FeSO4 + 2CsF 💧→ FeF2↓ + Cs2SO4
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The reaction of iron(II) sulfate and caesium fluoride yields iron(II) fluoride and caesium sulfate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(II) sulfate and caesium fluoride
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(II) sulfate and caesium fluoride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSO4 | Iron(II) sulfate | 1 | Lewis acid | Soluble in water |
| CsF | Caesium fluoride | 2 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeF2 | Iron(II) fluoride | 1 | Lewis conjugate | Slightly soluble in water |
| Cs2SO4 | Caesium sulfate | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(II) sulfate and caesium fluoride◆
ΔrG −120.4 kJ/mol K 1.24 × 1021 pK −21.09
| 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 | −118.9 | −120.4 | 5.8 | 0.25 |
per 1 mol of | −118.9 | −120.4 | 5.8 | 0.250 |
per 1 mol of | −59.45 | −60.20 | 2.9 | 0.125 |
per 1 mol of | −118.9 | −120.4 | 5.8 | 0.250 |
per 1 mol of | −118.9 | −120.4 | 5.8 | 0.250 |
Changes in aqueous solution (1)
- Reaction of iron(II) sulfate and caesium 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 | −60.8 | – | – | – |
per 1 mol of | −60.8 | – | – | – |
per 1 mol of | −30.4 | – | – | – |
per 1 mol of | −60.8 | – | – | – |
per 1 mol of | −60.8 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(II) sulfate and caesium fluoride◆
ΔrG −34.7 kJ/mol K 1.20 × 106 pK −6.08
| 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 | −34.7 | 27.3 | – |
per 1 mol of | −26.9 | −34.7 | 27.3 | – |
per 1 mol of | −13.4 | −17.4 | 13.7 | – |
per 1 mol of | −26.9 | −34.7 | 27.3 | – |
per 1 mol of | −26.9 | −34.7 | 27.3 | – |
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 |
|---|---|---|---|---|
| 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] |
| CsF (cr) | -553.5[1] | -525.5[1] | 92.80[1] | 51.09[1] |
| CsF (g) | -359.0[1] | -375.7[1] | 243.24[1] | 35.86[1] |
| CsF (ai) | -590.91[1] | -570.81[1] | 119.2[1] | – |
| CsF (cr) 1.5 hydrate | -1013.8[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| 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] | – | – | – |
| Cs2SO4 (cr) | -1443.02[1] | -1323.58[1] | 211.92[1] | 134.89[1] |
| Cs2SO4 (g) | -1102.9[1] | – | – | – |
| Cs2SO4 (ai) | -1425.82[1] | -1328.56[1] | 286.2[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (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°, -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°, -553.5 kJ · mol−1
- ^ ΔfG°, -525.5 kJ · mol−1
- ^ S°, 92.80 J · K−1 · mol−1
- ^ Cp°, 51.09 J · K−1 · mol−1
- ^ ΔfH°, -359.0 kJ · mol−1
- ^ ΔfG°, -375.7 kJ · mol−1
- ^ S°, 243.24 J · K−1 · mol−1
- ^ Cp°, 35.86 J · K−1 · mol−1
- ^ ΔfH°, -590.91 kJ · mol−1
- ^ ΔfG°, -570.81 kJ · mol−1
- ^ S°, 119.2 J · K−1 · mol−1
- ^ ΔfH°, -1013.8 kJ · mol−1
- ^ 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°, -1443.02 kJ · mol−1
- ^ ΔfG°, -1323.58 kJ · mol−1
- ^ S°, 211.92 J · K−1 · mol−1
- ^ Cp°, 134.89 J · K−1 · mol−1
- ^ ΔfH°, -1102.9 kJ · mol−1
- ^ ΔfH°, -1425.82 kJ · mol−1
- ^ ΔfG°, -1328.56 kJ · mol−1
- ^ S°, 286.2 J · K−1 · mol−1