SrSO4 🔥⚡→ Sr + S + 2O2↑
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- Molten salt electrolysis of strontium sulfate
Molten salt electrolysis of strontium 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 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
Thermodynamic changes
Changes in standard condition (1)
- Molten salt electrolysis of strontium sulfate◆
ΔrG 1340.9 kJ/mol K 0.12 × 10−234 pK 234.92
| 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 | 1453.1 | 1340.9 | 377 | – |
per 1 mol of | 1453.1 | 1340.9 | 377 | – |
| 1453.1 | 1340.9 | 377 | – | |
| 1453.1 | 1340.9 | 377 | – | |
| 726.55 | 670.45 | 189 | – |
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 | 1453.4 | – | – | – |
per 1 mol of | 1453.4 | – | – | – |
| 1453.4 | – | – | – | |
| 1453.4 | – | – | – | |
| 726.70 | – | – | – |
Changes in standard condition (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 | 1449.8 | – | – | – |
per 1 mol of | 1449.8 | – | – | – |
| 1449.8 | – | – | – | |
| 1449.8 | – | – | – | |
| 724.90 | – | – | – |
Changes in standard condition (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 | 1450.1 | – | – | – |
per 1 mol of | 1450.1 | – | – | – |
| 1450.1 | – | – | – | |
| 1450.1 | – | – | – | |
| 725.05 | – | – | – |
Changes in aqueous solution (1)
- Molten salt electrolysis of strontium sulfate◆
ΔrG 1340.9 kJ/mol K 0.12 × 10−234 pK 234.92
| 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 | 1453.1 | 1340.9 | 377 | – |
per 1 mol of | 1453.1 | 1340.9 | 377 | – |
| 1453.1 | 1340.9 | 377 | – | |
| 1453.1 | 1340.9 | 377 | – | |
| 726.55 | 670.45 | 189 | – |
Changes in aqueous solution (2)
- Molten salt electrolysis of strontium sulfate◆
ΔrG 1373.7 kJ/mol K 0.22 × 10−240 pK 240.66 - SrSO4Crystalline solidCrystalline 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 | 1429.7 | 1373.7 | 189 | – |
per 1 mol of | 1429.7 | 1373.7 | 189 | – |
| 1429.7 | 1373.7 | 189 | – | |
| 1429.7 | 1373.7 | 189 | – | |
| 714.85 | 686.85 | 94.5 | – |
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 | 1449.8 | – | – | – |
per 1 mol of | 1449.8 | – | – | – |
| 1449.8 | – | – | – | |
| 1449.8 | – | – | – | |
| 724.90 | – | – | – |
Changes in aqueous solution (4)
- Molten salt electrolysis of strontium sulfate
- SrSO4Crystalline solidprecipitatedCrystalline 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 | 1426.4 | – | – | – |
per 1 mol of | 1426.4 | – | – | – |
| 1426.4 | – | – | – | |
| 1426.4 | – | – | – | |
| 713.20 | – | – | – |
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 |
|---|---|---|---|---|
| (cr) α | 0[1] | 0[1] | 52.3[1] | 26.4[1] |
| (g) | 164.4[1] | 130.9[1] | 164.62[1] | 20.786[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°, -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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 52.3 J · K−1 · mol−1
- ^ Cp°, 26.4 J · K−1 · mol−1
- ^ ΔfH°, 164.4 kJ · mol−1
- ^ ΔfG°, 130.9 kJ · mol−1
- ^ S°, 164.62 J · K−1 · mol−1
- ^ Cp°, 20.786 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