15Co(OH)2 + 2KMnO4 → 5Co3O4 + 2MnO + 2KOH + 14H2O
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The reaction of cobalt(II) hydroxide and potassium permanganate yields cobalt(II,III) oxide, manganese(II) oxide, potassium hydroxide, 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 cobalt(II) hydroxide 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 cobalt(II) hydroxide and potassium permanganate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Co(OH)2 | Cobalt(II) hydroxide | 15 | Reducing | Hardly oxidizable |
KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Co3O4 | Cobalt(II,III) oxide | 5 | Oxidized | – |
MnO | Manganese(II) oxide | 2 | Reduced | – |
KOH | Potassium hydroxide | 2 | – | – |
H2O | Water | 14 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −447 kJ/mol K 2.05 × 1078 pK −78.31
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 | – | −447 | – | – |
per 1 mol of | – | −29.8 | – | – |
per 1 mol of | – | −224 | – | – |
per 1 mol of | – | −89.4 | – | – |
per 1 mol of | – | −224 | – | – |
per 1 mol of | – | −224 | – | – |
per 1 mol of | – | −31.9 | – | – |
Changes in standard condition (2)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −384 kJ/mol K 1.88 × 1067 pK −67.27
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 | −307 | −384 | 240 | – |
per 1 mol of | −20.5 | −25.6 | 16.0 | – |
per 1 mol of | −154 | −192 | 120 | – |
per 1 mol of | −61.4 | −76.8 | 48.0 | – |
per 1 mol of | −154 | −192 | 120 | – |
per 1 mol of | −154 | −192 | 120 | – |
per 1 mol of | −21.9 | −27.4 | 17.1 | – |
Changes in standard condition (3)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −327 kJ/mol K 1.94 × 1057 pK −57.29
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 | – | −327 | – | – |
per 1 mol of | – | −21.8 | – | – |
per 1 mol of | – | −164 | – | – |
per 1 mol of | – | −65.4 | – | – |
per 1 mol of | – | −164 | – | – |
per 1 mol of | – | −164 | – | – |
per 1 mol of | – | −23.4 | – | – |
Changes in aqueous solution (1)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −1010 kJ/mol K 8.80 × 10176 pK −176.94
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 | – | −1010 | – | – |
per 1 mol of | – | −67.33 | – | – |
per 1 mol of | – | −505.0 | – | – |
per 1 mol of | – | −202.0 | – | – |
per 1 mol of | – | −505.0 | – | – |
per 1 mol of | – | −505.0 | – | – |
per 1 mol of | – | −72.14 | – | – |
Changes in aqueous solution (2)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −584 kJ/mol K 2.05 × 10102 pK −102.31
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 | – | −584 | – | – |
per 1 mol of | – | −38.9 | – | – |
per 1 mol of | – | −292 | – | – |
per 1 mol of | – | −117 | – | – |
per 1 mol of | – | −292 | – | – |
per 1 mol of | – | −292 | – | – |
per 1 mol of | – | −41.7 | – | – |
Changes in aqueous solution (3)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −521 kJ/mol K 1.88 × 1091 pK −91.28
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 | −509 | −521 | 21 | – |
per 1 mol of | −33.9 | −34.7 | 1.4 | – |
per 1 mol of | −255 | −261 | 11 | – |
per 1 mol of | −102 | −104 | 4.2 | – |
per 1 mol of | −255 | −261 | 11 | – |
per 1 mol of | −255 | −261 | 11 | – |
per 1 mol of | −36.4 | −37.2 | 1.5 | – |
Changes in aqueous solution (4)
- Reaction of cobalt(II) hydroxide and potassium permanganate◆
ΔrG −464 kJ/mol K 1.95 × 1081 pK −81.29
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 | – | −464 | – | – |
per 1 mol of | – | −30.9 | – | – |
per 1 mol of | – | −232 | – | – |
per 1 mol of | – | −92.8 | – | – |
per 1 mol of | – | −232 | – | – |
per 1 mol of | – | −232 | – | – |
per 1 mol of | – | −33.1 | – | – |
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 |
---|---|---|---|---|
Co(OH)2 (cr) blue, precipitated | – | -450.1[1] | – | – |
Co(OH)2 (cr) pink, precipitated | -539.7[1] | -454.3[1] | 79[1] | – |
Co(OH)2 (cr) pink, precipitated, aged | – | -458.1[1] | – | – |
Co(OH)2 (ai) | -518.0[1] | -369.0[1] | -134[1] | – |
Co(OH)2 (ao) | – | -421.7[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] |
* (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 |
---|---|---|---|---|
Co3O4 (cr) | -891[1] | -774[1] | 102.5[1] | 123.4[1] |
MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
MnO (g) | 124.22[1] | – | – | – |
KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[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
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)
- ^ ΔfG°, -450.1 kJ · mol−1
- ^ ΔfH°, -539.7 kJ · mol−1
- ^ ΔfG°, -454.3 kJ · mol−1
- ^ S°, 79. J · K−1 · mol−1
- ^ ΔfG°, -458.1 kJ · mol−1
- ^ ΔfH°, -518.0 kJ · mol−1
- ^ ΔfG°, -369.0 kJ · mol−1
- ^ S°, -134. J · K−1 · mol−1
- ^ ΔfG°, -421.7 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°, -891. kJ · mol−1
- ^ ΔfG°, -774. kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 kJ · mol−1
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 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