ZnCl2 💧⚡→ Zn + Cl2↑
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- Electrolysis of aqueous zinc chloride without water as reactant
Electrolysis of aqueous zinc chloride yields and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous zinc chloride without water as reactant
General equation
- Electrolysis of aqueous solution without water as reactant
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous zinc chloride without water as reactant
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnCl2 | Zinc chloride | 1 | Self redox agent | Very soluble in water |
Products
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous zinc chloride without water as reactant◆
ΔrG 369.398 kJ/mol K 0.19 × 10−64 pK 64.72
| 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 | 415.05 | 369.398 | 153.24 | −12.03 |
per 1 mol of | 415.05 | 369.398 | 153.24 | −12.03 |
| 415.05 | 369.398 | 153.24 | −12.03 | |
| 415.05 | 369.398 | 153.24 | −12.03 |
Changes in aqueous solution (1)
- Electrolysis of aqueous zinc chloride without water as reactant◆
ΔrG 409.50 kJ/mol K 0.18 × 10−71 pK 71.74
| 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 | 488.19 | 409.50 | 263.9 | 285 |
per 1 mol of | 488.19 | 409.50 | 263.9 | 285 |
| 488.19 | 409.50 | 263.9 | 285 | |
| 488.19 | 409.50 | 263.9 | 285 |
Changes in aqueous solution (2)
- Electrolysis of aqueous zinc chloride without water as reactant◆
ΔrG 416.44 kJ/mol K 0.11 × 10−72 pK 72.96
| 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 | 464.8 | 416.44 | 162 | – |
per 1 mol of | 464.8 | 416.44 | 162 | – |
| 464.8 | 416.44 | 162 | – | |
| 464.8 | 416.44 | 162 | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous zinc chloride without water as reactant◆
ΔrG 403.7 kJ/mol K 0.19 × 10−70 pK 70.73
| 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 | – | 403.7 | – | – |
per 1 mol of | – | 403.7 | – | – |
| – | 403.7 | – | – | |
| – | 403.7 | – | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous zinc chloride without water as reactant◆
ΔrG 410.6 kJ/mol K 0.12 × 10−71 pK 71.93
| 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 | – | 410.6 | – | – |
per 1 mol of | – | 410.6 | – | – |
| – | 410.6 | – | – | |
| – | 410.6 | – | – |
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] | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 41.63[1] | 25.40[1] |
| (g) | 130.729[1] | 95.145[1] | 160.984[1] | 20.786[1] |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
* (cr):Crystalline solid, (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°, -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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.63 J · K−1 · mol−1
- ^ Cp°, 25.40 J · K−1 · mol−1
- ^ ΔfH°, 130.729 kJ · mol−1
- ^ ΔfG°, 95.145 kJ · mol−1
- ^ S°, 160.984 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1