CoS + Ca(OH)2 → CaS + Co(OH)2
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The reaction of cobalt(II) sulfide and calcium hydroxide yields calcium sulfide and cobalt(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of cobalt(II) sulfide and calcium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of cobalt(II) sulfide and calcium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CoS | Cobalt(II) sulfide | 1 | Brønsted acid | Salt of weak base |
| Ca(OH)2 | Calcium hydroxide | 1 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaS | Calcium sulfide | 1 | Conjugate acid | Salt of strong base |
| Co(OH)2 | Cobalt(II) hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of cobalt(II) sulfide and calcium 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 cobalt(II) sulfide and calcium 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 | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
Changes in standard condition (3)
- Reaction of cobalt(II) sulfide and calcium 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 cobalt(II) sulfide and calcium 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 cobalt(II) sulfide and calcium 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 cobalt(II) sulfide and calcium 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 | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
per 1 mol of | 46.8 | – | – | – |
Changes in aqueous solution (4)
- Reaction of cobalt(II) sulfide and calcium 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 |
|---|---|---|---|---|
| CoS (cr) | -82.8[1] | – | – | – |
| Ca(OH)2 (cr) | -986.09[1] | -898.49[1] | 83.39[1] | 87.49[1] |
| Ca(OH)2 (g) | -544[1] | – | – | – |
| Ca(OH)2 (ai) | -1002.82[1] | -868.07[1] | -74.5[1] | – |
| Ca(OH)2 (cr) 2 hydrate | -1218.4[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| CaS (cr) | -482.4[1] | -477.4[1] | 56.5[1] | 47.40[1] |
| CaS (g) | – | – | – | – |
| 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
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°, -82.8 kJ · mol−1
- ^ ΔfH°, -986.09 kJ · mol−1
- ^ ΔfG°, -898.49 kJ · mol−1
- ^ S°, 83.39 J · K−1 · mol−1
- ^ Cp°, 87.49 J · K−1 · mol−1
- ^ ΔfH°, -544. kJ · mol−1
- ^ ΔfH°, -1002.82 kJ · mol−1
- ^ ΔfG°, -868.07 kJ · mol−1
- ^ S°, -74.5 J · K−1 · mol−1
- ^ ΔfH°, -1218.4 kJ · mol−1
- ^ ΔfH°, -482.4 kJ · mol−1
- ^ ΔfG°, -477.4 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, 47.40 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