FeF2 + H2SO4 → FeSO4 + 2HF↑
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The reaction of iron(II) fluoride and sulfuric acid yields iron(II) sulfate 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(II) fluoride and sulfuric acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of iron(II) fluoride and sulfuric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeF2 | Iron(II) fluoride | 1 | Brønsted base | Salt of weak acid Salt of volatile acid |
| H2SO4 | Sulfuric acid | 1 | Brønsted acid | Strong acid Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSO4 | Iron(II) sulfate | 1 | Conjugate base | Salt of strong acid Salt of non volatile acid |
| HF | Hydrogen fluoride | 2 | Conjugate acid | Weak acid Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(II) fluoride and sulfuric acid◆
ΔrG −8.6 kJ/mol K 3.21 × 101 pK −1.51
| 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 | 54.7 | −8.6 | 211.2 | −48.18 |
per 1 mol of | 54.7 | −8.6 | 211.2 | −48.18 |
per 1 mol of | 54.7 | −8.6 | 211.2 | −48.18 |
per 1 mol of | 54.7 | −8.6 | 211.2 | −48.18 |
per 1 mol of | 27.4 | −4.3 | 105.6 | −24.09 |
Changes in aqueous solution (1)
- Reaction of iron(II) fluoride and sulfuric 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 | 183.9 | – | – | – |
per 1 mol of | 183.9 | – | – | – |
per 1 mol of | 183.9 | – | – | – |
per 1 mol of | 183.9 | – | – | – |
per 1 mol of | 91.95 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(II) fluoride and sulfuric 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 | 85.9 | – | – | – |
per 1 mol of | 85.9 | – | – | – |
per 1 mol of | 85.9 | – | – | – |
per 1 mol of | 85.9 | – | – | – |
per 1 mol of | 43.0 | – | – | – |
Changes in aqueous solution (3)
- Reaction of iron(II) fluoride and sulfuric 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 | 85.9 | – | – | – |
per 1 mol of | 85.9 | – | – | – |
per 1 mol of | 85.9 | – | – | – |
per 1 mol of | 85.9 | – | – | – |
per 1 mol of | 43.0 | – | – | – |
Changes in aqueous solution (4)
- Reaction of iron(II) fluoride and sulfuric acid◆
ΔrG 45.9 kJ/mol K 0.91 × 10−8 pK 8.04
| 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 | 150.0 | 45.9 | 348.0 | 384 |
per 1 mol of | 150.0 | 45.9 | 348.0 | 384 |
per 1 mol of | 150.0 | 45.9 | 348.0 | 384 |
per 1 mol of | 150.0 | 45.9 | 348.0 | 384 |
per 1 mol of | 75.00 | 22.9 | 174.0 | 192 |
Changes in aqueous solution (5)
- Reaction of iron(II) fluoride and sulfuric acid◆
ΔrG −1.3 kJ/mol K 1.69 × 100 pK −0.23
| 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 | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 26.0 | −0.65 | 88.90 | – |
Changes in aqueous solution (6)
- Reaction of iron(II) fluoride and sulfuric acid◆
ΔrG −1.3 kJ/mol K 1.69 × 100 pK −0.23
| 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 | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 52.0 | −1.3 | 177.8 | – |
per 1 mol of | 26.0 | −0.65 | 88.90 | – |
Changes in aqueous solution (7)
- Reaction of iron(II) fluoride and sulfuric 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 | 60.8 | – | – | – |
per 1 mol of | 60.8 | – | – | – |
per 1 mol of | 60.8 | – | – | – |
per 1 mol of | 60.8 | – | – | – |
per 1 mol of | 30.4 | – | – | – |
Changes in aqueous solution (8)
- Reaction of iron(II) fluoride and sulfuric acid◆
ΔrG 34.8 kJ/mol K 0.80 × 10−6 pK 6.10
| 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 | 26.9 | 34.8 | −27.2 | 112 |
per 1 mol of | 26.9 | 34.8 | −27.2 | 112 |
per 1 mol of | 26.9 | 34.8 | −27.2 | 112 |
per 1 mol of | 26.9 | 34.8 | −27.2 | 112 |
per 1 mol of | 13.4 | 17.4 | −13.6 | 56.0 |
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 |
|---|---|---|---|---|
| FeF2 (cr) | -711.3[1] | -668.6[1] | 86.99[1] | 68.12[1] |
| FeF2 (ai) | -754.4[1] | -636.48[1] | -165.3[1] | – |
| FeF2 (aq) | -745.2[1] | – | – | – |
| H2SO4 (cr) | – | – | – | – |
| H2SO4 (l) | -813.989[1] | -690.003[1] | 156.904[1] | 138.91[1] |
| H2SO4 (ai) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
| H2SO4 (l) 1 hydrate | -1127.621[1] | -950.383[1] | 211.54[1] | 214.85[1] |
| H2SO4 (l) 2 hydrate | -1427.100[1] | -1199.650[1] | 276.40[1] | 260.83[1] |
| H2SO4 (l) 3 hydrate | -1720.402[1] | -1443.980[1] | 345.39[1] | 318.95[1] |
| H2SO4 (l) 4 hydrate | -2011.199[1] | -1685.863[1] | 414.59[1] | 382.21[1] |
| H2SO4 (l) 6.5 hydrate | -2733.256[1] | -2285.734[1] | 587.89[1] | 570.28[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| FeSO4 (cr) | -928.4[1] | -820.8[1] | 107.5[1] | 100.58[1] |
| FeSO4 (ai) | -998.3[1] | -823.43[1] | -117.6[1] | – |
| FeSO4 (cr) 1 hydrate | -1243.69[1] | – | – | – |
| FeSO4 (cr) 4 hydrate | -2129.2[1] | – | – | – |
| FeSO4 (cr) 7 hydrate | -3014.57[1] | -2509.87[1] | 409.2[1] | 394.47[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, (ai):Ionized aqueous solution, (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°, -711.3 kJ · mol−1
- ^ ΔfG°, -668.6 kJ · mol−1
- ^ S°, 86.99 J · K−1 · mol−1
- ^ Cp°, 68.12 J · K−1 · mol−1
- ^ ΔfH°, -754.4 kJ · mol−1
- ^ ΔfG°, -636.48 kJ · mol−1
- ^ S°, -165.3 J · K−1 · mol−1
- ^ ΔfH°, -745.2 kJ · mol−1
- ^ ΔfH°, -813.989 kJ · mol−1
- ^ ΔfG°, -690.003 kJ · mol−1
- ^ S°, 156.904 J · K−1 · mol−1
- ^ Cp°, 138.91 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1
- ^ ΔfH°, -1127.621 kJ · mol−1
- ^ ΔfG°, -950.383 kJ · mol−1
- ^ S°, 211.54 J · K−1 · mol−1
- ^ Cp°, 214.85 J · K−1 · mol−1
- ^ ΔfH°, -1427.100 kJ · mol−1
- ^ ΔfG°, -1199.650 kJ · mol−1
- ^ S°, 276.40 J · K−1 · mol−1
- ^ Cp°, 260.83 J · K−1 · mol−1
- ^ ΔfH°, -1720.402 kJ · mol−1
- ^ ΔfG°, -1443.980 kJ · mol−1
- ^ S°, 345.39 J · K−1 · mol−1
- ^ Cp°, 318.95 J · K−1 · mol−1
- ^ ΔfH°, -2011.199 kJ · mol−1
- ^ ΔfG°, -1685.863 kJ · mol−1
- ^ S°, 414.59 J · K−1 · mol−1
- ^ Cp°, 382.21 J · K−1 · mol−1
- ^ ΔfH°, -2733.256 kJ · mol−1
- ^ ΔfG°, -2285.734 kJ · mol−1
- ^ S°, 587.89 J · K−1 · mol−1
- ^ Cp°, 570.28 J · K−1 · mol−1
- ^ ΔfH°, -928.4 kJ · mol−1
- ^ ΔfG°, -820.8 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ Cp°, 100.58 J · K−1 · mol−1
- ^ ΔfH°, -998.3 kJ · mol−1
- ^ ΔfG°, -823.43 kJ · mol−1
- ^ S°, -117.6 J · K−1 · mol−1
- ^ ΔfH°, -1243.69 kJ · mol−1
- ^ ΔfH°, -2129.2 kJ · mol−1
- ^ ΔfH°, -3014.57 kJ · mol−1
- ^ ΔfG°, -2509.87 kJ · mol−1
- ^ S°, 409.2 J · K−1 · mol−1
- ^ Cp°, 394.47 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