
| 532.625 | 478.68 | 181.0 | 3.58 |
Changes in standard condition (2)
- Molten salt electrolysis of manganese(II) 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 | 1065.58 | – | – | – |
per 1 mol of | 1065.58 | – | – | – |
| 1065.58 | – | – | – | |
| 1065.58 | – | – | – | |
| 532.790 | – | – | – |
Changes in standard condition (3)
- Molten salt electrolysis of manganese(II) 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 | – | – | 364.4 | 7.38 |
per 1 mol of | – | – | 364.4 | 7.38 |
| – | – | 364.4 | 7.38 | |
| – | – | 364.4 | 7.38 | |
| – | – | 182.2 | 3.69 |
Changes in standard condition (4)
- Molten salt electrolysis of manganese(II) 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
| – | – | – | – | |
| – | – | – | – |
Changes in standard condition (5)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 958.78 kJ/mol K 0.11 × 10−167 pK 167.97
| 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 | 1066.80 | 958.78 | 362.4 | 8.42 |
per 1 mol of | 1066.80 | 958.78 | 362.4 | 8.42 |
| 1066.80 | 958.78 | 362.4 | 8.42 | |
| 1066.80 | 958.78 | 362.4 | 8.42 | |
| 533.400 | 479.39 | 181.2 | 4.21 |
Changes in standard condition (6)
- Molten salt electrolysis of manganese(II) 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 | 1067.13 | – | – | – |
per 1 mol of | 1067.13 | – | – | – |
| 1067.13 | – | – | – | |
| 1067.13 | – | – | – | |
| 533.565 | – | – | – |
Changes in aqueous solution (1)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 985.7 kJ/mol K 0.21 × 10−172 pK 172.69
| 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 | 1115.9 | 985.7 | 437.7 | – |
per 1 mol of | 1115.9 | 985.7 | 437.7 | – |
| 1115.9 | 985.7 | 437.7 | – | |
| 1115.9 | 985.7 | 437.7 | – | |
| 557.95 | 492.9 | 218.8 | – |
Changes in aqueous solution (2)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 1018.5 kJ/mol K 0.37 × 10−178 pK 178.43 - MnSO4Un-ionized aqueous solutionCrystalline solidα + Crystalline solidrhombic + 2↑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 | 1092.5 | 1018.5 | 249.2 | – |
per 1 mol of | 1092.5 | 1018.5 | 249.2 | – |
| 1092.5 | 1018.5 | 249.2 | – | |
| 1092.5 | 1018.5 | 249.2 | – | |
| 546.25 | 509.25 | 124.6 | – |
Changes in aqueous solution (3)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 972.7 kJ/mol K 0.39 × 10−170 pK 170.41
| 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 | 1130.1 | 972.7 | 527.7 | 351 |
per 1 mol of | 1130.1 | 972.7 | 527.7 | 351 |
| 1130.1 | 972.7 | 527.7 | 351 | |
| 1130.1 | 972.7 | 527.7 | 351 | |
| 565.05 | 486.4 | 263.9 | 176 |
Changes in aqueous solution (4)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 1005.5 kJ/mol K 0.70 × 10−176 pK 176.16 - MnSO4Ionized aqueous solutionCrystalline solidα + Crystalline solidrhombic + 2↑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 | 1106.7 | 1005.5 | 339.2 | – |
per 1 mol of | 1106.7 | 1005.5 | 339.2 | – |
| 1106.7 | 1005.5 | 339.2 | – | |
| 1106.7 | 1005.5 | 339.2 | – | |
| 553.35 | 502.75 | 169.6 | – |
Changes in aqueous solution (5)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 985.7 kJ/mol K 0.21 × 10−172 pK 172.69
| 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 | 1115.9 | 985.7 | 437.7 | – |
per 1 mol of | 1115.9 | 985.7 | 437.7 | – |
| 1115.9 | 985.7 | 437.7 | – | |
| 1115.9 | 985.7 | 437.7 | – | |
| 557.95 | 492.9 | 218.8 | – |
Changes in aqueous solution (6)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 1018.5 kJ/mol K 0.37 × 10−178 pK 178.43 - MnSO4Un-ionized aqueous solutionCrystalline solidα + Crystalline solidrhombic + 2↑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 | 1092.5 | 1018.5 | 249.2 | – |
per 1 mol of | 1092.5 | 1018.5 | 249.2 | – |
| 1092.5 | 1018.5 | 249.2 | – | |
| 1092.5 | 1018.5 | 249.2 | – | |
| 546.25 | 509.25 | 124.6 | – |
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 |
|---|---|---|---|---|
| MnSO4 (cr) | -1065.25[1] | -957.36[1] | 112.1[1] | 100.50[1] |
| MnSO4 (ai) | -1130.1[1] | -972.7[1] | -53.6[1] | -243[1] |
| MnSO4 (ao) | -1115.9[1] | -985.7[1] | 36.4[1] | – |
| MnSO4 (cr) 1 hydrate α | -1376.5[1] | – | – | – |
| MnSO4 (cr) 1 hydrate β | -1348.1[1] | – | – | – |
| MnSO4 (cr) 4 hydrate | -2258.1[1] | – | – | – |
| MnSO4 (cr) 5 hydrate | -2553.1[1] | – | – | 326[1] |
| MnSO4 (cr) 7 hydrate | -3139.3[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| (cr) α | 0[1] | 0[1] | 32.01[1] | 26.32[1] |
| (cr) β | – | – | 34.39[1] | 26.53[1] |
| (cr) γ | 1.55[1] | 1.42[1] | 32.43[1] | 27.57[1] |
| (g) | 280.7[1] | 238.5[1] | 173.70[1] | 20.79[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°, -1065.25 kJ · mol−1
- ^ ΔfG°, -957.36 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 100.50 J · K−1 · mol−1
- ^ ΔfH°, -1130.1 kJ · mol−1
- ^ ΔfG°, -972.7 kJ · mol−1
- ^ S°, -53.6 J · K−1 · mol−1
- ^ Cp°, -243. J · K−1 · mol−1
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfG°, -985.7 kJ · mol−1
- ^ S°, 36.4 J · K−1 · mol−1
- ^ ΔfH°, -1376.5 kJ · mol−1
- ^ ΔfH°, -1348.1 kJ · mol−1
- ^ ΔfH°, -2258.1 kJ · mol−1
- ^ ΔfH°, -2553.1 kJ · mol−1
- ^ Cp°, 326. J · K−1 · mol−1
- ^ ΔfH°, -3139.3 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 32.01 J · K−1 · mol−1
- ^ Cp°, 26.32 J · K−1 · mol−1
- ^ S°, 34.39 J · K−1 · mol−1
- ^ Cp°, 26.53 J · K−1 · mol−1
- ^ ΔfH°, 1.55 kJ · mol−1
- ^ ΔfG°, 1.42 kJ · mol−1
- ^ S°, 32.43 J · K−1 · mol−1
- ^ Cp°, 27.57 J · K−1 · mol−1
- ^ ΔfH°, 280.7 kJ · mol−1
- ^ ΔfG°, 238.5 kJ · mol−1
- ^ S°, 173.70 J · K−1 · mol−1
- ^ Cp°, 20.79 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