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26Cu + 2Fe(NO3)3 + 30H+ → 26Cu+ + 2Fe2+ + 3NH4NO3 + 9H2O

Reaction of copper and iron(III) nitrate under acidic condition
26CuCopper + 2Fe(NO3)3Iron(III) nitrate + 30H+Hydrogen ion
26Cu+Copper(I) ion + 2Fe2+Iron(II) ion + 3NH4NO3Ammonium nitrate + 9H2OWater

The reaction of copper, iron(III) nitrate, and hydrogen ion yields copper(I) ion, iron(II) ion, ammonium nitrate, 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

Reaction of copper and iron(III) nitrate under acidic condition
26CuCopper + 2Fe(NO3)3Iron(III) nitrate + 30H+Hydrogen ion
26Cu+Copper(I) ion + 2Fe2+Iron(II) ion + 3NH4NO3Ammonium nitrate + 9H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

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

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper26
Reducing
Oxidizable
Fe(NO3)3Iron(III) nitrate2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion30
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu+Copper(I) ion26
Oxidized
Fe2+Iron(II) ion2
Reduced
NH4NO3Ammonium nitrate3
Reduced
H2OWater9
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper and iron(III) nitrate under acidic condition
ΔrG−887.6 kJ/mol
K3.17 × 10155
pK−155.50
26CuCrystalline solid + 2Fe(NO3)3Ionized aqueous solution + 30H+Un-ionized aqueous solution
26Cu+Un-ionized aqueous solution + 2Fe2+Un-ionized aqueous solution + 3NH4NO3Ionized aqueous solution + 9H2OLiquid
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
−565.5−887.61080.1
per 1 mol of
−21.75−34.1441.542
per 1 mol of
−282.8−443.8540.05
per 1 mol of
Hydrogen ion
−18.85−29.5936.003
per 1 mol of
Copper(I) ion
−21.75−34.1441.542
per 1 mol of
Iron(II) ion
−282.8−443.8540.05
per 1 mol of
−188.5−295.9360.03
per 1 mol of
−62.83−98.62120.01

Changes in standard condition (2)

Reaction of copper and iron(III) nitrate under acidic condition
26CuCrystalline solid + 2Fe(NO3)3Aqueous solution + 30H+Un-ionized aqueous solution
26Cu+Un-ionized aqueous solution + 2Fe2+Un-ionized aqueous solution + 3NH4NO3Ionized aqueous solution + 9H2OLiquid
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
−557.1
per 1 mol of
−21.43
per 1 mol of
−278.6
per 1 mol of
Hydrogen ion
−18.57
per 1 mol of
Copper(I) ion
−21.43
per 1 mol of
Iron(II) ion
−278.6
per 1 mol of
−185.7
per 1 mol of
−61.90

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]
H+ (g)1536.202[1]
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):Aqueous solution, (ao):Un-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
Cu+ (g)1089.986[1]
Cu+ (ao)71.67[1]49.98[1]40.6[1]
Fe2+ (g)2749.93[1]
Fe2+ (ao)-89.1[1]-78.90[1]-137.7[1]
NH4NO3 (cr)-365.56[1]-183.87[1]151.08[1]139.3[1]
NH4NO3 (ai)-339.87[1]-190.56[1]259.8[1]-6.7[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]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)