4PbCl2 + 2KMnO4 → 4PbO2 + Cl2↑ + 2MnCl2 + 2KCl
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The reaction of lead(II) chloride and potassium permanganate yields lead(IV) oxide, , manganese(II) chloride, and potassium chloride (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) chloride and potassium permanganate
General equation
- Reaction of hardly oxidizable species and oxidizing species
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of lead(II) chloride and potassium permanganate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbCl2 | Lead(II) chloride | 4 | Reducing | Hardly oxidizable |
KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbO2 | Lead(IV) oxide | 4 | Oxidized | – |
1 | Oxidized | – | ||
MnCl2 | Manganese(II) chloride | 2 | Reduced | – |
KCl | Potassium chloride | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG 163.0 kJ/mol K 0.28 × 10−28 pK 28.56
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 | 166.4 | 163.0 | 11.7 | – |
per 1 mol of | 41.60 | 40.75 | 2.92 | – |
per 1 mol of | 83.20 | 81.50 | 5.85 | – |
per 1 mol of | 41.60 | 40.75 | 2.92 | – |
166.4 | 163.0 | 11.7 | – | |
per 1 mol of | 83.20 | 81.50 | 5.85 | – |
per 1 mol of | 83.20 | 81.50 | 5.85 | – |
Changes in aqueous solution (1)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −71.5 kJ/mol K 3.36 × 1012 pK −12.53
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 | −127.2 | −71.5 | −187.7 | – |
per 1 mol of | −31.80 | −17.9 | −46.92 | – |
per 1 mol of | −63.60 | −35.8 | −93.85 | – |
per 1 mol of | −31.80 | −17.9 | −46.92 | – |
−127.2 | −71.5 | −187.7 | – | |
per 1 mol of | −63.60 | −35.8 | −93.85 | – |
per 1 mol of | −63.60 | −35.8 | −93.85 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −73.9 kJ/mol K 8.85 × 1012 pK −12.95
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 | – | −73.9 | – | – |
per 1 mol of | – | −18.5 | – | – |
per 1 mol of | – | −37.0 | – | – |
per 1 mol of | – | −18.5 | – | – |
– | −73.9 | – | – | |
per 1 mol of | – | −37.0 | – | – |
per 1 mol of | – | −37.0 | – | – |
Changes in aqueous solution (3)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −64.5 kJ/mol K 1.99 × 1011 pK −11.30
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 | −150.6 | −64.5 | −290 | – |
per 1 mol of | −37.65 | −16.1 | −72.5 | – |
per 1 mol of | −75.30 | −32.3 | −145 | – |
per 1 mol of | −37.65 | −16.1 | −72.5 | – |
−150.6 | −64.5 | −290 | – | |
per 1 mol of | −75.30 | −32.3 | −145 | – |
per 1 mol of | −75.30 | −32.3 | −145 | – |
Changes in aqueous solution (4)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −66.9 kJ/mol K 5.25 × 1011 pK −11.72
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 | – | −66.9 | – | – |
per 1 mol of | – | −16.7 | – | – |
per 1 mol of | – | −33.5 | – | – |
per 1 mol of | – | −16.7 | – | – |
– | −66.9 | – | – | |
per 1 mol of | – | −33.5 | – | – |
per 1 mol of | – | −33.5 | – | – |
Changes in aqueous solution (5)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −30.3 kJ/mol K 2.03 × 105 pK −5.31
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 | – | −30.3 | – | – |
per 1 mol of | – | −7.58 | – | – |
per 1 mol of | – | −15.2 | – | – |
per 1 mol of | – | −7.58 | – | – |
– | −30.3 | – | – | |
per 1 mol of | – | −15.2 | – | – |
per 1 mol of | – | −15.2 | – | – |
Changes in aqueous solution (6)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −32.7 kJ/mol K 5.36 × 105 pK −5.73
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 | – | −32.7 | – | – |
per 1 mol of | – | −8.18 | – | – |
per 1 mol of | – | −16.4 | – | – |
per 1 mol of | – | −8.18 | – | – |
– | −32.7 | – | – | |
per 1 mol of | – | −16.4 | – | – |
per 1 mol of | – | −16.4 | – | – |
Changes in aqueous solution (7)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −23.3 kJ/mol K 1.21 × 104 pK −4.08
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 | – | −23.3 | – | – |
per 1 mol of | – | −5.83 | – | – |
per 1 mol of | – | −11.7 | – | – |
per 1 mol of | – | −5.83 | – | – |
– | −23.3 | – | – | |
per 1 mol of | – | −11.7 | – | – |
per 1 mol of | – | −11.7 | – | – |
Changes in aqueous solution (8)
- Reaction of lead(II) chloride and potassium permanganate◆
ΔrG −25.7 kJ/mol K 3.18 × 104 pK −4.50
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 | – | −25.7 | – | – |
per 1 mol of | – | −6.42 | – | – |
per 1 mol of | – | −12.8 | – | – |
per 1 mol of | – | −6.42 | – | – |
– | −25.7 | – | – | |
per 1 mol of | – | −12.8 | – | – |
per 1 mol of | – | −12.8 | – | – |
Thermodynamic data of reactants
Chemical formula | Standard 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 |
---|---|---|---|---|
PbCl2 (cr) | -359.41[1] | -314.10[1] | 136.0[1] | – |
PbCl2 (ai) | -336.0[1] | -286.86[1] | 123.4[1] | – |
PbCl2 (ao) | – | -297.16[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
Thermodynamic data of products
Chemical formula | Standard 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] |
(g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
(ao) | -23.4[1] | 6.94[1] | 121[1] | – |
MnCl2 (cr) | -481.29[1] | -440.50[1] | 118.24[1] | 72.93[1] |
MnCl2 (g) | -263.6[1] | – | – | – |
MnCl2 (ai) | -555.05[1] | -490.8[1] | 38.9[1] | -222[1] |
MnCl2 (ao) | – | -492.0[1] | – | – |
MnCl2 (cr) 1 hydrate | -789.9[1] | -696.1[1] | 174.1[1] | – |
MnCl2 (cr) 2 hydrate | -1092.0[1] | -942.1[1] | 218.8[1] | – |
MnCl2 (cr) 4 hydrate | -1687.4[1] | -1423.6[1] | 303.3[1] | – |
KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[1] |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -359.41 kJ · mol−1
- ^ ΔfG°, -314.10 kJ · mol−1
- ^ S°, 136.0 J · K−1 · mol−1
- ^ ΔfH°, -336.0 kJ · mol−1
- ^ ΔfG°, -286.86 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfG°, -297.16 kJ · mol−1
- ^ ΔfH°, -837.2 kJ · mol−1
- ^ ΔfG°, -737.6 kJ · mol−1
- ^ S°, 171.71 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -793.8 kJ · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ S°, 293.7 J · K−1 · mol−1
- ^ Cp°, -60.2 J · K−1 · mol−1
- ^ ΔfH°, -277.4 kJ · mol−1
- ^ ΔfG°, -217.33 kJ · mol−1
- ^ S°, 68.6 J · K−1 · mol−1
- ^ Cp°, 64.64 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, -481.29 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 118.24 J · K−1 · mol−1
- ^ Cp°, 72.93 J · K−1 · mol−1
- ^ ΔfH°, -263.6 kJ · mol−1
- ^ ΔfH°, -555.05 kJ · mol−1
- ^ ΔfG°, -490.8 kJ · mol−1
- ^ S°, 38.9 J · K−1 · mol−1
- ^ Cp°, -222. J · K−1 · mol−1
- ^ ΔfG°, -492.0 kJ · mol−1
- ^ ΔfH°, -789.9 kJ · mol−1
- ^ ΔfG°, -696.1 kJ · mol−1
- ^ S°, 174.1 J · K−1 · mol−1
- ^ ΔfH°, -1092.0 kJ · mol−1
- ^ ΔfG°, -942.1 kJ · mol−1
- ^ S°, 218.8 J · K−1 · mol−1
- ^ ΔfH°, -1687.4 kJ · mol−1
- ^ ΔfG°, -1423.6 kJ · mol−1
- ^ S°, 303.3 J · K−1 · mol−1
- ^ ΔfH°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1