Pb(NO3)2 + Rb2S 💧→ PbS↓ + 2RbNO3
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The reaction of lead(II) nitrate and rubidium sulfide yields lead(II) sulfide and rubidium nitrate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) nitrate 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) nitrate and rubidium sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(NO3)2 | Lead(II) nitrate | 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 |
| RbNO3 | Rubidium nitrate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) nitrate and rubidium 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 | −277.9 | – | – | – |
per 1 mol of | −277.9 | – | – | – |
per 1 mol of | −277.9 | – | – | – |
per 1 mol of | −277.9 | – | – | – |
per 1 mol of | −138.9 | – | – | – |
Changes in aqueous solution
- Reaction of lead(II) nitrate and rubidium sulfide◆
ΔrG −160.3 kJ/mol K 1.21 × 1028 pK −28.08
| 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 | −131.7 | −160.3 | 95.1 | – |
per 1 mol of | −131.7 | −160.3 | 95.1 | – |
per 1 mol of | −131.7 | −160.3 | 95.1 | – |
per 1 mol of | −131.7 | −160.3 | 95.1 | – |
per 1 mol of | −65.85 | −80.15 | 47.5 | – |
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(NO3)2 (cr) | -451.9[1] | – | – | – |
| Pb(NO3)2 (ai) | -416.3[1] | -246.93[1] | 303.3[1] | – |
| Rb2S (cr) | -360.7[1] | – | – | – |
| Rb2S (ai) | -469.4[1] | -482.0[1] | 228.4[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 |
|---|---|---|---|---|
| PbS (cr) | -100.4[1] | -98.7[1] | 91.2[1] | 49.50[1] |
| RbNO3 (cr) | -495.05[1] | -395.78[1] | 147.3[1] | 102.1[1] |
| RbNO3 (ai) | -458.52[1] | -395.24[1] | 267.8[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°, -451.9 kJ · mol−1
- ^ ΔfH°, -416.3 kJ · mol−1
- ^ ΔfG°, -246.93 kJ · mol−1
- ^ S°, 303.3 J · K−1 · 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°, -495.05 kJ · mol−1
- ^ ΔfG°, -395.78 kJ · mol−1
- ^ S°, 147.3 J · K−1 · mol−1
- ^ Cp°, 102.1 J · K−1 · mol−1
- ^ ΔfH°, -458.52 kJ · mol−1
- ^ ΔfG°, -395.24 kJ · mol−1
- ^ S°, 267.8 J · K−1 · mol−1