H2 + Co(OH)2 → Co + 2H2O
Last updated:
- Reaction of and cobalt(II) hydroxide
The reaction of and cobalt(II) hydroxide yields and water. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and cobalt(II) hydroxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and cobalt(II) hydroxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
1 | Reducing | Reducing | ||
Co(OH)2 | Cobalt(II) hydroxide | 1 | Oxidizing | Reducible |
Products
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −24.2 kJ/mol K 1.74 × 104 pK −4.24
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 | – | −24.2 | – | – |
– | −24.2 | – | – | |
per 1 mol of | – | −24.2 | – | – |
– | −24.2 | – | – | |
per 1 mol of | – | −12.1 | – | – |
Changes in standard condition (2)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −23.9 kJ/mol K 1.54 × 104 pK −4.19
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 | – | −23.9 | – | – |
– | −23.9 | – | – | |
per 1 mol of | – | −23.9 | – | – |
– | −23.9 | – | – | |
per 1 mol of | – | −11.9 | – | – |
Changes in standard condition (3)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −20.0 kJ/mol K 3.19 × 103 pK −3.50
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 | −32.0 | −20.0 | −40 | – |
−32.0 | −20.0 | −40 | – | |
per 1 mol of | −32.0 | −20.0 | −40 | – |
−32.0 | −20.0 | −40 | – | |
per 1 mol of | −16.0 | −10.0 | −20 | – |
Changes in standard condition (4)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −19.7 kJ/mol K 2.83 × 103 pK −3.45
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 | −31.5 | −19.7 | −39 | – |
−31.5 | −19.7 | −39 | – | |
per 1 mol of | −31.5 | −19.7 | −39 | – |
−31.5 | −19.7 | −39 | – | |
per 1 mol of | −15.8 | −9.85 | −20 | – |
Changes in standard condition (5)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −16.2 kJ/mol K 6.89 × 102 pK −2.84
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 | – | −16.2 | – | – |
– | −16.2 | – | – | |
per 1 mol of | – | −16.2 | – | – |
– | −16.2 | – | – | |
per 1 mol of | – | −8.10 | – | – |
Changes in standard condition (6)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −15.9 kJ/mol K 6.10 × 102 pK −2.79
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 | – | −15.9 | – | – |
– | −15.9 | – | – | |
per 1 mol of | – | −15.9 | – | – |
– | −15.9 | – | – | |
per 1 mol of | – | −7.95 | – | – |
Changes in aqueous solution (1)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −70.2 kJ/mol K 1.99 × 1012 pK −12.30
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 | – | −70.2 | – | – |
– | −70.2 | – | – | |
per 1 mol of | – | −70.2 | – | – |
– | −70.2 | – | – | |
per 1 mol of | – | −35.1 | – | – |
Changes in aqueous solution (2)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −41.8 kJ/mol K 2.10 × 107 pK −7.32
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 | – | −41.8 | – | – |
– | −41.8 | – | – | |
per 1 mol of | – | −41.8 | – | – |
– | −41.8 | – | – | |
per 1 mol of | – | −20.9 | – | – |
Changes in aqueous solution (3)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −37.6 kJ/mol K 3.87 × 106 pK −6.59
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 | −27.8 | −37.6 | −486 | – |
−27.8 | −37.6 | −486 | – | |
per 1 mol of | −27.8 | −37.6 | −486 | – |
−27.8 | −37.6 | −486 | – | |
per 1 mol of | −13.9 | −18.8 | −243 | – |
Changes in aqueous solution (4)
- Reaction of and cobalt(II) hydroxide◆
ΔrG −33.8 kJ/mol K 8.35 × 105 pK −5.92
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 | – | −33.8 | – | – |
– | −33.8 | – | – | |
per 1 mol of | – | −33.8 | – | – |
– | −33.8 | – | – | |
per 1 mol of | – | −16.9 | – | – |
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 |
---|---|---|---|---|
(g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
(ao) | -4.2[1] | 17.6[1] | 577[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] | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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 |
---|---|---|---|---|
(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)
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1
- ^ 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°, 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