4BaSO4 + 8e− → 4BaO + S2− + 3SO42−
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- Reduction of barium sulfate
Reduction of barium sulfate yields barium oxide, sulfide ion, and sulfate ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of barium sulfate
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of barium sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaSO4 | Barium sulfate | 4 | Oxidizing | – |
| e− | Electron | 8 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaO | Barium oxide | 4 | – | – |
| S2− | Sulfide ion | 1 | Reduced | – |
| SO42− | Sulfate ion | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of barium sulfate◆
ΔrG 973.0 kJ/mol K 0.34 × 10−170 pK 170.46
| 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 | −4329.9 | 973.0 | 208.6 | – |
per 1 mol of | −1082.5 | 243.3 | 52.15 | – |
per 1 mol of Electron | −541.24 | 121.6 | 26.07 | – |
per 1 mol of | −1082.5 | 243.3 | 52.15 | – |
per 1 mol of Sulfide ion | −4329.9 | 973.0 | 208.6 | – |
per 1 mol of Sulfate ion | −1443.3 | 324.3 | 69.53 | – |
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 |
|---|---|---|---|---|
| BaSO4 (cr) | -1473.2[1] | -1362.2[1] | 132.2[1] | 101.75[1] |
| BaSO4 (cr) precipitated | -1466.5[1] | – | – | – |
| BaSO4 (ai) | -144.691[1] | -1305.30[1] | 29.7[1] | – |
| e− | – | – | – | – |
* (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 |
|---|---|---|---|---|
| BaO (cr) | -553.5[1] | -525.1[1] | 70.42[1] | 47.78[1] |
| BaO (g) | -117[1] | – | – | 33.1[1] |
| S2− (ao) | 33.1[1] | 85.8[1] | -14.6[1] | – |
| SO42− (ao) | -909.27[1] | -744.53[1] | 20.1[1] | -293[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°, -1473.2 kJ · mol−1
- ^ ΔfG°, -1362.2 kJ · mol−1
- ^ S°, 132.2 J · K−1 · mol−1
- ^ Cp°, 101.75 J · K−1 · mol−1
- ^ ΔfH°, -1466.5 kJ · mol−1
- ^ ΔfH°, -144.691 kJ · mol−1
- ^ ΔfG°, -1305.30 kJ · mol−1
- ^ S°, 29.7 J · K−1 · mol−1
- ^ ΔfH°, -553.5 kJ · mol−1
- ^ ΔfG°, -525.1 kJ · mol−1
- ^ S°, 70.42 J · K−1 · mol−1
- ^ Cp°, 47.78 J · K−1 · mol−1
- ^ ΔfH°, -117. kJ · mol−1
- ^ Cp°, 33.1 J · K−1 · mol−1
- ^ ΔfH°, 33.1 kJ · mol−1
- ^ ΔfG°, 85.8 kJ · mol−1
- ^ S°, -14.6 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1