Sr(CH3COO)2 + Rb2S 💧→ SrS↓ + 2CH3COORb
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The reaction of strontium acetate and rubidium sulfide yields strontium sulfide and rubidium 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 rubidium 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 rubidium sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Sr(CH3COO)2 | Strontium acetate | 1 | Lewis acid | Very soluble in water |
| Rb2S | Rubidium 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 |
| CH3COORb | Rubidium acetate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of strontium acetate and rubidium sulfide
- Sr(CH3COO)2Aqueous solution + Rb2SIonized aqueous solutionSrS↓Crystalline solid + 2CH3COORbIonized 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 | 34.7 | – | – | – |
per 1 mol of | 34.7 | – | – | – |
per 1 mol of | 34.7 | – | – | – |
per 1 mol of | 34.7 | – | – | – |
per 1 mol of | 17.4 | – | – | – |
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] | – | – | – |
| Rb2S (cr) | -360.7[1] | – | – | – |
| Rb2S (ai) | -469.4[1] | -482.0[1] | 228.4[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] | – | – | – |
| CH3COORb (ai) | -737.18[1] | -653.29[1] | 207.9[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°, -360.7 kJ · mol−1
- ^ ΔfH°, -469.4 kJ · mol−1
- ^ ΔfG°, -482.0 kJ · mol−1
- ^ S°, 228.4 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°, -737.18 kJ · mol−1
- ^ ΔfG°, -653.29 kJ · mol−1
- ^ S°, 207.9 J · K−1 · mol−1