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10Cu + 2CsIO3 + H2O → 5Cu2O + I2 + 2CsOH

The reaction of copper, caesium iodate, and water yields copper(I) oxide, iodine, and caesium 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 caesium iodate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper10
Reducing
Oxidizable
CsIO3Caesium iodate2
Oxidizing
Oxidizing
H2OWater1
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2OCopper(I) oxide5
Oxidized
I2Iodine1
Reduced
CsOHCaesium hydroxide2

Thermodynamic changes

Changes in standard condition

Reaction of copper and caesium iodate under neutral condition
10CuCrystalline solid + 2CsIO3Crystalline solid + H2OLiquid
5Cu2OCrystalline solid + I2Crystalline solid + 2CsOHCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution

Reaction of copper and caesium iodate under neutral condition
ΔrG−535.0 kJ/mol
K5.34 × 1093
pK−93.73
10CuCrystalline solid + 2CsIO3Ionized aqueous solution + H2OLiquid
5Cu2OCrystalline solid + I2Un-ionized aqueous solution + 2CsOHIonized 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
−552.1−535.0−56.9
per 1 mol of
−55.21−53.50−5.69
per 1 mol of
−276.1−267.5−28.4
per 1 mol of
−552.1−535.0−56.9
per 1 mol of
−110.4−107.0−11.4
per 1 mol of
−552.1−535.0−56.9
per 1 mol of
−276.1−267.5−28.4

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]
CsIO3 (cr)-433.8[1]
CsIO3 (ai)-479.5[1]-420.0[1]251.5[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]
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[1]
CsOH (cr)-417.23[1]
CsOH (g)-247[1]-247[1]254.83[1]49.71[1]
CsOH (ai)-488.27[1]-449.25[1]122.30[1]
CsOH (cr)
1 hydrate
-754.04[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)