7PbCl2 + 6KMnO4 + 6H+ → 7PbO2 + 2HClO4 + 6MnCl2 + 6K+ + 2H2O
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- Reaction of lead(II) chloride and potassium permanganate under acidic condition
- 7PbCl2Lead(II) chloride + 6KMnO4Potassium permanganate + 6H+Hydrogen ion7PbO2Lead(IV) oxide + 2HClO4Perchloric acid + 6MnCl2Manganese(II) chloride + 6K+Potassium ion + 2H2OWater⟶
The reaction of lead(II) chloride, potassium permanganate, and hydrogen ion yields lead(IV) oxide, perchloric acid, manganese(II) chloride, potassium ion, and water (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 under acidic condition
- 7PbCl2Lead(II) chloride + 6KMnO4Potassium permanganate + 6H+Hydrogen ion7PbO2Lead(IV) oxide + 2HClO4Perchloric acid + 6MnCl2Manganese(II) chloride + 6K+Potassium ion + 2H2OWater⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species under acidic condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of lead(II) chloride and potassium permanganate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbCl2 | Lead(II) chloride | 7 | Reducing | Hardly oxidizable |
| KMnO4 | Potassium permanganate | 6 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 6 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO2 | Lead(IV) oxide | 7 | Oxidized | – |
| HClO4 | Perchloric acid | 2 | Oxidized | – |
| MnCl2 | Manganese(II) chloride | 6 | Reduced | – |
| K+ | Potassium ion | 6 | – | – |
| H2O | Water | 2 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of lead(II) chloride and potassium permanganate under acidic condition◆
ΔrG −266.0 kJ/mol K 3.99 × 1046 pK −46.60
| 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 | −501.9 | −266.0 | −793.6 | – |
per 1 mol of | −71.70 | −38.00 | −113.4 | – |
per 1 mol of | −83.65 | −44.33 | −132.3 | – |
per 1 mol of Hydrogen ion | −83.65 | −44.33 | −132.3 | – |
per 1 mol of | −71.70 | −38.00 | −113.4 | – |
per 1 mol of | −250.9 | −133.0 | −396.8 | – |
per 1 mol of | −83.65 | −44.33 | −132.3 | – |
per 1 mol of Potassium ion | −83.65 | −44.33 | −132.3 | – |
per 1 mol of | −250.9 | −133.0 | −396.8 | – |
Changes in standard condition (2)
- Reaction of lead(II) chloride and potassium permanganate under acidic condition◆
ΔrG −273.2 kJ/mol K 7.29 × 1047 pK −47.86
| 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 | – | −273.2 | – | – |
per 1 mol of | – | −39.03 | – | – |
per 1 mol of | – | −45.53 | – | – |
per 1 mol of Hydrogen ion | – | −45.53 | – | – |
per 1 mol of | – | −39.03 | – | – |
per 1 mol of | – | −136.6 | – | – |
per 1 mol of | – | −45.53 | – | – |
per 1 mol of Potassium ion | – | −45.53 | – | – |
per 1 mol of | – | −136.6 | – | – |
Changes in standard condition (3)
- Reaction of lead(II) chloride and potassium permanganate under acidic condition◆
ΔrG −193.9 kJ/mol K 9.33 × 1033 pK −33.97
| 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 | – | −193.9 | – | – |
per 1 mol of | – | −27.70 | – | – |
per 1 mol of | – | −32.32 | – | – |
per 1 mol of Hydrogen ion | – | −32.32 | – | – |
per 1 mol of | – | −27.70 | – | – |
per 1 mol of | – | −96.95 | – | – |
per 1 mol of | – | −32.32 | – | – |
per 1 mol of Potassium ion | – | −32.32 | – | – |
per 1 mol of | – | −96.95 | – | – |
Changes in standard condition (4)
- Reaction of lead(II) chloride and potassium permanganate under acidic condition◆
ΔrG −201.1 kJ/mol K 1.70 × 1035 pK −35.23
| 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 | – | −201.1 | – | – |
per 1 mol of | – | −28.73 | – | – |
per 1 mol of | – | −33.52 | – | – |
per 1 mol of Hydrogen ion | – | −33.52 | – | – |
per 1 mol of | – | −28.73 | – | – |
per 1 mol of | – | −100.5 | – | – |
per 1 mol of | – | −33.52 | – | – |
per 1 mol of Potassium ion | – | −33.52 | – | – |
per 1 mol of | – | −100.5 | – | – |
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] |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas
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] |
| HClO4 (l) | -40.58[1] | – | – | – |
| HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
| HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
| HClO4 (l) 2 hydrate | -677.98[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] | – |
| K+ (g) | 514.26[1] | – | – | – |
| K+ (ao) | -252.38[1] | -283.27[1] | 102.5[1] | 21.8[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, (l):Liquid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-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°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 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°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · 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°, 514.26 kJ · mol−1
- ^ ΔfH°, -252.38 kJ · mol−1
- ^ ΔfG°, -283.27 kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 21.8 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1