ZnCl2 + BeF2 💧→ ZnF2↓ + BeCl2
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The reaction of zinc chloride and beryllium fluoride yields zinc fluoride and beryllium chloride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of zinc chloride and beryllium 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 chloride and beryllium fluoride
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
ZnCl2 | Zinc chloride | 1 | Lewis acid | Very soluble in water |
BeF2 | Beryllium fluoride | 1 | 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 |
BeCl2 | Beryllium chloride | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of zinc chloride and beryllium fluoride◆
ΔrG 189.9 kJ/mol K 0.54 × 10−33 pK 33.27
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 | 187.1 | 189.9 | −8.45 | 7.32 |
per 1 mol of | 187.1 | 189.9 | −8.45 | 7.32 |
per 1 mol of | 187.1 | 189.9 | −8.45 | 7.32 |
per 1 mol of | 187.1 | 189.9 | −8.45 | 7.32 |
per 1 mol of | 187.1 | 189.9 | −8.45 | 7.32 |
Changes in standard condition (2)
- Reaction of zinc chloride and beryllium fluoride◆
ΔrG 186.6 kJ/mol K 0.20 × 10−32 pK 32.69
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 | 181.7 | 186.6 | −15.32 | 4.90 |
per 1 mol of | 181.7 | 186.6 | −15.32 | 4.90 |
per 1 mol of | 181.7 | 186.6 | −15.32 | 4.90 |
per 1 mol of | 181.7 | 186.6 | −15.32 | 4.90 |
per 1 mol of | 181.7 | 186.6 | −15.32 | 4.90 |
Changes in standard condition (3)
- Reaction of zinc chloride and beryllium 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 | 184.1 | – | – | – |
per 1 mol of | 184.1 | – | – | – |
per 1 mol of | 184.1 | – | – | – |
per 1 mol of | 184.1 | – | – | – |
per 1 mol of | 184.1 | – | – | – |
Changes in standard condition (4)
- Reaction of zinc chloride and beryllium 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 | 178.7 | – | – | – |
per 1 mol of | 178.7 | – | – | – |
per 1 mol of | 178.7 | – | – | – |
per 1 mol of | 178.7 | – | – | – |
per 1 mol of | 178.7 | – | – | – |
Changes in aqueous solution (1)
- Reaction of zinc chloride and beryllium 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 | 53.9 | – | – | – |
per 1 mol of | 53.9 | – | – | – |
per 1 mol of | 53.9 | – | – | – |
per 1 mol of | 53.9 | – | – | – |
per 1 mol of | 53.9 | – | – | – |
Changes in aqueous solution (2)
- Reaction of zinc chloride and beryllium 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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 |
---|---|---|---|---|
ZnCl2 (cr) | -415.05[1] | -369.398[1] | 111.46[1] | 71.34[1] |
ZnCl2 (g) | -266.1[1] | – | – | – |
ZnCl2 (ai) | -488.19[1] | -409.50[1] | 0.8[1] | -226[1] |
ZnCl2 (ao) | – | -403.7[1] | – | – |
BeF2 (cr) α, quartz | -1026.8[1] | -979.4[1] | 53.35[1] | 51.84[1] |
BeF2 (cr) β, cristobalite | -1023.8[1] | – | – | – |
BeF2 (vit) | -1022.2[1] | – | – | – |
BeF2 (g) | -793.7[1] | – | – | – |
BeF2 (aq) | -1046.0[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (vit):Vitreous liquid, (aq):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 |
---|---|---|---|---|
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] |
BeCl2 (cr) α | -490.4[1] | -445.6[1] | 82.68[1] | 64.85[1] |
BeCl2 (cr) β | -495.8[1] | -448.9[1] | 75.81[1] | 62.43[1] |
BeCl2 (g) | -358.6[1] | – | – | – |
BeCl2 (aq) | -715.9[1] | – | – | – |
BeCl2 (cr) 4 hydrate | -1808.3[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (aq):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°, -415.05 kJ · mol−1
- ^ ΔfG°, -369.398 kJ · mol−1
- ^ S°, 111.46 J · K−1 · mol−1
- ^ Cp°, 71.34 J · K−1 · mol−1
- ^ ΔfH°, -266.1 kJ · mol−1
- ^ ΔfH°, -488.19 kJ · mol−1
- ^ ΔfG°, -409.50 kJ · mol−1
- ^ S°, 0.8 J · K−1 · mol−1
- ^ Cp°, -226. J · K−1 · mol−1
- ^ ΔfG°, -403.7 kJ · mol−1
- ^ ΔfH°, -1026.8 kJ · mol−1
- ^ ΔfG°, -979.4 kJ · mol−1
- ^ S°, 53.35 J · K−1 · mol−1
- ^ Cp°, 51.84 J · K−1 · mol−1
- ^ ΔfH°, -1023.8 kJ · mol−1
- ^ ΔfH°, -1022.2 kJ · mol−1
- ^ ΔfH°, -793.7 kJ · mol−1
- ^ ΔfH°, -1046.0 kJ · 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°, -490.4 kJ · mol−1
- ^ ΔfG°, -445.6 kJ · mol−1
- ^ S°, 82.68 J · K−1 · mol−1
- ^ Cp°, 64.85 J · K−1 · mol−1
- ^ ΔfH°, -495.8 kJ · mol−1
- ^ ΔfG°, -448.9 kJ · mol−1
- ^ S°, 75.81 J · K−1 · mol−1
- ^ Cp°, 62.43 J · K−1 · mol−1
- ^ ΔfH°, -358.6 kJ · mol−1
- ^ ΔfH°, -715.9 kJ · mol−1
- ^ ΔfH°, -1808.3 kJ · mol−1