K3[Fe(CN)6] → 3K+ + [Fe(CN)6]3−
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- Electrolytic dissociation of potassium hexacyanidoferrate(III)
- K3[Fe(CN)6]Potassium hexacyanidoferrate(III)3K+Potassium ion + [Fe(CN)6]3−Hexacyanidoferrate(III) ion⟶
Electrolytic dissociation of potassium hexacyanidoferrate(III) yields potassium ion and hexacyanidoferrate(III) ion (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of potassium hexacyanidoferrate(III)
- K3[Fe(CN)6]Potassium hexacyanidoferrate(III)3K+Potassium ion + [Fe(CN)6]3−Hexacyanidoferrate(III) ion⟶
General equation
- Electrolytic dissociation of salt
- SaltLewis conjugate ⟶ CationLewis acid + AnionLewis base
Oxidation state of each atom
- Electrolytic dissociation of potassium hexacyanidoferrate(III)
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K3[Fe(CN)6] | Potassium hexacyanidoferrate(III) | 1 | Lewis conjugate | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K+ | Potassium ion | 3 | Lewis acid | Cation |
| [Fe(CN)6]3− | Hexacyanidoferrate(III) ion | 1 | Lewis base | Anion |
Thermodynamic changes
Changes in standard condition
- Electrolytic dissociation of potassium hexacyanidoferrate(III)◆
ΔrG 9.2 kJ/mol K 0.24 × 10−1 pK 1.61 - K3[Fe(CN)6]Crystalline solid3K+Un-ionized aqueous solution + [Fe(CN)6]3−Un-ionized aqueous solution⟶
| 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 | 54.6 | 9.2 | 151.7 | – |
per 1 mol of | 54.6 | 9.2 | 151.7 | – |
per 1 mol of Potassium ion | 18.2 | 3.1 | 50.57 | – |
per 1 mol of Hexacyanidoferrate(III) ion | 54.6 | 9.2 | 151.7 | – |
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 |
|---|---|---|---|---|
| K3[Fe(CN)6] (cr) | -249.8[1] | -129.6[1] | 426.06[1] | – |
| K3[Fe(CN)6] (ai) | -195.4[1] | -120.4[1] | 577.8[1] | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| K+ (g) | 514.26[1] | – | – | – |
| K+ (ao) | -252.38[1] | -283.27[1] | 102.5[1] | 21.8[1] |
| [Fe(CN)6]3− (ao) | 561.9[1] | 729.4[1] | 270.3[1] | – |
* (g):Gas, (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°, -249.8 kJ · mol−1
- ^ ΔfG°, -129.6 kJ · mol−1
- ^ S°, 426.06 J · K−1 · mol−1
- ^ ΔfH°, -195.4 kJ · mol−1
- ^ ΔfG°, -120.4 kJ · mol−1
- ^ S°, 577.8 J · K−1 · mol−1
- ^ ΔfH°, 514.26 kJ · mol−1
- ^ ΔfH°, -252.38 kJ · mol−1
- ^ ΔfG°, -283.27 kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 21.8 J · K−1 · mol−1
- ^ ΔfH°, 561.9 kJ · mol−1
- ^ ΔfG°, 729.4 kJ · mol−1
- ^ S°, 270.3 J · K−1 · mol−1