12FeO + SrSO4 🔥→ 4Fe3O4 + SrS
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The reaction of iron(II) oxide and strontium sulfate yields iron(II,III) oxide and strontium sulfide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(II) oxide and strontium sulfate
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of iron(II) oxide and strontium sulfate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
FeO | Iron(II) oxide | 12 | Reducing | Oxidizable |
SrSO4 | Strontium sulfate | 1 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe3O4 | Iron(II,III) oxide | 4 | Oxidized | – |
SrS | Strontium sulfide | 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) oxide and 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 | −228.9 | – | – | – |
per 1 mol of | −19.07 | – | – | – |
per 1 mol of | −228.9 | – | – | – |
per 1 mol of | −57.23 | – | – | – |
per 1 mol of | −228.9 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(II) oxide and 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 | −232.2 | – | – | – |
per 1 mol of | −19.35 | – | – | – |
per 1 mol of | −232.2 | – | – | – |
per 1 mol of | −58.05 | – | – | – |
per 1 mol of | −232.2 | – | – | – |
Changes in aqueous solution (1)
- Reaction of iron(II) oxide and 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 | −228.9 | – | – | – |
per 1 mol of | −19.07 | – | – | – |
per 1 mol of | −228.9 | – | – | – |
per 1 mol of | −57.23 | – | – | – |
per 1 mol of | −228.9 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(II) oxide and 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 | −232.2 | – | – | – |
per 1 mol of | −19.35 | – | – | – |
per 1 mol of | −232.2 | – | – | – |
per 1 mol of | −58.05 | – | – | – |
per 1 mol of | −232.2 | – | – | – |
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 |
---|---|---|---|---|
FeO (cr) | -272.0[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 |
---|---|---|---|---|
Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
SrS (cr) | -472.4[1] | -467.8[1] | 68.2[1] | 48.70[1] |
SrS (g) | 109[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas
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°, -272.0 kJ · mol−1
- ^ 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°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 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