FeS + 2AgOH → Ag2S + Fe(OH)2
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- Reaction of iron(II) sulfide and silver(I) hydroxide
The reaction of iron(II) sulfide and silver(I) hydroxide yields silver(I) sulfide and iron(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(II) sulfide and silver(I) hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of iron(II) sulfide and silver(I) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeS | Iron(II) sulfide | 1 | Brønsted acid | Salt of weak base |
| AgOH | Silver(I) hydroxide | 2 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ag2S | Silver(I) sulfide | 1 | Conjugate acid | Salt of strong base |
| Fe(OH)2 | Iron(II) hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(II) sulfide and silver(I) hydroxide◆
ΔrG −266.5 kJ/mol K 4.88 × 1046 pK −46.69
| 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 | −252.8 | −266.5 | 48 | – |
per 1 mol of | −252.8 | −266.5 | 48 | – |
per 1 mol of Silver(I) hydroxide | −126.4 | −133.3 | 24 | – |
per 1 mol of | −252.8 | −266.5 | 48 | – |
per 1 mol of | −252.8 | −266.5 | 48 | – |
Changes in aqueous solution (2)
- Reaction of iron(II) sulfide and silver(I) hydroxide◆
ΔrG −242.8 kJ/mol K 3.44 × 1042 pK −42.54
| 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 | – | −242.8 | – | – |
per 1 mol of | – | −242.8 | – | – |
per 1 mol of Silver(I) hydroxide | – | −121.4 | – | – |
per 1 mol of | – | −242.8 | – | – |
per 1 mol of | – | −242.8 | – | – |
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 |
|---|---|---|---|---|
| FeS (cr) iron-rich pyrrhotite, α | -100.0[1] | -100.4[1] | 60.29[1] | 50.54[1] |
| AgOH (ai) | -124.415[1] | -80.137[1] | 61.92[1] | -126.8[1] |
| AgOH (ao) | – | -92.0[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] | – |
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas
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°, -100.0 kJ · mol−1
- ^ ΔfG°, -100.4 kJ · mol−1
- ^ S°, 60.29 J · K−1 · mol−1
- ^ Cp°, 50.54 J · K−1 · mol−1
- ^ ΔfH°, -124.415 kJ · mol−1
- ^ ΔfG°, -80.137 kJ · mol−1
- ^ S°, 61.92 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfG°, -92.0 kJ · 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°, -569.0 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, 88. J · K−1 · mol−1
- ^ ΔfH°, -372. kJ · mol−1