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3FeO + Na[AuCl4] → Fe2O3 + FeCl3 + Au + NaCl

The reaction of iron(II) oxide and sodium tetrachloridoaurate(III) yields iron(III) oxide, iron(III) chloride, gold, and sodium chloride (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 oxidizable species and oxidizing species
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeOIron(II) oxide3
Reducing
Oxidizable
Na[AuCl4]Sodium tetrachloridoaurate(III)1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe2O3Iron(III) oxide1
Oxidized
FeCl3Iron(III) chloride1
Oxidized
AuGold1
Reduced
NaClSodium chloride1

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of iron(II) oxide and sodium tetrachloridoaurate(III)
3FeOCrystalline solid + Na[AuCl4]Ionized aqueous solution
Fe2O3Crystalline solid + FeCl3Un-ionized aqueous solution + AuCrystalline solid + NaClIonized 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (2)

Reaction of iron(II) oxide and sodium tetrachloridoaurate(III)
3FeOCrystalline solid + Na[AuCl4]Ionized aqueous solution
Fe2O3Crystalline solid + FeCl3Ionized aqueous solution + AuCrystalline solid + NaClIonized 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
−403.4
per 1 mol of
−134.5
−403.4
per 1 mol of
−403.4
per 1 mol of
−403.4
per 1 mol of
−403.4
per 1 mol of
−403.4

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
FeO (cr)-272.0[1]
Na[AuCl4] (ai)-562.3[1]-497.04[1]325.9[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
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
FeCl3 (cr)-399.49[1]-334.00[1]142.3[1]96.65[1]
FeCl3 (g)-254.0[1]
FeCl3 (ai)-550.2[1]-398.3[1]-146.4[1]
FeCl3 (ao)-404.5[1]
FeCl3 (cr)
6 hydrate
-2223.8[1]
Au (cr)0[1]0[1]47.40[1]25.418[1]
Au (g)366.1[1]326.3[1]180.503[1]20.786[1]
NaCl (cr)-411.153[1]-384.138[1]72.13[1]50.50[1]
NaCl (g)-176.65[1]-196.66[1]229.81[1]35.77[1]
NaCl (ai)-407.27[1]-393.133[1]115.5[1]-90.0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 1