4Co(OH)2 🔥→ Co3O4 + Co + 4H2O
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- Decomposition of cobalt(II) hydroxide
Decomposition of cobalt(II) hydroxide yields cobalt(II,III) oxide, , 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
- Decomposition of cobalt(II) hydroxide
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of cobalt(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co(OH)2 | Cobalt(II) hydroxide | 4 | – | Thermally decomposable |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co3O4 | Cobalt(II,III) oxide | 1 | Oxidized | – |
| 1 | Reduced | – | ||
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 78 kJ/mol K 0.22 × 10−13 pK 13.67
| 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 | – | 78 | – | – |
per 1 mol of | – | 20 | – | – |
per 1 mol of | – | 78 | – | – |
| – | 78 | – | – | |
per 1 mol of | – | 20 | – | – |
Changes in standard condition (2)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 78 kJ/mol K 0.22 × 10−13 pK 13.67
| 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 | – | 78 | – | – |
per 1 mol of | – | 20 | – | – |
per 1 mol of | – | 78 | – | – |
| – | 78 | – | – | |
per 1 mol of | – | 20 | – | – |
Changes in standard condition (3)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 95 kJ/mol K 0.23 × 10−16 pK 16.64
| 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 | 124 | 95 | 96 | – |
per 1 mol of | 31.0 | 24 | 24 | – |
per 1 mol of | 124 | 95 | 96 | – |
| 124 | 95 | 96 | – | |
per 1 mol of | 31.0 | 24 | 24 | – |
Changes in standard condition (4)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 95 kJ/mol K 0.23 × 10−16 pK 16.64
| 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 | 125 | 95 | 97 | – |
per 1 mol of | 31.3 | 24 | 24 | – |
per 1 mol of | 125 | 95 | 97 | – |
| 125 | 95 | 97 | – | |
per 1 mol of | 31.3 | 24 | 24 | – |
Changes in standard condition (5)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 110 kJ/mol K 0.54 × 10−19 pK 19.27
| 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 | – | 110 | – | – |
per 1 mol of | – | 27.5 | – | – |
per 1 mol of | – | 110 | – | – |
| – | 110 | – | – | |
per 1 mol of | – | 27.5 | – | – |
Changes in standard condition (6)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 110 kJ/mol K 0.54 × 10−19 pK 19.27
| 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 | – | 110 | – | – |
per 1 mol of | – | 27.5 | – | – |
per 1 mol of | – | 110 | – | – |
| – | 110 | – | – | |
per 1 mol of | – | 27.5 | – | – |
Changes in aqueous solution (1)
- Decomposition of cobalt(II) hydroxide◆
ΔrG −36 kJ/mol K 2.03 × 106 pK −6.31
| 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 | – | −36 | – | – |
per 1 mol of | – | −9.0 | – | – |
per 1 mol of | – | −36 | – | – |
| – | −36 | – | – | |
per 1 mol of | – | −9.0 | – | – |
Changes in aqueous solution (2)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 78 kJ/mol K 0.22 × 10−13 pK 13.67
| 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 | – | 78 | – | – |
per 1 mol of | – | 20 | – | – |
per 1 mol of | – | 78 | – | – |
| – | 78 | – | – | |
per 1 mol of | – | 20 | – | – |
Changes in aqueous solution (3)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 95 kJ/mol K 0.23 × 10−16 pK 16.64
| 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 | 124 | 95 | 96 | – |
per 1 mol of | 31.0 | 24 | 24 | – |
per 1 mol of | 124 | 95 | 96 | – |
| 124 | 95 | 96 | – | |
per 1 mol of | 31.0 | 24 | 24 | – |
Changes in aqueous solution (4)
- Decomposition of cobalt(II) hydroxide◆
ΔrG 110 kJ/mol K 0.54 × 10−19 pK 19.27
| 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 | – | 110 | – | – |
per 1 mol of | – | 27.5 | – | – |
per 1 mol of | – | 110 | – | – |
| – | 110 | – | – | |
per 1 mol of | – | 27.5 | – | – |
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 |
|---|---|---|---|---|
| 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] | – | – |
* (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] |
| (cr) α, hexagonal | 0[1] | 0[1] | 30.04[1] | 24.81[1] |
| (cr) β, face centered cubic | 0.46[1] | 0.25[1] | 30.71[1] | – |
| (g) | 424.7[1] | 380.3[1] | 179.515[1] | 23.020[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, (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°, -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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 30.04 J · K−1 · mol−1
- ^ Cp°, 24.81 J · K−1 · mol−1
- ^ ΔfH°, 0.46 kJ · mol−1
- ^ ΔfG°, 0.25 kJ · mol−1
- ^ S°, 30.71 J · K−1 · mol−1
- ^ ΔfH°, 424.7 kJ · mol−1
- ^ ΔfG°, 380.3 kJ · mol−1
- ^ S°, 179.515 J · K−1 · mol−1
- ^ Cp°, 23.020 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