4FePO4 + 12H[AuCl4] → 4FeCl3 + 12AuCl3 + P4O10 + 6H2O
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The reaction of iron(III) phosphate and tetrachloridoauric(III) acid yields iron(III) chloride, gold(III) chloride, tetraphosphorus decaoxide, and water (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) phosphate and tetrachloridoauric(III) acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of iron(III) phosphate and tetrachloridoauric(III) acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FePO4 | Iron(III) phosphate | 4 | Brønsted base | Salt of weak acid |
| H[AuCl4] | Tetrachloridoauric(III) acid | 12 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCl3 | Iron(III) chloride | 4 | Conjugate base | Salt of strong acid |
| AuCl3 | Gold(III) chloride | 12 | Conjugate base | Salt of strong acid |
| P4O10 | Tetraphosphorus decaoxide | 1 | – | Acidic oxide |
| H2O | Water | 6 | Conjugate acid | Water |
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 |
|---|---|---|---|---|
| FePO4 (cr) | -1297.5[1] | – | – | – |
| FePO4 (cr) 2 hydrate strengite | -1888.2[1] | -1657.5[1] | 171.25[1] | 180.54[1] |
| H[AuCl4] | – | – | – | – |
* (cr):Crystalline 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 |
|---|---|---|---|---|
| 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] | – | – | – |
| AuCl3 (cr) | -117.6[1] | – | – | – |
| AuCl3 (cr) 2 hydrate | -715.0[1] | – | – | – |
| P4O10 (cr) hexagonal | -2984.0[1] | -2697.7[1] | 228.86[1] | 211.71[1] |
| P4O10 (am) | -3042[1] | – | – | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous solid, (l):Liquid
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°, -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°, -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°, -117.6 kJ · mol−1
- ^ ΔfH°, -715.0 kJ · mol−1
- ^ ΔfH°, -2984.0 kJ · mol−1
- ^ ΔfG°, -2697.7 kJ · mol−1
- ^ S°, 228.86 J · K−1 · mol−1
- ^ Cp°, 211.71 J · K−1 · mol−1
- ^ ΔfH°, -3042. kJ · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1