Na2S2O3 + 4Fe2O3 → Na2SO4 + FeSO4 + 7FeO
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The reaction of sodium thiosulfate and iron(III) oxide yields sodium sulfate, iron(II) sulfate, 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 sodium thiosulfate and iron(III) oxide
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 sodium thiosulfate and iron(III) oxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2S2O3 | Sodium thiosulfate | 1 | Reducing | Reducing |
Fe2O3 | Iron(III) oxide | 4 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SO4 | Sodium sulfate | 1 | Oxidized | – |
FeSO4 | Iron(II) sulfate | 1 | Redoxed product | – |
FeO | Iron(II) oxide | 7 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium thiosulfate 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 | 200.3 | – | – | – |
per 1 mol of | 200.3 | – | – | – |
per 1 mol of | 50.08 | – | – | – |
per 1 mol of | 200.3 | – | – | – |
per 1 mol of | 200.3 | – | – | – |
per 1 mol of | 28.61 | – | – | – |
Changes in standard condition (2)
- Reaction of sodium thiosulfate 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution
- Reaction of sodium thiosulfate 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 | 207.3 | – | – | – |
per 1 mol of | 207.3 | – | – | – |
per 1 mol of | 51.83 | – | – | – |
per 1 mol of | 207.3 | – | – | – |
per 1 mol of | 207.3 | – | – | – |
per 1 mol of | 29.61 | – | – | – |
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 |
---|---|---|---|---|
Na2S2O3 (cr) | -1123.0[1] | -1028.0[1] | 155[1] | – |
Na2S2O3 (ai) | -1132.40[1] | -1046.0[1] | 184.1[1] | – |
Na2S2O3 (cr) 5 hydrate | -2607.93[1] | -2229.8[1] | 372[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 |
---|---|---|---|---|
Na2SO4 (cr) orthorhombic | -1387.08[1] | -1270.16[1] | 149.58[1] | 128.20[1] |
Na2SO4 (cr) metastable | – | – | 154.934[1] | 129.29[1] |
Na2SO4 (ai) | -1389.51[1] | -1268.36[1] | 138.1[1] | -201[1] |
Na2SO4 (cr) 10 hydrate | -4327.26[1] | -3646.85[1] | 592.0[1] | – |
FeSO4 (cr) | -928.4[1] | -820.8[1] | 107.5[1] | 100.58[1] |
FeSO4 (ai) | -998.3[1] | -823.43[1] | -117.6[1] | – |
FeSO4 (cr) 1 hydrate | -1243.69[1] | – | – | – |
FeSO4 (cr) 4 hydrate | -2129.2[1] | – | – | – |
FeSO4 (cr) 7 hydrate | -3014.57[1] | -2509.87[1] | 409.2[1] | 394.47[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°, -1123.0 kJ · mol−1
- ^ ΔfG°, -1028.0 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -1132.40 kJ · mol−1
- ^ ΔfG°, -1046.0 kJ · mol−1
- ^ S°, 184.1 J · K−1 · mol−1
- ^ ΔfH°, -2607.93 kJ · mol−1
- ^ ΔfG°, -2229.8 kJ · mol−1
- ^ S°, 372. 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°, -1387.08 kJ · mol−1
- ^ ΔfG°, -1270.16 kJ · mol−1
- ^ S°, 149.58 J · K−1 · mol−1
- ^ Cp°, 128.20 J · K−1 · mol−1
- ^ S°, 154.934 J · K−1 · mol−1
- ^ Cp°, 129.29 J · K−1 · mol−1
- ^ ΔfH°, -1389.51 kJ · mol−1
- ^ ΔfG°, -1268.36 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ Cp°, -201. J · K−1 · mol−1
- ^ ΔfH°, -4327.26 kJ · mol−1
- ^ ΔfG°, -3646.85 kJ · mol−1
- ^ S°, 592.0 J · K−1 · mol−1
- ^ ΔfH°, -928.4 kJ · mol−1
- ^ ΔfG°, -820.8 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ Cp°, 100.58 J · K−1 · mol−1
- ^ ΔfH°, -998.3 kJ · mol−1
- ^ ΔfG°, -823.43 kJ · mol−1
- ^ S°, -117.6 J · K−1 · mol−1
- ^ ΔfH°, -1243.69 kJ · mol−1
- ^ ΔfH°, -2129.2 kJ · mol−1
- ^ ΔfH°, -3014.57 kJ · mol−1
- ^ ΔfG°, -2509.87 kJ · mol−1
- ^ S°, 409.2 J · K−1 · mol−1
- ^ Cp°, 394.47 J · K−1 · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1