Fe2O3 + 6HF 🔥→ 2FeF3 + 3H2O
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- Reaction of iron(III) oxide and hydrogen fluoride
The reaction of iron(III) oxide and hydrogen fluoride yields iron(III) fluoride and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) oxide and hydrogen fluoride
General equation
- Reaction of basic oxide and acid
- Basic oxideBrønsted base + AcidBrønsted acid ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of weakly basic oxide and weak acid
- Weakly basic oxideBrønsted base + Weak acidBrønsted acid ⟶ Salt of weak acid and weak baseConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of iron(III) oxide and hydrogen fluoride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2O3 | Iron(III) oxide | 1 | Brønsted base | Basic oxide Weakly basic oxide |
| HF | Hydrogen fluoride | 6 | Brønsted acid | Acid Weak acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeF3 | Iron(III) fluoride | 2 | Conjugate base | Salt Salt of weak acid and weak base |
| H2O | Water | 3 | Conjugate acid | Water |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(III) oxide and hydrogen fluoride
| 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 | −145.4 | – | – | – |
per 1 mol of | −145.4 | – | – | – |
per 1 mol of | −24.23 | – | – | – |
per 1 mol of | −72.70 | – | – | – |
per 1 mol of | −48.47 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) oxide and hydrogen fluoride◆
ΔrG 129.9 kJ/mol K 0.17 × 10−22 pK 22.76
| 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 | −205.6 | 129.9 | −1124.5 | – |
per 1 mol of | −205.6 | 129.9 | −1124.5 | – |
per 1 mol of | −34.27 | 21.65 | −187.42 | – |
per 1 mol of | −102.8 | 64.95 | −562.25 | – |
per 1 mol of | −68.53 | 43.30 | −374.83 | – |
Changes in aqueous solution (3)
- Reaction of iron(III) oxide and hydrogen fluoride
| 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 | −70.1 | – | – | – |
per 1 mol of | −70.1 | – | – | – |
per 1 mol of | −11.7 | – | – | – |
per 1 mol of | −35.0 | – | – | – |
per 1 mol of | −23.4 | – | – | – |
Changes in aqueous solution (4)
- Reaction of iron(III) oxide and hydrogen fluoride◆
ΔrG 21.8 kJ/mol K 0.15 × 10−3 pK 3.82
| 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 | −130.3 | 21.8 | −509.5 | – |
per 1 mol of | −130.3 | 21.8 | −509.5 | – |
per 1 mol of | −21.72 | 3.63 | −84.92 | – |
per 1 mol of | −65.15 | 10.9 | −254.8 | – |
per 1 mol of | −43.43 | 7.27 | −169.8 | – |
Changes in aqueous solution (5)
- Reaction of iron(III) oxide and hydrogen fluoride
| 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 | −145.4 | – | – | – |
per 1 mol of | −145.4 | – | – | – |
per 1 mol of | −24.23 | – | – | – |
per 1 mol of | −72.70 | – | – | – |
per 1 mol of | −48.47 | – | – | – |
Changes in aqueous solution (6)
- Reaction of iron(III) oxide and hydrogen fluoride◆
ΔrG 129.9 kJ/mol K 0.17 × 10−22 pK 22.76
| 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 | −205.6 | 129.9 | −1124.5 | – |
per 1 mol of | −205.6 | 129.9 | −1124.5 | – |
per 1 mol of | −34.27 | 21.65 | −187.42 | – |
per 1 mol of | −102.8 | 64.95 | −562.25 | – |
per 1 mol of | −68.53 | 43.30 | −374.83 | – |
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 |
|---|---|---|---|---|
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[1] | – |
* (cr):Crystalline solid, (l):Liquid, (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 |
|---|---|---|---|---|
| FeF3 (ai) | -1046.4[1] | -840.9[1] | -357.3[1] | – |
| FeF3 (aq) | -1016.3[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] |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (l):Liquid, (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°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 J · K−1 · mol−1
- ^ ΔfH°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1
- ^ ΔfH°, -1046.4 kJ · mol−1
- ^ ΔfG°, -840.9 kJ · mol−1
- ^ S°, -357.3 J · K−1 · mol−1
- ^ ΔfH°, -1016.3 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