6FeBr2 + 4Na3[Fe(CN)6] 💧→ Fe2[Fe(CN)6]↓ + 3Na4[Fe(CN)6] + 4FeBr3
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The reaction of iron(II) bromide and sodium hexacyanidoferrate(III) yields iron(II) hexacyanidoferrate(II), sodium hexacyanidoferrate(II), and iron(III) bromide (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(II) bromide and sodium hexacyanidoferrate(III)
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 iron(II) bromide and sodium hexacyanidoferrate(III)
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
FeBr2 | Iron(II) bromide | 6 | Lewis acid | Very soluble in water |
Na3[Fe(CN)6] | Sodium hexacyanidoferrate(III) | 4 | Lewis base | Soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe2[Fe(CN)6] | Iron(II) hexacyanidoferrate(II) | 1 | Lewis conjugate | Insoluble in water |
Na4[Fe(CN)6] | Sodium hexacyanidoferrate(II) | 3 | Non-redox product | – |
FeBr3 | Iron(III) bromide | 4 | Non-redox product | – |
Thermodynamic changes
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] | – |
Na3[Fe(CN)6] (ai) | -158.6[1] | -56.4[1] | 447.3[1] | – |
* (cr):Crystalline solid, (g):Gas, (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 |
---|---|---|---|---|
Fe2[Fe(CN)6] | – | – | – | – |
Na4[Fe(CN)6] (ai) | -505.0[1] | -352.53[1] | 331.0[1] | – |
FeBr3 (cr) | -268.2[1] | – | – | – |
FeBr3 (g) | -123.8[1] | – | – | – |
FeBr3 (ai) | -413.4[1] | -316.7[1] | -68.6[1] | – |
* (ai):Ionized aqueous solution, (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°, -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°, -158.6 kJ · mol−1
- ^ ΔfG°, -56.4 kJ · mol−1
- ^ S°, 447.3 J · K−1 · mol−1
- ^ ΔfH°, -505.0 kJ · mol−1
- ^ ΔfG°, -352.53 kJ · mol−1
- ^ S°, 331.0 J · K−1 · mol−1
- ^ 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