Sr(CH3COO)2 + (NH4)2S 💧→ SrS↓ + 2CH3COONH4
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The reaction of strontium acetate and ammonium sulfide yields strontium sulfide and ammonium acetate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of strontium acetate 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 strontium acetate and ammonium sulfide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Sr(CH3COO)2 | Strontium acetate | 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 |
---|---|---|---|---|
SrS | Strontium sulfide | 1 | Lewis conjugate | Slightly soluble in water |
CH3COONH4 | Ammonium acetate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of strontium acetate and ammonium sulfide
- Sr(CH3COO)2Aqueous solution + (NH4)2SIonized aqueous solutionSrS↓Crystalline solid + 2CH3COONH4Ionized aqueous solution💧⟶
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 | 34.5 | – | – | – |
per 1 mol of | 34.5 | – | – | – |
per 1 mol of | 34.5 | – | – | – |
per 1 mol of | 34.5 | – | – | – |
per 1 mol of | 17.3 | – | – | – |
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 |
---|---|---|---|---|
Sr(CH3COO)2 (cr) | -1487.4[1] | – | – | – |
Sr(CH3COO)2 (aq) | -1512.1[1] | – | – | – |
Sr(CH3COO)2 (cr) 0.5 hydrate | -1631.8[1] | – | – | – |
(NH4)2S (ai) | -231.8[1] | -72.6[1] | 212.1[1] | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (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 |
---|---|---|---|---|
SrS (cr) | -472.4[1] | -467.8[1] | 68.2[1] | 48.70[1] |
SrS (g) | 109[1] | – | – | – |
CH3COONH4 (cr) | -616.14[1] | – | – | – |
CH3COONH4 (ai) | -618.52[1] | -448.61[1] | 200.0[1] | 73.6[1] |
* (cr):Crystalline solid, (g):Gas, (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°, -1487.4 kJ · mol−1
- ^ ΔfH°, -1512.1 kJ · mol−1
- ^ ΔfH°, -1631.8 kJ · mol−1
- ^ ΔfH°, -231.8 kJ · mol−1
- ^ ΔfG°, -72.6 kJ · mol−1
- ^ S°, 212.1 J · K−1 · mol−1
- ^ ΔfH°, -472.4 kJ · mol−1
- ^ ΔfG°, -467.8 kJ · mol−1
- ^ S°, 68.2 J · K−1 · mol−1
- ^ Cp°, 48.70 J · K−1 · mol−1
- ^ ΔfH°, 109. kJ · mol−1
- ^ ΔfH°, -616.14 kJ · mol−1
- ^ ΔfH°, -618.52 kJ · mol−1
- ^ ΔfG°, -448.61 kJ · mol−1
- ^ S°, 200.0 J · K−1 · mol−1
- ^ Cp°, 73.6 J · K−1 · mol−1