FeF3 + 3HNO3 → Fe(NO3)3 + 3HF↑
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The reaction of iron(III) fluoride and nitric acid yields iron(III) nitrate and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(III) fluoride and nitric acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
Oxidation state of each atom
- Reaction of iron(III) fluoride and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeF3 | Iron(III) fluoride | 1 | Brønsted base | Salt of weak acid |
| HNO3 | Nitric acid | 3 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(NO3)3 | Iron(III) nitrate | 1 | Conjugate base | Salt of strong acid |
| HF | Hydrogen fluoride | 3 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 154.4 | – | – | – |
per 1 mol of | 154.4 | – | – | – |
per 1 mol of | 51.47 | – | – | – |
per 1 mol of | 154.4 | – | – | – |
per 1 mol of | 51.47 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 7.4 | – | – | – |
per 1 mol of | 7.4 | – | – | – |
per 1 mol of | 2.5 | – | – | – |
per 1 mol of | 7.4 | – | – | – |
per 1 mol of | 2.5 | – | – | – |
Changes in aqueous solution (3)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 7.4 | – | – | – |
per 1 mol of | 7.4 | – | – | – |
per 1 mol of | 2.5 | – | – | – |
per 1 mol of | 7.4 | – | – | – |
per 1 mol of | 2.5 | – | – | – |
Changes in aqueous solution (4)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 150.2 | – | – | – |
per 1 mol of | 150.2 | – | – | – |
per 1 mol of | 50.07 | – | – | – |
per 1 mol of | 150.2 | – | – | – |
per 1 mol of | 50.07 | – | – | – |
Changes in aqueous solution (5)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 3.2 | – | – | – |
per 1 mol of | 3.2 | – | – | – |
per 1 mol of | 1.1 | – | – | – |
per 1 mol of | 3.2 | – | – | – |
per 1 mol of | 1.1 | – | – | – |
Changes in aqueous solution (6)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 3.2 | – | – | – |
per 1 mol of | 3.2 | – | – | – |
per 1 mol of | 1.1 | – | – | – |
per 1 mol of | 3.2 | – | – | – |
per 1 mol of | 1.1 | – | – | – |
Changes in aqueous solution (7)
- Reaction of iron(III) fluoride and nitric acid◆
ΔrG 16.8 kJ/mol K 0.11 × 10−2 pK 2.94
| 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 | 184.5 | 16.8 | 562.8 | – |
per 1 mol of | 184.5 | 16.8 | 562.8 | – |
per 1 mol of | 61.50 | 5.60 | 187.6 | – |
per 1 mol of | 184.5 | 16.8 | 562.8 | – |
per 1 mol of | 61.50 | 5.60 | 187.6 | – |
Changes in aqueous solution (8)
- Reaction of iron(III) fluoride and nitric acid◆
ΔrG −54.1 kJ/mol K 3.01 × 109 pK −9.48
| 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 | 37.5 | −54.1 | 307.6 | – |
per 1 mol of | 37.5 | −54.1 | 307.6 | – |
per 1 mol of | 12.5 | −18.0 | 102.5 | – |
per 1 mol of | 37.5 | −54.1 | 307.6 | – |
per 1 mol of | 12.5 | −18.0 | 102.5 | – |
Changes in aqueous solution (9)
- Reaction of iron(III) fluoride and nitric acid◆
ΔrG −54.1 kJ/mol K 3.01 × 109 pK −9.48
| 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 | 37.5 | −54.1 | 307.6 | – |
per 1 mol of | 37.5 | −54.1 | 307.6 | – |
per 1 mol of | 12.5 | −18.0 | 102.5 | – |
per 1 mol of | 37.5 | −54.1 | 307.6 | – |
per 1 mol of | 12.5 | −18.0 | 102.5 | – |
Changes in aqueous solution (10)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 180.3 | – | – | – |
per 1 mol of | 180.3 | – | – | – |
per 1 mol of | 60.10 | – | – | – |
per 1 mol of | 180.3 | – | – | – |
per 1 mol of | 60.10 | – | – | – |
Changes in aqueous solution (11)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 33.3 | – | – | – |
per 1 mol of | 33.3 | – | – | – |
per 1 mol of | 11.1 | – | – | – |
per 1 mol of | 33.3 | – | – | – |
per 1 mol of | 11.1 | – | – | – |
Changes in aqueous solution (12)
- Reaction of iron(III) fluoride and nitric acid
| 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 | 33.3 | – | – | – |
per 1 mol of | 33.3 | – | – | – |
per 1 mol of | 11.1 | – | – | – |
per 1 mol of | 33.3 | – | – | – |
per 1 mol of | 11.1 | – | – | – |
Changes in aqueous solution (13)
- Reaction of iron(III) fluoride and nitric acid
| 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 | −30.2 | – | – | – |
per 1 mol of | −30.2 | – | – | – |
per 1 mol of | −10.1 | – | – | – |
per 1 mol of | −30.2 | – | – | – |
per 1 mol of | −10.1 | – | – | – |
Changes in aqueous solution (14)
- Reaction of iron(III) fluoride and nitric acid
| 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 | −34.4 | – | – | – |
per 1 mol of | −34.4 | – | – | – |
per 1 mol of | −11.5 | – | – | – |
per 1 mol of | −34.4 | – | – | – |
per 1 mol of | −11.5 | – | – | – |
Changes in aqueous solution (15)
- Reaction of iron(III) fluoride and nitric acid◆
ΔrG 0.0 kJ/mol K 1.00 × 100 pK 0.00
| 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 | −0.1 | 0.0 | 0.1 | – |
per 1 mol of | −0.10 | 0.0 | 0.10 | – |
per 1 mol of | −0.033 | 0.0 | 0.033 | – |
per 1 mol of | −0.10 | 0.0 | 0.10 | – |
per 1 mol of | −0.033 | 0.0 | 0.033 | – |
Changes in aqueous solution (16)
- Reaction of iron(III) fluoride and nitric acid
| 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 | −4.3 | – | – | – |
per 1 mol of | −4.3 | – | – | – |
per 1 mol of | −1.4 | – | – | – |
per 1 mol of | −4.3 | – | – | – |
per 1 mol of | −1.4 | – | – | – |
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 |
|---|---|---|---|---|
| FeF3 (ai) | -1046.4[1] | -840.9[1] | -357.3[1] | – |
| FeF3 (aq) | -1016.3[1] | – | – | – |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| Fe(NO3)3 (ai) | -670.7[1] | -338.3[1] | 123.4[1] | – |
| Fe(NO3)3 (aq) | -674.9[1] | – | – | – |
| Fe(NO3)3 (cr) 9 hydrate | -3285.3[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] | – |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (l):Liquid, (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°, -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°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -670.7 kJ · mol−1
- ^ ΔfG°, -338.3 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -674.9 kJ · mol−1
- ^ ΔfH°, -3285.3 kJ · 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