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5Pb3(PO4)2 + 6KMnO4 + 6H2O → 15PbO2 + 2Mn3(PO4)2 + 2K3PO4 + 4H3PO4

The reaction of lead(II) phosphate, potassium permanganate, and water yields lead(IV) oxide, manganese(II) phosphate, potassium phosphate, and phosphoric acid (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 hardly oxidizable species and oxidizing species under neutral condition
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of lead(II) phosphate and potassium permanganate under neutral condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Pb3(PO4)2Lead(II) phosphate5
Reducing
Hardly oxidizable
KMnO4Potassium permanganate6
Oxidizing
Oxidizing
H2OWater6
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
PbO2Lead(IV) oxide15
Oxidized
Mn3(PO4)2Manganese(II) phosphate2
Reduced
K3PO4Potassium phosphate2
H3PO4Phosphoric acid4

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) phosphate and potassium permanganate under neutral condition
5Pb3(PO4)2Crystalline solid + 6KMnO4Crystalline solid + 6H2OLiquid
15PbO2Crystalline solid + 2Mn3(PO4)2Crystalline solid + 2K3PO4Crystalline solid + 4H3PO4Crystalline 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

Changes in aqueous solution (1)

Reaction of lead(II) phosphate and potassium permanganate under neutral condition
5Pb3(PO4)2Crystalline solid + 6KMnO4Ionized aqueous solution + 6H2OLiquid
15PbO2Crystalline solid + 2Mn3(PO4)2Crystalline solid + 2K3PO4Ionized aqueous solution + 4H3PO4Un-ionized 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (2)

Reaction of lead(II) phosphate and potassium permanganate under neutral condition
5Pb3(PO4)2Crystalline solid + 6KMnO4Ionized aqueous solution + 6H2OLiquid
15PbO2Crystalline solid + 2Mn3(PO4)2Crystalline solid + 2K3PO4Ionized aqueous solution + 4H3PO4Ionized 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (3)

Reaction of lead(II) phosphate and potassium permanganate under neutral condition
5Pb3(PO4)2Crystalline solid + 6KMnO4Ionized aqueous solution + 6H2OLiquid
15PbO2Crystalline solid + 2Mn3(PO4)2Crystalline solid + 2K3PO4Ionized aqueous solution + 4H3PO4Un-ionized 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

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
Pb3(PO4)2 (cr)353.1[1]256.27[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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
PbO2 (cr)-277.4[1]-217.33[1]68.6[1]64.64[1]
Mn3(PO4)2 (cr)-3116.7[1]
K3PO4 (cr)-1950.2[1]
K3PO4 (ai)-2034.7[1]-1868.7[1]87.2[1]
H3PO4 (cr)-1279.0[1]-1119.1[1]110.50[1]106.06[1]
H3PO4 (l)-1266.9[1]
H3PO4 (ai)-1277.4[1]-1018.7[1]-220.3[1]
H3PO4 (ao)-1288.34[1]-1142.54[1]158.2[1]
H3PO4 (cr)
0.5 hydrate
-1431.3[1]-1242.1[1]129.16[1]126.02[1]
H3PO4 (cr)
1 hydrate
-1568.83[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (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)