Co(NO3)2 + (NH4)2S 💧→ CoS↓ + 2NH4NO3
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The reaction of cobalt(II) nitrate and ammonium sulfide yields cobalt(II) sulfide and ammonium nitrate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of cobalt(II) nitrate and ammonium sulfide
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of cobalt(II) nitrate and ammonium sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co(NO3)2 | Cobalt(II) nitrate | 1 | Lewis acid | Very soluble in water |
| (NH4)2S | Ammonium sulfide | 1 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CoS | Cobalt(II) sulfide | 1 | Lewis conjugate | Insoluble in water |
| NH4NO3 | Ammonium nitrate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of cobalt(II) nitrate and ammonium sulfide
| 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 | −57.9 | – | – | – |
per 1 mol of | −57.9 | – | – | – |
per 1 mol of | −57.9 | – | – | – |
per 1 mol of | −57.9 | – | – | – |
per 1 mol of | −28.9 | – | – | – |
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 |
|---|---|---|---|---|
| Co(NO3)2 (cr) | -420.5[1] | – | – | – |
| Co(NO3)2 (ai) | -472.8[1] | -276.9[1] | 180[1] | – |
| Co(NO3)2 (cr) 2 hydrate | -1021.7[1] | – | – | – |
| Co(NO3)2 (cr) 3 hydrate | -1325.9[1] | – | – | – |
| Co(NO3)2 (cr) 4 hydrate | -1630.5[1] | – | – | – |
| Co(NO3)2 (cr) 6 hydrate | -2211.20[1] | – | – | 452[1] |
| (NH4)2S (ai) | -231.8[1] | -72.6[1] | 212.1[1] | – |
* (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 |
|---|---|---|---|---|
| CoS (cr) | -82.8[1] | – | – | – |
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
* (cr):Crystalline solid, (ai):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°, -420.5 kJ · mol−1
- ^ ΔfH°, -472.8 kJ · mol−1
- ^ ΔfG°, -276.9 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ ΔfH°, -1021.7 kJ · mol−1
- ^ ΔfH°, -1325.9 kJ · mol−1
- ^ ΔfH°, -1630.5 kJ · mol−1
- ^ ΔfH°, -2211.20 kJ · mol−1
- ^ Cp°, 452. J · K−1 · mol−1
- ^ ΔfH°, -231.8 kJ · mol−1
- ^ ΔfG°, -72.6 kJ · mol−1
- ^ S°, 212.1 J · K−1 · mol−1
- ^ ΔfH°, -82.8 kJ · mol−1
- ^ ΔfH°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 J · K−1 · mol−1