ZnBr2 + 2KF 💧→ ZnF2↓ + 2KBr
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- Reaction of zinc bromide and potassium fluoride
The reaction of zinc bromide and potassium fluoride yields zinc 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 zinc 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 zinc bromide and potassium fluoride
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
ZnBr2 | Zinc 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 |
---|---|---|---|---|
ZnF2 | Zinc fluoride | 1 | Lewis conjugate | Slightly soluble in water |
KBr | Potassium bromide | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of zinc bromide and potassium fluoride◆
ΔrG −87.0 kJ/mol K 1.74 × 1015 pK −15.24
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 | −88.8 | −87.0 | −6.2 | – |
per 1 mol of | −88.8 | −87.0 | −6.2 | – |
per 1 mol of | −44.4 | −43.5 | −3.1 | – |
per 1 mol of | −88.8 | −87.0 | −6.2 | – |
per 1 mol of | −44.4 | −43.5 | −3.1 | – |
Changes in aqueous solution (1)
- Reaction of zinc bromide and potassium fluoride◆
ΔrG −8.7 kJ/mol K 3.34 × 101 pK −1.52
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 | 54.8 | −8.7 | 213.4 | 233 |
per 1 mol of | 54.8 | −8.7 | 213.4 | 233 |
per 1 mol of | 27.4 | −4.3 | 106.7 | 117 |
per 1 mol of | 54.8 | −8.7 | 213.4 | 233 |
per 1 mol of | 27.4 | −4.3 | 106.7 | 117 |
Changes in aqueous solution (2)
- Reaction of zinc bromide and potassium fluoride◆
ΔrG −14.2 kJ/mol K 3.07 × 102 pK −2.49
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 | – | −14.2 | – | – |
per 1 mol of | – | −14.2 | – | – |
per 1 mol of | – | −7.10 | – | – |
per 1 mol of | – | −14.2 | – | – |
per 1 mol of | – | −7.10 | – | – |
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 |
---|---|---|---|---|
ZnBr2 (cr) | -328.65[1] | -312.13[1] | 138.5[1] | – |
ZnBr2 (ai) | -396.98[1] | -354.97[1] | 52.7[1] | -238[1] |
ZnBr2 (ao) | – | -349.4[1] | – | – |
ZnBr2 (cr) 2 hydrate | -937.2[1] | -799.5[1] | 198.7[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, (ai):Ionized aqueous solution, (ao):Un-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 |
---|---|---|---|---|
ZnF2 (cr) | -764.4[1] | -713.3[1] | 73.68[1] | 65.65[1] |
ZnF2 (ai) | -819.14[1] | -704.64[1] | -139.7[1] | -167[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, (ai):Ionized 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°, -328.65 kJ · mol−1
- ^ ΔfG°, -312.13 kJ · mol−1
- ^ S°, 138.5 J · K−1 · mol−1
- ^ ΔfH°, -396.98 kJ · mol−1
- ^ ΔfG°, -354.97 kJ · mol−1
- ^ S°, 52.7 J · K−1 · mol−1
- ^ Cp°, -238. J · K−1 · mol−1
- ^ ΔfG°, -349.4 kJ · mol−1
- ^ ΔfH°, -937.2 kJ · mol−1
- ^ ΔfG°, -799.5 kJ · mol−1
- ^ S°, 198.7 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°, -764.4 kJ · mol−1
- ^ ΔfG°, -713.3 kJ · mol−1
- ^ S°, 73.68 J · K−1 · mol−1
- ^ Cp°, 65.65 J · K−1 · mol−1
- ^ ΔfH°, -819.14 kJ · mol−1
- ^ ΔfG°, -704.64 kJ · mol−1
- ^ S°, -139.7 J · K−1 · mol−1
- ^ Cp°, -167. 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