FeCl3 + K3PO4 💧→ FePO4↓ + 3KCl
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The reaction of iron(III) chloride and potassium phosphate yields iron(III) phosphate and potassium chloride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) chloride and potassium phosphate
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(III) chloride and potassium phosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCl3 | Iron(III) chloride | 1 | Lewis acid | Very soluble in water |
| K3PO4 | Potassium phosphate | 1 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FePO4 | Iron(III) phosphate | 1 | Lewis conjugate | Insoluble in water |
| KCl | Potassium chloride | 3 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(III) chloride and potassium phosphate
| 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 | −258.1 | – | – | – |
per 1 mol of | −258.1 | – | – | – |
per 1 mol of | −258.1 | – | – | – |
per 1 mol of | −258.1 | – | – | – |
per 1 mol of | −86.03 | – | – | – |
Changes in aqueous solution (1)
- Reaction of iron(III) chloride and potassium phosphate
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) chloride and potassium phosphate
| 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 | 28.8 | – | – | – |
per 1 mol of | 28.8 | – | – | – |
per 1 mol of | 28.8 | – | – | – |
per 1 mol of | 28.8 | – | – | – |
per 1 mol of | 9.60 | – | – | – |
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 |
|---|---|---|---|---|
| FeCl3 (cr) | -399.49[1] | -334.00[1] | 142.3[1] | 96.65[1] |
| FeCl3 (g) | -254.0[1] | – | – | – |
| FeCl3 (ai) | -550.2[1] | -398.3[1] | -146.4[1] | – |
| FeCl3 (ao) | – | -404.5[1] | – | – |
| FeCl3 (cr) 6 hydrate | -2223.8[1] | – | – | – |
| K3PO4 (cr) | -1950.2[1] | – | – | – |
| K3PO4 (ai) | -2034.7[1] | -1868.7[1] | 87.2[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 |
|---|---|---|---|---|
| FePO4 (cr) | -1297.5[1] | – | – | – |
| FePO4 (cr) 2 hydrate strengite | -1888.2[1] | -1657.5[1] | 171.25[1] | 180.54[1] |
| KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
| KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
| KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[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°, -399.49 kJ · mol−1
- ^ ΔfG°, -334.00 kJ · mol−1
- ^ S°, 142.3 J · K−1 · mol−1
- ^ Cp°, 96.65 J · K−1 · mol−1
- ^ ΔfH°, -254.0 kJ · mol−1
- ^ ΔfH°, -550.2 kJ · mol−1
- ^ ΔfG°, -398.3 kJ · mol−1
- ^ S°, -146.4 J · K−1 · mol−1
- ^ ΔfG°, -404.5 kJ · mol−1
- ^ ΔfH°, -2223.8 kJ · mol−1
- ^ ΔfH°, -1950.2 kJ · mol−1
- ^ ΔfH°, -2034.7 kJ · mol−1
- ^ ΔfG°, -1868.7 kJ · mol−1
- ^ S°, 87.2 J · K−1 · mol−1
- ^ ΔfH°, -1297.5 kJ · mol−1
- ^ ΔfH°, -1888.2 kJ · mol−1
- ^ ΔfG°, -1657.5 kJ · mol−1
- ^ S°, 171.25 J · K−1 · mol−1
- ^ Cp°, 180.54 J · K−1 · mol−1
- ^ ΔfH°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1