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10Cu + 2KClO3 + H2O → 5Cu2O + Cl2↑ + 2KOH

The reaction of copper, potassium chlorate, and water yields copper(I) oxide, chlorine, and potassium 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 potassium chlorate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper10
Reducing
Oxidizable
KClO3Potassium chlorate2
Oxidizing
Oxidizing
H2OWater1
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2OCopper(I) oxide5
Oxidized
Cl2Chlorine1
Reduced
KOHPotassium hydroxide2

Thermodynamic changes

Changes in standard condition

Reaction of copper and potassium chlorate under neutral condition
ΔrG−658.5 kJ/mol
K2.31 × 10115
pK−115.36
10CuCrystalline solid + 2KClO3Crystalline solid + H2OLiquid
5Cu2OCrystalline solid + Cl2Gas + 2KOHCrystalline solid
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
−611.2−658.5159.0−38.2
per 1 mol of
−61.12−65.8515.90−3.82
per 1 mol of
−305.6−329.379.50−19.1
per 1 mol of
−611.2−658.5159.0−38.2
per 1 mol of
−122.2−131.731.80−7.64
per 1 mol of
−611.2−658.5159.0−38.2
−305.6−329.379.50−19.1

Changes in aqueous solution (1)

Reaction of copper and potassium chlorate under neutral condition
ΔrG−791.4 kJ/mol
K4.44 × 10138
pK−138.65
10CuCrystalline solid + 2KClO3Ionized aqueous solution + H2OLiquid
5Cu2OCrystalline solid + Cl2Gas + 2KOHIonized aqueous solution
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
−809.2−791.4−59.0
per 1 mol of
−80.92−79.14−5.90
per 1 mol of
−404.6−395.7−29.5
per 1 mol of
−809.2−791.4−59.0
per 1 mol of
−161.8−158.3−11.8
per 1 mol of
−809.2−791.4−59.0
−404.6−395.7−29.5

Changes in aqueous solution (2)

Reaction of copper and potassium chlorate under neutral condition
ΔrG−784.5 kJ/mol
K2.74 × 10137
pK−137.44
10CuCrystalline solid + 2KClO3Ionized aqueous solution + H2OLiquid
5Cu2OCrystalline solid + Cl2Un-ionized aqueous solution + 2KOHIonized aqueous solution
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
−832.6−784.5−161
per 1 mol of
−83.26−78.45−16.1
per 1 mol of
−416.3−392.3−80.5
per 1 mol of
−832.6−784.5−161
per 1 mol of
−166.5−156.9−32.2
per 1 mol of
−832.6−784.5−161
−416.3−392.3−80.5

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]
KClO3 (cr)-397.73[1]-296.25[1]143.1[1]100.25[1]
KClO3 (ai)-356.35[1]-291.22[1]264.8[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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
Cu2O (cr)-168.6[1]-146.0[1]93.14[1]63.64[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]
KOH (cr)-424.764[1]-379.08[1]78.9[1]64.9[1]
KOH (g)-231.0[1]-232.6[1]238.3[1]49.20[1]
KOH (ai)-482.37[1]-440.50[1]91.6[1]-126.8[1]
KOH (cr)
1 hydrate
-748.9[1]-645.1[1]117.2[1]
KOH (cr)
2 hydrate
-1051.0[1]-887.3[1]150.6[1]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution

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)