3CdCl2 + 2KMnO4 + 8H+ → 3Cd2+ + 3Cl2↑ + 2MnO2 + 2K+ + 4H2O
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- Reaction of cadmium chloride and potassium permanganate under acidic condition
- 3CdCl2Cadmium chloride + 2KMnO4Potassium permanganate + 8H+Hydrogen ion3Cd2+Cadmium ion + 3↑ + 2MnO2Manganese(IV) oxide + 2K+Potassium ion + 4H2OWater⟶
The reaction of cadmium chloride, potassium permanganate, and hydrogen ion yields cadmium ion, , manganese(IV) oxide, 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 cadmium chloride and potassium permanganate under acidic condition
- 3CdCl2Cadmium chloride + 2KMnO4Potassium permanganate + 8H+Hydrogen ion3Cd2+Cadmium ion + 3↑ + 2MnO2Manganese(IV) oxide + 2K+Potassium ion + 4H2OWater⟶
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 cadmium chloride and potassium permanganate under acidic condition
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CdCl2 | Cadmium chloride | 3 | Reducing | Hardly oxidizable |
KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing under acidic condition |
H+ | Hydrogen ion | 8 | – | Hydrogen ion |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Cd2+ | Cadmium ion | 3 | – | – |
3 | Oxidized | – | ||
MnO2 | Manganese(IV) oxide | 2 | Reduced | – |
K+ | Potassium ion | 2 | – | – |
H2O | Water | 4 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of cadmium chloride and potassium permanganate under acidic condition◆
ΔrG −197.0 kJ/mol K 3.26 × 1034 pK −34.51
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 | −97.6 | −197.0 | 333.8 | – |
per 1 mol of | −32.5 | −65.67 | 111.3 | – |
per 1 mol of | −48.8 | −98.50 | 166.9 | – |
per 1 mol of Hydrogen ion | −12.2 | −24.63 | 41.73 | – |
per 1 mol of Cadmium ion | −32.5 | −65.67 | 111.3 | – |
−32.5 | −65.67 | 111.3 | – | |
per 1 mol of | −48.8 | −98.50 | 166.9 | – |
per 1 mol of Potassium ion | −48.8 | −98.50 | 166.9 | – |
per 1 mol of | −24.4 | −49.25 | 83.45 | – |
Changes in standard condition (2)
- Reaction of cadmium chloride and potassium permanganate under acidic condition◆
ΔrG −176.1 kJ/mol K 7.10 × 1030 pK −30.85
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 | −167.8 | −176.1 | 28 | – |
per 1 mol of | −55.93 | −58.70 | 9.3 | – |
per 1 mol of | −83.90 | −88.05 | 14 | – |
per 1 mol of Hydrogen ion | −20.98 | −22.01 | 3.5 | – |
per 1 mol of Cadmium ion | −55.93 | −58.70 | 9.3 | – |
−55.93 | −58.70 | 9.3 | – | |
per 1 mol of | −83.90 | −88.05 | 14 | – |
per 1 mol of Potassium ion | −83.90 | −88.05 | 14 | – |
per 1 mol of | −41.95 | −44.02 | 7.0 | – |
Changes in standard condition (3)
- Reaction of cadmium chloride and potassium permanganate under acidic condition◆
ΔrG −139.3 kJ/mol K 2.54 × 1024 pK −24.40
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 | −113.2 | −139.3 | 87.5 | – |
per 1 mol of | −37.73 | −46.43 | 29.2 | – |
per 1 mol of | −56.60 | −69.65 | 43.8 | – |
per 1 mol of Hydrogen ion | −14.15 | −17.41 | 10.9 | – |
per 1 mol of Cadmium ion | −37.73 | −46.43 | 29.2 | – |
−37.73 | −46.43 | 29.2 | – | |
per 1 mol of | −56.60 | −69.65 | 43.8 | – |
per 1 mol of Potassium ion | −56.60 | −69.65 | 43.8 | – |
per 1 mol of | −28.30 | −34.83 | 21.9 | – |
Changes in standard condition (4)
- Reaction of cadmium chloride and potassium permanganate under acidic condition◆
ΔrG −118.5 kJ/mol K 5.76 × 1020 pK −20.76
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 | −183.4 | −118.5 | −219 | – |
per 1 mol of | −61.13 | −39.50 | −73.0 | – |
per 1 mol of | −91.70 | −59.25 | −110 | – |
per 1 mol of Hydrogen ion | −22.93 | −14.81 | −27.4 | – |
per 1 mol of Cadmium ion | −61.13 | −39.50 | −73.0 | – |
−61.13 | −39.50 | −73.0 | – | |
per 1 mol of | −91.70 | −59.25 | −110 | – |
per 1 mol of Potassium ion | −91.70 | −59.25 | −110 | – |
per 1 mol of | −45.85 | −29.63 | −54.8 | – |
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 |
---|---|---|---|---|
CdCl2 (cr) | -391.50[1] | -343.93[1] | 115.27[1] | 74.68[1] |
CdCl2 (ai) | -410.20[1] | -340.068[1] | 39.7[1] | – |
CdCl2 (ao) | -405.0[1] | -359.29[1] | 121.8[1] | – |
CdCl2 (cr) 1 hydrate | -688.44[1] | -586.975[1] | 167.8[1] | – |
CdCl2 (cr) 2.5 hydrate | -1131.94[1] | -943.939[1] | 227.2[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 |
---|---|---|---|---|
Cd2+ (g) | 2623.54[1] | – | – | – |
Cd2+ (ao) | -75.90[1] | -77.612[1] | -73.2[1] | – |
(g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
(ao) | -23.4[1] | 6.94[1] | 121[1] | – |
MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
MnO2 (am) precipitated | -502.5[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] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid, (l):Liquid
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°, -391.50 kJ · mol−1
- ^ ΔfG°, -343.93 kJ · mol−1
- ^ S°, 115.27 J · K−1 · mol−1
- ^ Cp°, 74.68 J · K−1 · mol−1
- ^ ΔfH°, -410.20 kJ · mol−1
- ^ ΔfG°, -340.068 kJ · mol−1
- ^ S°, 39.7 J · K−1 · mol−1
- ^ ΔfH°, -405.0 kJ · mol−1
- ^ ΔfG°, -359.29 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -688.44 kJ · mol−1
- ^ ΔfG°, -586.975 kJ · mol−1
- ^ S°, 167.8 J · K−1 · mol−1
- ^ ΔfH°, -1131.94 kJ · mol−1
- ^ ΔfG°, -943.939 kJ · mol−1
- ^ S°, 227.2 J · K−1 · 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°, 2623.54 kJ · mol−1
- ^ ΔfH°, -75.90 kJ · mol−1
- ^ ΔfG°, -77.612 kJ · mol−1
- ^ S°, -73.2 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°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · 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