H2 + FeS 🔥→ Fe + H2S
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- Reaction of and iron(II) sulfide
The reaction of and iron(II) sulfide yields and hydrogen sulfide. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and iron(II) sulfide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and iron(II) sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing | ||
| FeS | Iron(II) sulfide | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reduced | – | ||
| H2S | Hydrogen sulfide | 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and iron(II) sulfide◆
ΔrG 66.8 kJ/mol K 0.20 × 10−11 pK 11.70
| 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 | 79.4 | 66.8 | 42.10 | −20.03 |
| 79.4 | 66.8 | 42.10 | −20.03 | |
per 1 mol of | 79.4 | 66.8 | 42.10 | −20.03 |
| 79.4 | 66.8 | 42.10 | −20.03 | |
per 1 mol of | 79.4 | 66.8 | 42.10 | −20.03 |
Changes in aqueous solution (1)
- Reaction of and iron(II) sulfide◆
ΔrG 49.2 kJ/mol K 0.24 × 10−8 pK 8.62
| 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 | 83.6 | 49.2 | −404 | – |
| 83.6 | 49.2 | −404 | – | |
per 1 mol of | 83.6 | 49.2 | −404 | – |
| 83.6 | 49.2 | −404 | – | |
per 1 mol of | 83.6 | 49.2 | −404 | – |
Changes in aqueous solution (2)
- Reaction of and iron(II) sulfide◆
ΔrG 55.0 kJ/mol K 0.23 × 10−9 pK 9.64
| 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 | 64.5 | 55.0 | −489 | – |
| 64.5 | 55.0 | −489 | – | |
per 1 mol of | 64.5 | 55.0 | −489 | – |
| 64.5 | 55.0 | −489 | – | |
per 1 mol of | 64.5 | 55.0 | −489 | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
| FeS (cr) iron-rich pyrrhotite, α | -100.0[1] | -100.4[1] | 60.29[1] | 50.54[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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) | 0[1] | 0[1] | 27.28[1] | 25.10[1] |
| (g) | 416.3[1] | 370.7[1] | 180.490[1] | 25.677[1] |
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1
- ^ ΔfH°, -100.0 kJ · mol−1
- ^ ΔfG°, -100.4 kJ · mol−1
- ^ S°, 60.29 J · K−1 · mol−1
- ^ Cp°, 50.54 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 27.28 J · K−1 · mol−1
- ^ Cp°, 25.10 J · K−1 · mol−1
- ^ ΔfH°, 416.3 kJ · mol−1
- ^ ΔfG°, 370.7 kJ · mol−1
- ^ S°, 180.490 J · K−1 · mol−1
- ^ Cp°, 25.677 J · K−1 · mol−1
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1