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10CsI + 2KMnO4 + 5H2O 🔥→ 10CsOH + 4I2 + Mn2O3 + 2KI

The reaction of caesium iodide, potassium permanganate, and water yields caesium hydroxide, iodine, manganese(III) oxide, and potassium iodide (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 caesium iodide and potassium permanganate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CsICaesium iodide10
Reducing
Oxidizable
KMnO4Potassium permanganate2
Oxidizing
Oxidizing
H2OWater5
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
CsOHCaesium hydroxide10
I2Iodine4
Oxidized
Mn2O3Manganese(III) oxide1
Reduced
KIPotassium iodide2

Thermodynamic changes

Changes in standard condition

Reaction of caesium iodide and potassium permanganate under neutral condition
10CsICrystalline solid + 2KMnO4Crystalline solid + 5H2OLiquid
🔥
10CsOHCrystalline solid + 4I2Crystalline solid + Mn2O3Crystalline solid + 2KICrystalline 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
782.4
per 1 mol of
78.24
391.2
per 1 mol of
156.5
per 1 mol of
78.24
per 1 mol of
195.6
782.4
per 1 mol of
391.2

Changes in aqueous solution

Reaction of caesium iodide and potassium permanganate under neutral condition
ΔrG104.8 kJ/mol
K0.44 × 10−18
pK18.36
10CsIIonized aqueous solution + 2KMnO4Ionized aqueous solution + 5H2OLiquid
🔥
10CsOHIonized aqueous solution + 4I2Un-ionized aqueous solution + Mn2O3Crystalline solid + 2KIIonized 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
−215.0104.8−1070.1
per 1 mol of
−21.5010.48−107.01
−107.552.40−535.05
per 1 mol of
−43.0020.96−214.02
per 1 mol of
−21.5010.48−107.01
per 1 mol of
−53.7526.20−267.52
−215.0104.8−1070.1
per 1 mol of
−107.552.40−535.05

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
CsI (cr)-346.60[1]-340.58[1]123.05[1]52.80[1]
CsI (g)-151.9[1]-191.2[1]275.29[1]37.45[1]
CsI (ai)-313.47[1]-343.59[1]244.3[1]-152.7[1]
KMnO4 (cr)-837.2[1]-737.6[1]171.71[1]117.57[1]
KMnO4 (ai)-793.8[1]-730.5[1]293.7[1]-60.2[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
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]
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]
Mn2O3 (cr)-959.0[1]-881.1[1]110.5[1]107.65[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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)