2AgNO3 + (NH4)2S 💧→ Ag2S↓ + 2NH4NO3
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The reaction of silver(I) nitrate and ammonium sulfide yields silver(I) 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 silver(I) 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 silver(I) nitrate and ammonium sulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AgNO3 | Silver(I) nitrate | 2 | 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 |
|---|---|---|---|---|
| Ag2S | Silver(I) sulfide | 1 | Lewis conjugate | Insoluble in water |
| NH4NO3 | Ammonium nitrate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of silver(I) nitrate and ammonium sulfide◆
ΔrG −280.9 kJ/mol K 1.63 × 1049 pK −49.21
| 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 | −276.9 | −280.9 | 13.1 | – |
per 1 mol of | −138.4 | −140.4 | 6.55 | – |
per 1 mol of | −276.9 | −280.9 | 13.1 | – |
per 1 mol of | −276.9 | −280.9 | 13.1 | – |
per 1 mol of | −138.4 | −140.4 | 6.55 | – |
Changes in aqueous solution (2)
- Reaction of silver(I) nitrate and ammonium sulfide◆
ΔrG −284.2 kJ/mol K 6.16 × 1049 pK −49.79
| 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 | – | −284.2 | – | – |
per 1 mol of | – | −142.1 | – | – |
per 1 mol of | – | −284.2 | – | – |
per 1 mol of | – | −284.2 | – | – |
per 1 mol of | – | −142.1 | – | – |
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 |
|---|---|---|---|---|
| AgNO3 (cr) | -124.39[1] | -33.41[1] | 140.92[1] | 93.05[1] |
| AgNO3 (ai) | -101.80[1] | -34.16[1] | 219.2[1] | -64.9[1] |
| AgNO3 (ao) | – | -32.49[1] | – | – |
| (NH4)2S (ai) | -231.8[1] | -72.6[1] | 212.1[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 |
|---|---|---|---|---|
| Ag2S (cr) α, orthorhombic | -32.59[1] | -40.67[1] | 144.01[1] | 76.53[1] |
| Ag2S (cr) β | -29.41[1] | -39.46[1] | 150.6[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°, -124.39 kJ · mol−1
- ^ ΔfG°, -33.41 kJ · mol−1
- ^ S°, 140.92 J · K−1 · mol−1
- ^ Cp°, 93.05 J · K−1 · mol−1
- ^ ΔfH°, -101.80 kJ · mol−1
- ^ ΔfG°, -34.16 kJ · mol−1
- ^ S°, 219.2 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfG°, -32.49 kJ · mol−1
- ^ ΔfH°, -231.8 kJ · mol−1
- ^ ΔfG°, -72.6 kJ · mol−1
- ^ S°, 212.1 J · K−1 · mol−1
- ^ ΔfH°, -32.59 kJ · mol−1
- ^ ΔfG°, -40.67 kJ · mol−1
- ^ S°, 144.01 J · K−1 · mol−1
- ^ Cp°, 76.53 J · K−1 · mol−1
- ^ ΔfH°, -29.41 kJ · mol−1
- ^ ΔfG°, -39.46 kJ · mol−1
- ^ S°, 150.6 J · K−1 · 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