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5FeSO4 🔥→ Fe3O4 + Fe2(SO4)3 + 2SO2

Decomposition of iron(II) sulfate yields iron(II,III) oxide, iron(III) sulfate, and sulfur dioxide (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

Thermal decomposition with redox
Thermally decomposable substanceSelf redox agent
🔥
ProductOxidation product + ProductReduction product
Thermal decomposition of oxoacid salt with redox
Oxoacid saltSelf redox agent
🔥
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Decomposition of iron(II) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeSO4Iron(II) sulfate5
Self redox agent
Thermally decomposable
Oxoacid salt

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe3O4Iron(II,III) oxide1
Oxidized
Fe2(SO4)3Iron(III) sulfate1
Oxidized
SO2Sulfur dioxide2
Reduced

Thermodynamic changes

Changes in standard condition

Decomposition of iron(II) sulfate
5FeSO4Crystalline solid
🔥
Fe3O4Crystalline solid + Fe2(SO4)3Crystalline solid + 2SO2Gas
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
348.4
per 1 mol of
69.68
per 1 mol of
348.4
per 1 mol of
348.4
per 1 mol of
174.2

Changes in aqueous solution (1)

Decomposition of iron(II) sulfate
ΔrG245.4 kJ/mol
K0.10 × 10−42
pK42.99
5FeSO4Crystalline solid
🔥
Fe3O4Crystalline solid + Fe2(SO4)3Ionized aqueous solution + 2SO2Gas
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
104.9245.4−466.2
per 1 mol of
20.9849.08−93.24
per 1 mol of
104.9245.4−466.2
per 1 mol of
104.9245.4−466.2
per 1 mol of
52.45122.7−233.1

Changes in aqueous solution (2)

Decomposition of iron(II) sulfate
ΔrG244.4 kJ/mol
K0.15 × 10−42
pK42.82
5FeSO4Crystalline solid
🔥
Fe3O4Crystalline solid + Fe2(SO4)3Ionized aqueous solution + 2SO2Un-ionized aqueous solution
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
52.6244.4−638.8
per 1 mol of
10.548.88−127.8
per 1 mol of
52.6244.4−638.8
per 1 mol of
52.6244.4−638.8
per 1 mol of
26.3122.2−319.4

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
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]
* (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
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
Fe2(SO4)3 (cr)-2581.5[1]
Fe2(SO4)3 (ai)-2825.0[1]-2242.8[1]-571.5[1]
SO2 (l)-320.5[1]
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1