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4Cu + Fe(NO3)3 + 6H+ → 4Cu+ + Fe2+ + NO↑ + 2HNO3 + 2H2O

Reaction of copper and iron(III) nitrate under acidic condition
4CuCopper + Fe(NO3)3Iron(III) nitrate + 6H+Hydrogen ion
4Cu+Copper(I) ion + Fe2+Iron(II) ion + NONitrogen monoxide + 2HNO3Nitric acid + 2H2OWater

The reaction of copper, iron(III) nitrate, and hydrogen ion yields copper(I) ion, iron(II) ion, nitrogen monoxide, nitric acid, 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
4CuCopper + Fe(NO3)3Iron(III) nitrate + 6H+Hydrogen ion
4Cu+Copper(I) ion + Fe2+Iron(II) ion + NONitrogen monoxide + 2HNO3Nitric acid + 2H2OWater

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
CuCopper4
Reducing
Oxidizable
Fe(NO3)3Iron(III) nitrate1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion6
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu+Copper(I) ion4
Oxidized
Fe2+Iron(II) ion1
Reduced
NONitrogen monoxide1
Reduced
HNO3Nitric acid2
H2OWater2
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper and iron(III) nitrate under acidic condition
ΔrG−150.9 kJ/mol
K2.73 × 1026
pK−26.44
4CuCrystalline solid + Fe(NO3)3Ionized aqueous solution + 6H+Un-ionized aqueous solution
4Cu+Un-ionized aqueous solution + Fe2+Un-ionized aqueous solution + NOGas + 2HNO3Ionized aqueous solution + 2H2OLiquid
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
−27.8−150.9412.1
per 1 mol of
−6.95−37.73103.0
per 1 mol of
−27.8−150.9412.1
per 1 mol of
Hydrogen ion
−4.63−25.1568.68
per 1 mol of
Copper(I) ion
−6.95−37.73103.0
per 1 mol of
Iron(II) ion
−27.8−150.9412.1
per 1 mol of
−27.8−150.9412.1
per 1 mol of
−13.9−75.45206.1
per 1 mol of
−13.9−75.45206.1

Changes in standard condition (2)

Reaction of copper and iron(III) nitrate under acidic condition
4CuCrystalline solid + Fe(NO3)3Aqueous solution + 6H+Un-ionized aqueous solution
4Cu+Un-ionized aqueous solution + Fe2+Un-ionized aqueous solution + NOGas + 2HNO3Ionized aqueous solution + 2H2OLiquid
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
−23.7
per 1 mol of
−5.92
per 1 mol of
−23.7
per 1 mol of
Hydrogen ion
−3.95
per 1 mol of
Copper(I) ion
−5.92
per 1 mol of
Iron(II) ion
−23.7
per 1 mol of
−23.7
per 1 mol of
−11.8
per 1 mol of
−11.8

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]
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[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, (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid

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)