2MnSO4 🔥⚡→ 2MnO + 2SO2↑ + O2↑
Last updated:
- Molten salt electrolysis of manganese(II) sulfate
Molten salt electrolysis of manganese(II) sulfate yields manganese(II) oxide, sulfur dioxide, 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 | 2 | Self redox agent | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnO | Manganese(II) oxide | 2 | – | – |
| SO2 | Sulfur dioxide | 2 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 588.53 kJ/mol K 0.78 × 10−103 pK 103.11
| 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 | 766.40 | 588.53 | 596.8 | −1.03 |
per 1 mol of | 383.20 | 294.26 | 298.4 | −0.515 |
per 1 mol of | 383.20 | 294.26 | 298.4 | −0.515 |
per 1 mol of | 383.20 | 294.26 | 298.4 | −0.515 |
| 766.40 | 588.53 | 596.8 | −1.03 |
Changes in aqueous solution (1)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 645.2 kJ/mol K 0.92 × 10−113 pK 113.03
| 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 | 867.7 | 645.2 | 748.2 | – |
per 1 mol of | 433.9 | 322.6 | 374.1 | – |
per 1 mol of | 433.9 | 322.6 | 374.1 | – |
per 1 mol of | 433.9 | 322.6 | 374.1 | – |
| 867.7 | 645.2 | 748.2 | – |
Changes in aqueous solution (2)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 661.6 kJ/mol K 0.12 × 10−115 pK 115.91
| 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 | 856.0 | 661.6 | 654.0 | – |
per 1 mol of | 428.0 | 330.8 | 327.0 | – |
per 1 mol of | 428.0 | 330.8 | 327.0 | – |
per 1 mol of | 428.0 | 330.8 | 327.0 | – |
| 856.0 | 661.6 | 654.0 | – |
Changes in aqueous solution (3)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 644.2 kJ/mol K 0.14 × 10−112 pK 112.86
| 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 | 815.4 | 644.2 | 575.6 | – |
per 1 mol of | 407.7 | 322.1 | 287.8 | – |
per 1 mol of | 407.7 | 322.1 | 287.8 | – |
per 1 mol of | 407.7 | 322.1 | 287.8 | – |
| 815.4 | 644.2 | 575.6 | – |
Changes in aqueous solution (4)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 660.6 kJ/mol K 0.19 × 10−115 pK 115.73
| 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 | 803.7 | 660.6 | 481.3 | – |
per 1 mol of | 401.9 | 330.3 | 240.7 | – |
per 1 mol of | 401.9 | 330.3 | 240.7 | – |
per 1 mol of | 401.9 | 330.3 | 240.7 | – |
| 803.7 | 660.6 | 481.3 | – |
Changes in aqueous solution (5)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 619.2 kJ/mol K 0.33 × 10−108 pK 108.48
| 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 | 896.1 | 619.2 | 928.2 | 686 |
per 1 mol of | 448.1 | 309.6 | 464.1 | 343 |
per 1 mol of | 448.1 | 309.6 | 464.1 | 343 |
per 1 mol of | 448.1 | 309.6 | 464.1 | 343 |
| 896.1 | 619.2 | 928.2 | 686 |
Changes in aqueous solution (6)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 635.6 kJ/mol K 0.44 × 10−111 pK 111.35
| 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 | 884.4 | 635.6 | 834.0 | – |
per 1 mol of | 442.2 | 317.8 | 417.0 | – |
per 1 mol of | 442.2 | 317.8 | 417.0 | – |
per 1 mol of | 442.2 | 317.8 | 417.0 | – |
| 884.4 | 635.6 | 834.0 | – |
Changes in aqueous solution (7)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 618.2 kJ/mol K 0.50 × 10−108 pK 108.30
| 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 | 843.8 | 618.2 | 755.6 | – |
per 1 mol of | 421.9 | 309.1 | 377.8 | – |
per 1 mol of | 421.9 | 309.1 | 377.8 | – |
per 1 mol of | 421.9 | 309.1 | 377.8 | – |
| 843.8 | 618.2 | 755.6 | – |
Changes in aqueous solution (8)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 634.6 kJ/mol K 0.67 × 10−111 pK 111.18
| 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 | 832.1 | 634.6 | 661.3 | – |
per 1 mol of | 416.1 | 317.3 | 330.6 | – |
per 1 mol of | 416.1 | 317.3 | 330.6 | – |
per 1 mol of | 416.1 | 317.3 | 330.6 | – |
| 832.1 | 634.6 | 661.3 | – |
Changes in aqueous solution (9)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 645.2 kJ/mol K 0.92 × 10−113 pK 113.03
| 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 | 867.7 | 645.2 | 748.2 | – |
per 1 mol of | 433.9 | 322.6 | 374.1 | – |
per 1 mol of | 433.9 | 322.6 | 374.1 | – |
per 1 mol of | 433.9 | 322.6 | 374.1 | – |
| 867.7 | 645.2 | 748.2 | – |
Changes in aqueous solution (10)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 661.6 kJ/mol K 0.12 × 10−115 pK 115.91
| 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 | 856.0 | 661.6 | 654.0 | – |
per 1 mol of | 428.0 | 330.8 | 327.0 | – |
per 1 mol of | 428.0 | 330.8 | 327.0 | – |
per 1 mol of | 428.0 | 330.8 | 327.0 | – |
| 856.0 | 661.6 | 654.0 | – |
Changes in aqueous solution (11)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 644.2 kJ/mol K 0.14 × 10−112 pK 112.86
| 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 | 815.4 | 644.2 | 575.6 | – |
per 1 mol of | 407.7 | 322.1 | 287.8 | – |
per 1 mol of | 407.7 | 322.1 | 287.8 | – |
per 1 mol of | 407.7 | 322.1 | 287.8 | – |
| 815.4 | 644.2 | 575.6 | – |
Changes in aqueous solution (12)
- Molten salt electrolysis of manganese(II) sulfate◆
ΔrG 660.6 kJ/mol K 0.19 × 10−115 pK 115.73
| 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 | 803.7 | 660.6 | 481.3 | – |
per 1 mol of | 401.9 | 330.3 | 240.7 | – |
per 1 mol of | 401.9 | 330.3 | 240.7 | – |
per 1 mol of | 401.9 | 330.3 | 240.7 | – |
| 803.7 | 660.6 | 481.3 | – |
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 |
|---|---|---|---|---|
| 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 |
|---|---|---|---|---|
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[1] | – | – | – |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[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, (l):Liquid, (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°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 kJ · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 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