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4H2 + Fe3O4 🔥→ 3Fe + 4H2O

The reaction of hydrogen and iron(II,III) oxide yields iron and water (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
Reaction of reducing nonmetal and oxide
Reducing nonmetalReducing agent + OxideOxidizing agent
🔥
Elementary substance/OxideReduction product + Nonmetal oxideOxidation product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen4
Reducing
Reducing
Reducing nonmetal
Fe3O4Iron(II,III) oxide1
Oxidizing
Reducible
Oxide

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeIron3
Reduced
Elementary substance
H2OWater4
Oxidized
Oxide

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen and iron(II,III) oxide
ΔrG66.9 kJ/mol
K0.19 × 10−11
pK11.72
4H2Gas + Fe3O4Crystalline solid
🔥
3FeCrystalline solid + 4H2OLiquid
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
−24.966.9−307.7117.74
per 1 mol of
−6.2216.7−76.9229.435
per 1 mol of
−24.966.9−307.7117.74
per 1 mol of
−8.3022.3−102.639.247
per 1 mol of
−6.2216.7−76.9229.435

Changes in aqueous solution

Reaction of hydrogen and iron(II,III) oxide
ΔrG−3.5 kJ/mol
K4.10 × 100
pK−0.61
4H2Un-ionized aqueous solution + Fe3O4Crystalline solid
🔥
3FeCrystalline solid + 4H2OLiquid
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
−8.1−3.5−2093
per 1 mol of
−2.0−0.88−523.3
per 1 mol of
−8.1−3.5−2093
per 1 mol of
−2.7−1.2−697.7
per 1 mol of
−2.0−0.88−523.3

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]
Fe3O4 (cr)-1118.4[1]-1015.4[1]146.4[1]143.43[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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
Fe (cr)0[1]0[1]27.28[1]25.10[1]
Fe (g)416.3[1]370.7[1]180.490[1]25.677[1]
H2O (cr)
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (g):Gas, (l):Liquid

References

List of references

  1. 1