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K2S2O3 + 3Fe2O3 🔥→ K2SO4 + S + 2Fe3O4

The reaction of potassium thiosulfate and iron(III) oxide yields potassium sulfate, sulfur, and iron(II,III) oxide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K2S2O3Potassium thiosulfate1
Reducing
Reducing
Fe2O3Iron(III) oxide3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate1
Oxidized
SSulfur1
Oxidized
Fe3O4Iron(II,III) oxide2
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium thiosulfate and iron(III) oxide
K2S2O3Crystalline solid + 3Fe2O3Crystalline solid
🔥
K2SO4Crystalline solid + SCrystalline solidrhombic + 2Fe3O4Crystalline solid
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
−28.4
−28.4
per 1 mol of
−9.47
per 1 mol of
−28.4
per 1 mol of
−28.4
per 1 mol of
−14.2

Changes in standard condition (2)

Reaction of potassium thiosulfate and iron(III) oxide
K2S2O3Crystalline solid + 3Fe2O3Crystalline solid
🔥
K2SO4Crystalline solid + SCrystalline solidmonoclinic + 2Fe3O4Crystalline solid
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
−28.1
−28.1
per 1 mol of
−9.37
per 1 mol of
−28.1
per 1 mol of
−28.1
per 1 mol of
−14.1

Changes in aqueous solution

Reaction of potassium thiosulfate and iron(III) oxide
ΔrG−26.3 kJ/mol
K4.05 × 104
pK−4.61
K2S2O3Ionized aqueous solution + 3Fe2O3Crystalline solid
🔥
K2SO4Ionized aqueous solution + SCrystalline solidrhombic + 2Fe3O4Crystalline solid
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
−21.3−26.316
−21.3−26.316
per 1 mol of
−7.10−8.775.3
per 1 mol of
−21.3−26.316
per 1 mol of
−21.3−26.316
per 1 mol of
−10.7−13.28.0

Thermodynamic data of reactants

Chemical formulaStandard 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
K2S2O3 (cr)-1173.6[1]
K2S2O3 (ai)-1156.9[1]-1089.0[1]272[1]
K2S2O3 (cr)
1 hydrate
-1464.8[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 formulaStandard 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
K2SO4 (cr)-1437.79[1]-1321.37[1]175.56[1]131.46[1]
K2SO4 (g)-1096[1]-1033[1]364[1]108.8[1]
K2SO4 (ai)-1414.02[1]-1311.07[1]225.1[1]-251[1]
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

References

List of references

  1. 1