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8Cu + KNO3 + 10H+ → 8Cu+ + NH4+ + K+ + 3H2O

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Reaction of copper and potassium nitrate under acidic condition
8CuCopper + KNO3Potassium nitrate + 10H+Hydrogen ion
⟶
8Cu+Copper(I) ion + NH4+Ammonium ion + K+Potassium ion + 3H2OWater

The reaction of copper, potassium nitrate, and hydrogen ion yields copper(I) ion, ammonium ion, potassium ion, 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 potassium nitrate under acidic condition
8CuCopper + KNO3Potassium nitrate + 10H+Hydrogen ion
⟶
8Cu+Copper(I) ion + NH4+Ammonium ion + K+Potassium ion + 3H2OWater

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 potassium nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper8
Reducing
Oxidizable
KNO3Potassium nitrate1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion10
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu+Copper(I) ion8
Oxidized
–
NH4+Ammonium ion1
Reduced
–
K+Potassium ion1
–
–
H2OWater3
–
Water

Thermodynamic changes

Changes in standard condition

Reaction of copper and potassium nitrate under acidic condition
◆
ΔrG−279.60 kJ/mol
K9.63 × 1048
pK−48.98
8CuCrystalline solid + KNO3Ionized aqueous solution + 10H+Un-ionized aqueous solution
⟶
8Cu+Un-ionized aqueous solution + NH4+Un-ionized aqueous solution + K+Un-ionized aqueous solution + 3H2OLiquid
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
−209.28−279.60236.3–
per 1 mol of
−26.160−34.95029.54–
per 1 mol of
−209.28−279.60236.3–
per 1 mol of
Hydrogen ion
−20.928−27.96023.63–
per 1 mol of
Copper(I) ion
−26.160−34.95029.54–
per 1 mol of
Ammonium ion
−209.28−279.60236.3–
per 1 mol of
Potassium ion
−209.28−279.60236.3–
per 1 mol of
−69.760−93.20078.77–

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]
KNO3 (cr)-494.63[1]-394.86[1]133.05[1]96.40[1]
KNO3 (ai)-459.74[1]-394.53[1]248.9[1]-64.9[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]–
NH4+ (ao)-132.51[1]-79.31[1]113.4[1]79.9[1]
K+ (g)514.26[1]–––
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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)