FeBr3 + 3AgOH → 3AgBr + Fe(OH)3
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- Reaction of iron(III) bromide and silver(I) hydroxide
- FeBr3Iron(III) bromide + 3AgOHSilver(I) hydroxide3AgBrSilver(I) bromide + Fe(OH)3Iron(III) hydroxide⟶
The reaction of iron(III) bromide and silver(I) hydroxide yields silver(I) bromide and iron(III) hydroxide (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) bromide and silver(I) hydroxide
- FeBr3Iron(III) bromide + 3AgOHSilver(I) hydroxide3AgBrSilver(I) bromide + Fe(OH)3Iron(III) 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(III) bromide and silver(I) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeBr3 | Iron(III) bromide | 1 | Brønsted acid | Salt of weak base |
| AgOH | Silver(I) hydroxide | 3 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| AgBr | Silver(I) bromide | 3 | Conjugate acid | Salt of strong base |
| Fe(OH)3 | Iron(III) hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(III) bromide and silver(I) hydroxide◆
ΔrG −182.8 kJ/mol K 1.06 × 1032 pK −32.03
| 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 | – | −182.8 | – | – |
per 1 mol of | – | −182.8 | – | – |
per 1 mol of Silver(I) hydroxide | – | −60.93 | – | – |
per 1 mol of | – | −60.93 | – | – |
per 1 mol of | – | −182.8 | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) bromide and silver(I) hydroxide◆
ΔrG −255.2 kJ/mol K 5.12 × 1044 pK −44.71
| 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 | – | −255.2 | – | – |
per 1 mol of | – | −255.2 | – | – |
per 1 mol of Silver(I) hydroxide | – | −85.07 | – | – |
per 1 mol of | – | −85.07 | – | – |
per 1 mol of | – | −255.2 | – | – |
Changes in aqueous solution (3)
- Reaction of iron(III) bromide and silver(I) hydroxide◆
ΔrG −147.2 kJ/mol K 6.14 × 1025 pK −25.79
| 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 | – | −147.2 | – | – |
per 1 mol of | – | −147.2 | – | – |
per 1 mol of Silver(I) hydroxide | – | −49.07 | – | – |
per 1 mol of | – | −49.07 | – | – |
per 1 mol of | – | −147.2 | – | – |
Changes in aqueous solution (4)
- Reaction of iron(III) bromide and silver(I) hydroxide◆
ΔrG −219.6 kJ/mol K 2.97 × 1038 pK −38.47
| 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 | – | −219.6 | – | – |
per 1 mol of | – | −219.6 | – | – |
per 1 mol of Silver(I) hydroxide | – | −73.20 | – | – |
per 1 mol of | – | −73.20 | – | – |
per 1 mol of | – | −219.6 | – | – |
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 |
|---|---|---|---|---|
| FeBr3 (cr) | -268.2[1] | – | – | – |
| FeBr3 (g) | -123.8[1] | – | – | – |
| FeBr3 (ai) | -413.4[1] | -316.7[1] | -68.6[1] | – |
| AgOH (ai) | -124.415[1] | -80.137[1] | 61.92[1] | -126.8[1] |
| AgOH (ao) | – | -92.0[1] | – | – |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| AgBr (cr) | -100.37[1] | -96.90[1] | 107.1[1] | 52.38[1] |
| AgBr (ai) | -15.98[1] | -26.86[1] | 155.2[1] | -120.1[1] |
| AgBr (ao) | – | -51.0[1] | – | – |
| Fe(OH)3 (cr) precipitated | -823.0[1] | -696.5[1] | 106.7[1] | – |
| Fe(OH)3 (ao) | – | -659.3[1] | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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°, -268.2 kJ · mol−1
- ^ ΔfH°, -123.8 kJ · mol−1
- ^ ΔfH°, -413.4 kJ · mol−1
- ^ ΔfG°, -316.7 kJ · mol−1
- ^ S°, -68.6 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°, -100.37 kJ · mol−1
- ^ ΔfG°, -96.90 kJ · mol−1
- ^ S°, 107.1 J · K−1 · mol−1
- ^ Cp°, 52.38 J · K−1 · mol−1
- ^ ΔfH°, -15.98 kJ · mol−1
- ^ ΔfG°, -26.86 kJ · mol−1
- ^ S°, 155.2 J · K−1 · mol−1
- ^ Cp°, -120.1 J · K−1 · mol−1
- ^ ΔfG°, -51.0 kJ · mol−1
- ^ ΔfH°, -823.0 kJ · mol−1
- ^ ΔfG°, -696.5 kJ · mol−1
- ^ S°, 106.7 J · K−1 · mol−1
- ^ ΔfG°, -659.3 kJ · mol−1