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Cu + Mn2O3 + 2H2O 🔥→ CuO + 2Mn(OH)2

The reaction of copper, manganese(III) oxide, and water yields copper(II) oxide and manganese(II) hydroxide (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 manganese(III) oxide under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper1
Reducing
Oxidizable
Mn2O3Manganese(III) oxide1
Oxidizing
Oxidizing
H2OWater2
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
CuOCopper(II) oxide1
Oxidized
Mn(OH)2Manganese(II) hydroxide2
Reduced

Thermodynamic changes

Changes in standard condition

Reaction of copper and manganese(III) oxide under neutral condition
ΔrG−4.3 kJ/mol
K5.67 × 100
pK−0.75
CuCrystalline solid + Mn2O3Crystalline solid + 2H2OLiquid
🔥
CuOCrystalline solid + 2Mn(OH)2Amorphous solidprecipitated
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
−17.4−4.3−42.4
per 1 mol of
−17.4−4.3−42.4
−17.4−4.3−42.4
per 1 mol of
−8.70−2.1−21.2
per 1 mol of
−17.4−4.3−42.4
−8.70−2.1−21.2

Changes in aqueous solution

Reaction of copper and manganese(III) oxide under neutral condition
ΔrG−4.3 kJ/mol
K5.67 × 100
pK−0.75
CuCrystalline solid + Mn2O3Crystalline solid + 2H2OLiquid
🔥
CuOCrystalline solid + 2Mn(OH)2Amorphous solidprecipitated
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
−17.4−4.3−42.4
per 1 mol of
−17.4−4.3−42.4
−17.4−4.3−42.4
per 1 mol of
−8.70−2.1−21.2
per 1 mol of
−17.4−4.3−42.4
−8.70−2.1−21.2

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]
Mn2O3 (cr)-959.0[1]-881.1[1]110.5[1]107.65[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, (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
CuO (cr)-157.3[1]-129.7[1]42.63[1]42.30[1]
Mn(OH)2 (am)
precipitated
-695.4[1]-615.0[1]99.2[1]
* (cr):Crystalline solid, (am):Amorphous solid

References

List of references

  1. 1