FeBr2 + Mg(OH)2 → MgBr2 + Fe(OH)2
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The reaction of iron(II) bromide and magnesium hydroxide yields magnesium bromide 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) bromide and magnesium 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) bromide and magnesium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeBr2 | Iron(II) bromide | 1 | Brønsted acid | Salt of weak base |
| Mg(OH)2 | Magnesium hydroxide | 1 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgBr2 | Magnesium bromide | 1 | Conjugate acid | Salt of strong base |
| Fe(OH)2 | Iron(II) hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) bromide and magnesium hydroxide◆
ΔrG 81.3 kJ/mol K 0.57 × 10−14 pK 14.24
| 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 | 81.0 | 81.3 | 1 | – |
per 1 mol of | 81.0 | 81.3 | 1 | – |
per 1 mol of | 81.0 | 81.3 | 1 | – |
per 1 mol of | 81.0 | 81.3 | 1 | – |
per 1 mol of | 81.0 | 81.3 | 1 | – |
Changes in standard condition (2)
- Reaction of iron(II) bromide and magnesium hydroxide
| 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 | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
per 1 mol of | 77.0 | – | – | – |
Changes in aqueous solution (1)
- Reaction of iron(II) bromide and magnesium hydroxide◆
ΔrG −28.9 kJ/mol K 1.16 × 105 pK −5.06
| 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 | −22.2 | −28.9 | 24 | – |
per 1 mol of | −22.2 | −28.9 | 24 | – |
per 1 mol of | −22.2 | −28.9 | 24 | – |
per 1 mol of | −22.2 | −28.9 | 24 | – |
per 1 mol of | −22.2 | −28.9 | 24 | – |
Changes in aqueous solution (2)
- Reaction of iron(II) bromide and magnesium hydroxide
| 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 | −26.2 | – | – | – |
per 1 mol of | −26.2 | – | – | – |
per 1 mol of | −26.2 | – | – | – |
per 1 mol of | −26.2 | – | – | – |
per 1 mol of | −26.2 | – | – | – |
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 |
|---|---|---|---|---|
| FeBr2 (cr) | -249.8[1] | -238.1[1] | 140.6[1] | – |
| FeBr2 (g) | -46[1] | – | – | – |
| FeBr2 (ai) | -332.2[1] | -286.81[1] | 27.2[1] | – |
| Mg(OH)2 (cr) | -924.54[1] | -833.51[1] | 63.18[1] | 77.03[1] |
| Mg(OH)2 (am) precipitated | -920.5[1] | – | – | – |
| Mg(OH)2 (g) | -561[1] | – | – | – |
| Mg(OH)2 (ai) | -926.84[1] | -769.4[1] | -159.4[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (am):Amorphous solid
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 |
|---|---|---|---|---|
| MgBr2 (cr) | -524.3[1] | -503.8[1] | 117.2[1] | – |
| MgBr2 (g) | -309.6[1] | – | – | – |
| MgBr2 (ai) | -709.94[1] | -662.7[1] | 26.8[1] | – |
| MgBr2 (cr) 6 hydrate | -2410.0[1] | -2055.7[1] | 397[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, (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°, -249.8 kJ · mol−1
- ^ ΔfG°, -238.1 kJ · mol−1
- ^ S°, 140.6 J · K−1 · mol−1
- ^ ΔfH°, -46. kJ · mol−1
- ^ ΔfH°, -332.2 kJ · mol−1
- ^ ΔfG°, -286.81 kJ · mol−1
- ^ S°, 27.2 J · K−1 · mol−1
- ^ ΔfH°, -924.54 kJ · mol−1
- ^ ΔfG°, -833.51 kJ · mol−1
- ^ S°, 63.18 J · K−1 · mol−1
- ^ Cp°, 77.03 J · K−1 · mol−1
- ^ ΔfH°, -920.5 kJ · mol−1
- ^ ΔfH°, -561. kJ · mol−1
- ^ ΔfH°, -926.84 kJ · mol−1
- ^ ΔfG°, -769.4 kJ · mol−1
- ^ S°, -159.4 J · K−1 · mol−1
- ^ ΔfH°, -524.3 kJ · mol−1
- ^ ΔfG°, -503.8 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -309.6 kJ · mol−1
- ^ ΔfH°, -709.94 kJ · mol−1
- ^ ΔfG°, -662.7 kJ · mol−1
- ^ S°, 26.8 J · K−1 · mol−1
- ^ ΔfH°, -2410.0 kJ · mol−1
- ^ ΔfG°, -2055.7 kJ · mol−1
- ^ S°, 397. 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