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  3. 6KI + 2RbClO4 + 8H^+ → 6K^+ + 3I2 + 2ClO2↑ + 2Rb^+ + 4H2O

6KI + 2RbClO4 + 8H+ → 6K+ + 3I2 + 2ClO2↑ + 2Rb+ + 4H2O

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Reaction of potassium iodide and rubidium perchlorate under acidic condition
6KIPotassium iodide + 2RbClO4Rubidium perchlorate + 8H+Hydrogen ion
⟶
6K+Potassium ion + 3I2Iodine + 2ClO2↑Chlorine dioxide + 2Rb+Rubidium ion + 4H2OWater

The reaction of potassium iodide, rubidium perchlorate, and hydrogen ion yields potassium ion, iodine, chlorine dioxide, rubidium 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 potassium iodide and rubidium perchlorate under acidic condition
6KIPotassium iodide + 2RbClO4Rubidium perchlorate + 8H+Hydrogen ion
⟶
6K+Potassium ion + 3I2Iodine + 2ClO2↑Chlorine dioxide + 2Rb+Rubidium ion + 4H2OWater

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 potassium iodide and rubidium perchlorate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide6
Reducing
Oxidizable
RbClO4Rubidium perchlorate2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion8
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
K+Potassium ion6
–
–
I2Iodine3
Oxidized
–
ClO2Chlorine dioxide2
Reduced
–
Rb+Rubidium ion2
–
–
H2OWater4
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium iodide and rubidium perchlorate under acidic condition
◆
ΔrG−331.8 kJ/mol
K1.35 × 1058
pK−58.13
6KIIonized aqueous solution + 2RbClO4Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
6K+Un-ionized aqueous solution + 3I2Un-ionized aqueous solution + 2ClO2↑Gas + 2Rb+Un-ionized aqueous solution + 4H2OLiquid
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
−280.7−331.8173.5–
per 1 mol of
−46.78−55.3028.92–
−140.3−165.986.75–
per 1 mol of
Hydrogen ion
−35.09−41.4821.69–
per 1 mol of
Potassium ion
−46.78−55.3028.92–
per 1 mol of
−93.57−110.657.83–
per 1 mol of
−140.3−165.986.75–
per 1 mol of
Rubidium ion
−140.3−165.986.75–
per 1 mol of
−70.17−82.9543.38–

Changes in standard condition (2)

Reaction of potassium iodide and rubidium perchlorate under acidic condition
◆
ΔrG−332.6 kJ/mol
K1.86 × 1058
pK−58.27
6KIIonized aqueous solution + 2RbClO4Ionized aqueous solution + 8H+Un-ionized aqueous solution
⟶
6K+Un-ionized aqueous solution + 3I2Un-ionized aqueous solution + 2ClO2↑Un-ionized aqueous solution + 2Rb+Un-ionized aqueous solution + 4H2OLiquid
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
−335.9−332.6−10.6–
per 1 mol of
−55.98−55.43−1.77–
−167.9−166.3−5.30–
per 1 mol of
Hydrogen ion
−41.99−41.58−1.32–
per 1 mol of
Potassium ion
−55.98−55.43−1.77–
per 1 mol of
−112.0−110.9−3.53–
per 1 mol of
−167.9−166.3−5.30–
per 1 mol of
Rubidium ion
−167.9−166.3−5.30–
per 1 mol of
−83.97−83.15−2.65–

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
KI (cr)-327.900[1]-324.892[1]106.32[1]52.93[1]
KI (g)-125.5[1]-166.1[1]258.3[1]37.11[1]
KI (ai)-307.57[1]-334.85[1]213.8[1]-120.5[1]
RbClO4 (cr)-437.23[1]-306.90[1]161.1[1]–
RbClO4 (ai)-380.49[1]-292.51[1]303.3[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
K+ (g)514.26[1]–––
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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]–
ClO2 (g)102.5[1]120.5[1]256.84[1]41.97[1]
ClO2 (ao)74.9[1]120.1[1]164.8[1]–
Rb+ (g)490.101[1]–––
Rb+ (ao)-251.17[1]-283.98[1]121.50[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)