9Co(NO3)2 + 18H2O 💧⚡→ 3Co3O4 + 9NH4NO3 + 11O3↑
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- Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent
Electrolysis of aqueous cobalt(II) nitrate yields cobalt(II,III) oxide, ammonium nitrate, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent
General equation
- Electrolysis of aqueous solution with water as non redox agent
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co(NO3)2 | Cobalt(II) nitrate | 9 | Self redox agent | Very soluble in water |
| H2O | Water | 18 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co3O4 | Cobalt(II,III) oxide | 3 | Oxidized | – |
| NH4NO3 | Ammonium nitrate | 9 | Reduced | – |
| 11 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent
| 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 | 4536 | – | – | – |
per 1 mol of | 504.0 | – | – | – |
per 1 mol of | 252.0 | – | – | – |
per 1 mol of | 1512 | – | – | – |
per 1 mol of | 504.0 | – | – | – |
| 412.4 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent◆
ΔrG 4519 kJ/mol K 0.20 × 10−791 pK 791.69
| 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 | 5238 | 4519 | 2396 | – |
per 1 mol of | 582.0 | 502.1 | 266.2 | – |
per 1 mol of | 291.0 | 251.1 | 133.1 | – |
per 1 mol of | 1746 | 1506 | 798.7 | – |
per 1 mol of | 582.0 | 502.1 | 266.2 | – |
| 476.2 | 410.8 | 217.8 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent◆
ΔrG 4638 kJ/mol K 0.29 × 10−812 pK 812.54
| 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 | 5053 | 4638 | 1373 | – |
per 1 mol of | 561.4 | 515.3 | 152.6 | – |
per 1 mol of | 280.7 | 257.7 | 76.28 | – |
per 1 mol of | 1684 | 1546 | 457.7 | – |
per 1 mol of | 561.4 | 515.3 | 152.6 | – |
| 459.4 | 421.6 | 124.8 | – |
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 |
|---|---|---|---|---|
| Co(NO3)2 (cr) | -420.5[1] | – | – | – |
| Co(NO3)2 (ai) | -472.8[1] | -276.9[1] | 180[1] | – |
| Co(NO3)2 (cr) 2 hydrate | -1021.7[1] | – | – | – |
| Co(NO3)2 (cr) 3 hydrate | -1325.9[1] | – | – | – |
| Co(NO3)2 (cr) 4 hydrate | -1630.5[1] | – | – | – |
| Co(NO3)2 (cr) 6 hydrate | -2211.20[1] | – | – | 452[1] |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (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 |
|---|---|---|---|---|
| Co3O4 (cr) | -891[1] | -774[1] | 102.5[1] | 123.4[1] |
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -420.5 kJ · mol−1
- ^ ΔfH°, -472.8 kJ · mol−1
- ^ ΔfG°, -276.9 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ ΔfH°, -1021.7 kJ · mol−1
- ^ ΔfH°, -1325.9 kJ · mol−1
- ^ ΔfH°, -1630.5 kJ · mol−1
- ^ ΔfH°, -2211.20 kJ · mol−1
- ^ Cp°, 452. J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1
- ^ ΔfH°, -891. kJ · mol−1
- ^ ΔfG°, -774. kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1