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22Cu + 2Fe(NO3)3 + 28H2O 🔥→ 22Cu(OH)2 + 2FeO + 3N2H4

The reaction of copper, iron(III) nitrate, and water yields copper(II) hydroxide, iron(II) oxide, and hydrazine (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 under neutral condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of copper and iron(III) nitrate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper22
Reducing
Oxidizable
Fe(NO3)3Iron(III) nitrate2
Oxidizing
Oxidizing
H2OWater28
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu(OH)2Copper(II) hydroxide22
Oxidized
FeOIron(II) oxide2
Reduced
N2H4Hydrazine3
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of copper and iron(III) nitrate under neutral condition
22CuCrystalline solid + 2Fe(NO3)3Ionized aqueous solution + 28H2OLiquid
🔥
22Cu(OH)2Ionized aqueous solution + 2FeOCrystalline solid + 3N2H4Un-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
208.7
per 1 mol of
9.486
per 1 mol of
104.3
per 1 mol of
7.454
9.486
per 1 mol of
104.3
per 1 mol of
69.57

Changes in aqueous solution (2)

Reaction of copper and iron(III) nitrate under neutral condition
22CuCrystalline solid + 2Fe(NO3)3Aqueous solution + 28H2OLiquid
🔥
22Cu(OH)2Ionized aqueous solution + 2FeOCrystalline solid + 3N2H4Un-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
217.1
per 1 mol of
9.868
per 1 mol of
108.5
per 1 mol of
7.754
9.868
per 1 mol of
108.5
per 1 mol of
72.37

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
Cu (cr)0[1]0[1]33.150[1]24.435[1]
Cu (g)338.32[1]298.58[1]166.38[1]20.786[1]
Fe(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]
Fe(NO3)3 (aq)-674.9[1]
Fe(NO3)3 (cr)
9 hydrate
-3285.3[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, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid

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
Cu(OH)2 (cr)-449.8[1]
Cu(OH)2 (ai)-395.22[1]-249.01[1]-120.9[1]
FeO (cr)-272.0[1]
N2H4 (l)50.63[1]149.34[1]121.21[1]98.87[1]
N2H4 (g)95.40[1]159.35[1]238.47[1]49.58[1]
N2H4 (ao)34.31[1]128.1[1]138[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1