4S + 4Co(OH)2 → CoSO4 + 3CoS + 4H2O
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- Reaction of and cobalt(II) hydroxide
The reaction of and cobalt(II) hydroxide yields cobalt(II) sulfate, cobalt(II) sulfide, 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 self redoxing species and base
- Self-redoxing speciesSelf redox agent + BaseNon-redox agent ⟶ ProductOxidation product + ProductReduction product
- Self redox agent + Hydroxide base ⟶ Oxoacid saltOxidation product + Salt of hydracid/HydrideReduction product + OxideNon-redox product
Oxidation state of each atom
- Reaction of and cobalt(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 4 | – | Self redoxing Nonmetal | ||
| Co(OH)2 | Cobalt(II) hydroxide | 4 | – | Base Hydroxide base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CoSO4 | Cobalt(II) sulfate | 1 | Oxidized | – Oxoacid salt |
| CoS | Cobalt(II) sulfide | 3 | Reduced | – Salt of hydracid |
| H2O | Water | 4 | – | – Hydride |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (2)
- Reaction of and cobalt(II) hydroxide
| 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 | −121.2 | – | – | – |
| −30.30 | – | – | – | |
per 1 mol of | −30.30 | – | – | – |
per 1 mol of | −121.2 | – | – | – |
per 1 mol of | −40.40 | – | – | – |
per 1 mol of | −30.30 | – | – | – |
Changes in standard condition (3)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (4)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (5)
- Reaction of and cobalt(II) hydroxide
| 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 | −122.5 | – | – | – |
| −30.63 | – | – | – | |
per 1 mol of | −30.63 | – | – | – |
per 1 mol of | −122.5 | – | – | – |
per 1 mol of | −40.83 | – | – | – |
per 1 mol of | −30.63 | – | – | – |
Changes in standard condition (6)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (1)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (2)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (3)
- Reaction of and cobalt(II) hydroxide
| 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 | −121.2 | – | – | – |
| −30.30 | – | – | – | |
per 1 mol of | −30.30 | – | – | – |
per 1 mol of | −121.2 | – | – | – |
per 1 mol of | −40.40 | – | – | – |
per 1 mol of | −30.30 | – | – | – |
Changes in aqueous solution (4)
- Reaction of and cobalt(II) hydroxide
| 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 | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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 |
|---|---|---|---|---|
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[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, (g):Gas, (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 |
|---|---|---|---|---|
| CoSO4 (cr) | -888.3[1] | -782.3[1] | 118.0[1] | – |
| CoSO4 (ai) | -967.3[1] | -799.1[1] | -92[1] | – |
| CoSO4 (cr) 6 hydrate | -2683.6[1] | -2235.36[1] | 367.61[1] | 353.38[1] |
| CoSO4 (cr) 7 hydrate | -2979.93[1] | -2473.42[1] | 406.06[1] | 390.49[1] |
| CoS (cr) | -82.8[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 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°, -888.3 kJ · mol−1
- ^ ΔfG°, -782.3 kJ · mol−1
- ^ S°, 118.0 J · K−1 · mol−1
- ^ ΔfH°, -967.3 kJ · mol−1
- ^ ΔfG°, -799.1 kJ · mol−1
- ^ S°, -92. J · K−1 · mol−1
- ^ ΔfH°, -2683.6 kJ · mol−1
- ^ ΔfG°, -2235.36 kJ · mol−1
- ^ S°, 367.61 J · K−1 · mol−1
- ^ Cp°, 353.38 J · K−1 · mol−1
- ^ ΔfH°, -2979.93 kJ · mol−1
- ^ ΔfG°, -2473.42 kJ · mol−1
- ^ S°, 406.06 J · K−1 · mol−1
- ^ Cp°, 390.49 J · K−1 · mol−1
- ^ ΔfH°, -82.8 kJ · 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