SrBr2 + 2KF 💧→ SrF2↓ + 2KBr
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The reaction of strontium bromide and potassium fluoride yields strontium fluoride and potassium bromide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of strontium bromide and potassium 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 strontium bromide and potassium fluoride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SrBr2 | Strontium bromide | 1 | Lewis acid | Very soluble in water |
| KF | Potassium fluoride | 2 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SrF2 | Strontium fluoride | 1 | Lewis conjugate | Very slightly soluble in water |
| KBr | Potassium bromide | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of strontium bromide and potassium fluoride◆
ΔrG −153.5 kJ/mol K 7.80 × 1026 pK −26.89
| 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 | −151.8 | −153.5 | 5.69 | 1.17 |
per 1 mol of | −151.8 | −153.5 | 5.69 | 1.17 |
per 1 mol of | −75.90 | −76.75 | 2.85 | 0.585 |
per 1 mol of | −151.8 | −153.5 | 5.69 | 1.17 |
per 1 mol of | −75.90 | −76.75 | 2.85 | 0.585 |
Changes in aqueous solution
- Reaction of strontium bromide and potassium fluoride◆
ΔrG −47.8 kJ/mol K 2.37 × 108 pK −8.37
| 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 | −5.2 | −47.8 | 142.3 | – |
per 1 mol of | −5.2 | −47.8 | 142.3 | – |
per 1 mol of | −2.6 | −23.9 | 71.15 | – |
per 1 mol of | −5.2 | −47.8 | 142.3 | – |
per 1 mol of | −2.6 | −23.9 | 71.15 | – |
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 |
|---|---|---|---|---|
| SrBr2 (cr) | -717.6[1] | -697.1[1] | 135.10[1] | 75.35[1] |
| SrBr2 (g) | -410[1] | -444[1] | 323.5[1] | 60.7[1] |
| SrBr2 (ai) | -788.89[1] | -767.39[1] | 132.2[1] | – |
| SrBr2 (cr) 1 hydrate | -1031.4[1] | -954.3[1] | 180[1] | 120.9[1] |
| SrBr2 (cr) 6 hydrate | -2531.3[1] | -2174.1[1] | 406[1] | 343.5[1] |
| KF (cr) | -567.27[1] | -537.75[1] | 66.57[1] | 49.04[1] |
| KF (g) | -325.43[1] | -343.62[1] | 226.41[1] | 35.23[1] |
| KF (ai) | -585.01[1] | -562.06[1] | 88.7[1] | -84.9[1] |
| KF (cr) 2 hydrate | -1163.621[1] | -1021.49[1] | 155.2[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
|---|---|---|---|---|
| SrF2 (cr) | -1216.3[1] | -1164.8[1] | 82.13[1] | 70.00[1] |
| SrF2 (g) | -764.4[1] | -775.3[1] | 291.06[1] | 52.97[1] |
| KBr (cr) | -393.798[1] | -380.66[1] | 95.90[1] | 52.30[1] |
| KBr (g) | -180.08[1] | -212.96[1] | 250.52[1] | 36.920[1] |
| KBr (ai) | -373.92[1] | -387.23[1] | 184.9[1] | -120.1[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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°, -717.6 kJ · mol−1
- ^ ΔfG°, -697.1 kJ · mol−1
- ^ S°, 135.10 J · K−1 · mol−1
- ^ Cp°, 75.35 J · K−1 · mol−1
- ^ ΔfH°, -410. kJ · mol−1
- ^ ΔfG°, -444. kJ · mol−1
- ^ S°, 323.5 J · K−1 · mol−1
- ^ Cp°, 60.7 J · K−1 · mol−1
- ^ ΔfH°, -788.89 kJ · mol−1
- ^ ΔfG°, -767.39 kJ · mol−1
- ^ S°, 132.2 J · K−1 · mol−1
- ^ ΔfH°, -1031.4 kJ · mol−1
- ^ ΔfG°, -954.3 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ Cp°, 120.9 J · K−1 · mol−1
- ^ ΔfH°, -2531.3 kJ · mol−1
- ^ ΔfG°, -2174.1 kJ · mol−1
- ^ S°, 406. J · K−1 · mol−1
- ^ Cp°, 343.5 J · K−1 · mol−1
- ^ ΔfH°, -567.27 kJ · mol−1
- ^ ΔfG°, -537.75 kJ · mol−1
- ^ S°, 66.57 J · K−1 · mol−1
- ^ Cp°, 49.04 J · K−1 · mol−1
- ^ ΔfH°, -325.43 kJ · mol−1
- ^ ΔfG°, -343.62 kJ · mol−1
- ^ S°, 226.41 J · K−1 · mol−1
- ^ Cp°, 35.23 J · K−1 · mol−1
- ^ ΔfH°, -585.01 kJ · mol−1
- ^ ΔfG°, -562.06 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1
- ^ Cp°, -84.9 J · K−1 · mol−1
- ^ ΔfH°, -1163.621 kJ · mol−1
- ^ ΔfG°, -1021.49 kJ · mol−1
- ^ S°, 155.2 J · K−1 · mol−1
- ^ ΔfH°, -1216.3 kJ · mol−1
- ^ ΔfG°, -1164.8 kJ · mol−1
- ^ S°, 82.13 J · K−1 · mol−1
- ^ Cp°, 70.00 J · K−1 · mol−1
- ^ ΔfH°, -764.4 kJ · mol−1
- ^ ΔfG°, -775.3 kJ · mol−1
- ^ S°, 291.06 J · K−1 · mol−1
- ^ Cp°, 52.97 J · K−1 · mol−1
- ^ ΔfH°, -393.798 kJ · mol−1
- ^ ΔfG°, -380.66 kJ · mol−1
- ^ S°, 95.90 J · K−1 · mol−1
- ^ Cp°, 52.30 J · K−1 · mol−1
- ^ ΔfH°, -180.08 kJ · mol−1
- ^ ΔfG°, -212.96 kJ · mol−1
- ^ S°, 250.52 J · K−1 · mol−1
- ^ Cp°, 36.920 J · K−1 · mol−1
- ^ ΔfH°, -373.92 kJ · mol−1
- ^ ΔfG°, -387.23 kJ · mol−1
- ^ S°, 184.9 J · K−1 · mol−1
- ^ Cp°, -120.1 J · K−1 · mol−1