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26Cu + Fe2(SO4)3 + 30H+ 🔥→ 26Cu+ + 2Fe2+ + 3H2S↑ + 12H2O

Reaction of copper and iron(III) sulfate under acidic condition
26CuCopper + Fe2(SO4)3Iron(III) sulfate + 30H+Hydrogen ion
🔥
26Cu+Copper(I) ion + 2Fe2+Iron(II) ion + 3H2SHydrogen sulfide + 12H2OWater

The reaction of copper, iron(III) sulfate, and hydrogen ion yields copper(I) ion, iron(II) ion, hydrogen sulfide, 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) sulfate under acidic condition
26CuCopper + Fe2(SO4)3Iron(III) sulfate + 30H+Hydrogen ion
🔥
26Cu+Copper(I) ion + 2Fe2+Iron(II) ion + 3H2SHydrogen sulfide + 12H2OWater

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) sulfate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper26
Reducing
Oxidizable
Fe2(SO4)3Iron(III) sulfate1
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
H2SHydrogen sulfide3
Reduced
H2OWater12
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper and iron(III) sulfate under acidic condition
ΔrG438.3 kJ/mol
K0.16 × 10−76
pK76.79
26CuCrystalline solid + Fe2(SO4)3Ionized aqueous solution + 30H+Un-ionized aqueous solution
🔥
26Cu+Un-ionized aqueous solution + 2Fe2+Un-ionized aqueous solution + 3H2SGas + 12H2OLiquid
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
1018.4438.31946.1
per 1 mol of
39.16916.8674.850
per 1 mol of
1018.4438.31946.1
per 1 mol of
Hydrogen ion
33.94714.6164.870
per 1 mol of
Copper(I) ion
39.16916.8674.850
per 1 mol of
Iron(II) ion
509.20219.2973.05
per 1 mol of
339.47146.1648.70
per 1 mol of
84.86736.52162.17

Changes in standard condition (2)

Reaction of copper and iron(III) sulfate under acidic condition
ΔrG455.4 kJ/mol
K0.16 × 10−79
pK79.78
26CuCrystalline solid + Fe2(SO4)3Ionized aqueous solution + 30H+Un-ionized aqueous solution
🔥
26Cu+Un-ionized aqueous solution + 2Fe2+Un-ionized aqueous solution + 3H2SUn-ionized aqueous solution + 12H2OLiquid
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
961.2455.41692
per 1 mol of
36.9717.5265.08
per 1 mol of
961.2455.41692
per 1 mol of
Hydrogen ion
32.0415.1856.40
per 1 mol of
Copper(I) ion
36.9717.5265.08
per 1 mol of
Iron(II) ion
480.6227.7846.0
per 1 mol of
320.4151.8564.0
per 1 mol of
80.1037.95141.0

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]
Fe2(SO4)3 (cr)-2581.5[1]
Fe2(SO4)3 (ai)-2825.0[1]-2242.8[1]-571.5[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, (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]
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[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, (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)