Pb(CH3COO)2 + Rb2S 💧→ PbS↓ + 2CH3COORb
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The reaction of lead(II) acetate and rubidium sulfide yields lead(II) 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 lead(II) 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 lead(II) acetate and rubidium sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(CH3COO)2 | Lead(II) 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 |
|---|---|---|---|---|
| PbS | Lead(II) sulfide | 1 | Lewis conjugate | Insoluble in water |
| CH3COORb | Rubidium acetate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of lead(II) acetate and rubidium sulfide◆
ΔrG −160.2 kJ/mol K 1.16 × 1028 pK −28.07 - Pb(CH3COO)2Ionized aqueous solution + Rb2SIonized aqueous solutionPbS↓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 | −131.8 | −160.2 | 95.8 | – |
per 1 mol of | −131.8 | −160.2 | 95.8 | – |
per 1 mol of | −131.8 | −160.2 | 95.8 | – |
per 1 mol of | −131.8 | −160.2 | 95.8 | – |
per 1 mol of | −65.90 | −80.10 | 47.9 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) acetate and rubidium sulfide◆
ΔrG −143.6 kJ/mol K 1.44 × 1025 pK −25.16 - Pb(CH3COO)2Un-ionized aqueous solution + Rb2SIonized aqueous solutionPbS↓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 | – | −143.6 | – | – |
per 1 mol of | – | −143.6 | – | – |
per 1 mol of | – | −143.6 | – | – |
per 1 mol of | – | −143.6 | – | – |
per 1 mol of | – | −71.80 | – | – |
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 |
|---|---|---|---|---|
| Pb(CH3COO)2 (cr) | -963.83[1] | – | – | – |
| Pb(CH3COO)2 (ai) | -973.6[1] | -763.04[1] | 182.8[1] | – |
| Pb(CH3COO)2 (ao) | – | -779.7[1] | – | – |
| Pb(CH3COO)2 (cr) 3 hydrate | -1851.50[1] | – | – | – |
| Rb2S (cr) | -360.7[1] | – | – | – |
| Rb2S (ai) | -469.4[1] | -482.0[1] | 228.4[1] | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| PbS (cr) | -100.4[1] | -98.7[1] | 91.2[1] | 49.50[1] |
| CH3COORb (ai) | -737.18[1] | -653.29[1] | 207.9[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°, -963.83 kJ · mol−1
- ^ ΔfH°, -973.6 kJ · mol−1
- ^ ΔfG°, -763.04 kJ · mol−1
- ^ S°, 182.8 J · K−1 · mol−1
- ^ ΔfG°, -779.7 kJ · mol−1
- ^ ΔfH°, -1851.50 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°, -100.4 kJ · mol−1
- ^ ΔfG°, -98.7 kJ · mol−1
- ^ S°, 91.2 J · K−1 · mol−1
- ^ Cp°, 49.50 J · K−1 · mol−1
- ^ ΔfH°, -737.18 kJ · mol−1
- ^ ΔfG°, -653.29 kJ · mol−1
- ^ S°, 207.9 J · K−1 · mol−1