K2SeO3 + Fe2O3 🔥→ K2SeO4 + 2FeO
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The reaction of potassium selenite and iron(III) oxide yields potassium selenate and iron(II) oxide (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 potassium selenite and iron(III) oxide
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 potassium selenite and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SeO3 | Potassium selenite | 1 | Reducing | Oxidizable |
| Fe2O3 | Iron(III) oxide | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SeO4 | Potassium selenate | 1 | Oxidized | – |
| FeO | Iron(II) oxide | 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium selenite and iron(III) oxide
| 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 | 152.2 | – | – | – |
per 1 mol of | 152.2 | – | – | – |
per 1 mol of | 152.2 | – | – | – |
per 1 mol of | 152.2 | – | – | – |
per 1 mol of | 76.10 | – | – | – |
Changes in aqueous solution
- Reaction of potassium selenite and iron(III) oxide
| 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 | 190.3 | – | – | – |
per 1 mol of | 190.3 | – | – | – |
per 1 mol of | 190.3 | – | – | – |
per 1 mol of | 190.3 | – | – | – |
per 1 mol of | 95.15 | – | – | – |
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 |
|---|---|---|---|---|
| K2SeO3 (cr) | -982.0[1] | – | – | – |
| K2SeO3 (ai) | -1013.8[1] | -936.3[1] | 218.0[1] | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[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 |
|---|---|---|---|---|
| K2SeO4 (cr) | -1110.02[1] | -1002.8[1] | 222[1] | – |
| K2SeO4 (ai) | -1103.7[1] | -1007.9[1] | 259.0[1] | – |
| FeO (cr) | -272.0[1] | – | – | – |
* (cr):Crystalline solid, (ai):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°, -982.0 kJ · mol−1
- ^ ΔfH°, -1013.8 kJ · mol−1
- ^ ΔfG°, -936.3 kJ · mol−1
- ^ S°, 218.0 J · K−1 · mol−1
- ^ ΔfH°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 J · K−1 · mol−1
- ^ ΔfH°, -1110.02 kJ · mol−1
- ^ ΔfG°, -1002.8 kJ · mol−1
- ^ S°, 222. J · K−1 · mol−1
- ^ ΔfH°, -1103.7 kJ · mol−1
- ^ ΔfG°, -1007.9 kJ · mol−1
- ^ S°, 259.0 J · K−1 · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1