SrSO4 🔥⚡→ SrS + 2O2↑
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- Molten salt electrolysis of strontium sulfate
Molten salt electrolysis of strontium sulfate yields strontium sulfide 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 strontium sulfate
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of strontium sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SrSO4 | Strontium sulfate | 1 | Self redox agent | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SrS | Strontium sulfide | 1 | Reduced | – |
| 2 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Molten salt electrolysis of strontium sulfate◆
ΔrG 873.1 kJ/mol K 0.11 × 10−152 pK 152.96
| 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 | 980.7 | 873.1 | 361 | – |
per 1 mol of | 980.7 | 873.1 | 361 | – |
per 1 mol of | 980.7 | 873.1 | 361 | – |
| 490.4 | 436.6 | 181 | – |
Changes in standard condition (2)
- Molten salt electrolysis of strontium 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 | 977.4 | – | – | – |
per 1 mol of | 977.4 | – | – | – |
per 1 mol of | 977.4 | – | – | – |
| 488.7 | – | – | – |
Changes in aqueous solution (1)
- Molten salt electrolysis of strontium sulfate◆
ΔrG 873.1 kJ/mol K 0.11 × 10−152 pK 152.96
| 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 | 980.7 | 873.1 | 361 | – |
per 1 mol of | 980.7 | 873.1 | 361 | – |
per 1 mol of | 980.7 | 873.1 | 361 | – |
| 490.4 | 436.6 | 181 | – |
Changes in aqueous solution (2)
- Molten salt electrolysis of strontium sulfate◆
ΔrG 905.9 kJ/mol K 0.20 × 10−158 pK 158.71
| 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 | 957.3 | 905.9 | 173 | – |
per 1 mol of | 957.3 | 905.9 | 173 | – |
per 1 mol of | 957.3 | 905.9 | 173 | – |
| 478.6 | 452.9 | 86.5 | – |
Changes in aqueous solution (3)
- Molten salt electrolysis of strontium 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 | 977.4 | – | – | – |
per 1 mol of | 977.4 | – | – | – |
per 1 mol of | 977.4 | – | – | – |
| 488.7 | – | – | – |
Changes in aqueous solution (4)
- Molten salt electrolysis of strontium 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 | 954.0 | – | – | – |
per 1 mol of | 954.0 | – | – | – |
per 1 mol of | 954.0 | – | – | – |
| 477.0 | – | – | – |
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 |
|---|---|---|---|---|
| SrSO4 (cr) | -1453.1[1] | -1340.9[1] | 117[1] | – |
| SrSO4 (cr) precipitated | -1449.8[1] | – | – | – |
| SrSO4 (ai) | -1455.07[1] | -1304.00[1] | -12.6[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 |
|---|---|---|---|---|
| SrS (cr) | -472.4[1] | -467.8[1] | 68.2[1] | 48.70[1] |
| SrS (g) | 109[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°, -1453.1 kJ · mol−1
- ^ ΔfG°, -1340.9 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -1449.8 kJ · mol−1
- ^ ΔfH°, -1455.07 kJ · mol−1
- ^ ΔfG°, -1304.00 kJ · mol−1
- ^ S°, -12.6 J · K−1 · mol−1
- ^ ΔfH°, -472.4 kJ · mol−1
- ^ ΔfG°, -467.8 kJ · mol−1
- ^ S°, 68.2 J · K−1 · mol−1
- ^ Cp°, 48.70 J · K−1 · mol−1
- ^ ΔfH°, 109. kJ · 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