2Al(NO3)3 + 9H2O 💧⚡→ 2Al(OH)3 + 3N2H4 + 7O3↑
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- Electrolysis of aqueous aluminium nitrate with water as reducing agent
Electrolysis of aqueous aluminium nitrate yields aluminium hydroxide, hydrazine, 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 aluminium nitrate with water as reducing agent
General equation
- Electrolysis of aqueous solution with water as reducing agent
- Miscible with water/Very soluble in water/Soluble in waterOxidizing agent + H2OReducing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous aluminium nitrate with water as reducing agent
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Al(NO3)3 | Aluminium nitrate | 2 | Oxidizing | Very soluble in water |
H2O | Water | 9 | Reducing | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Al(OH)3 | Aluminium hydroxide | 2 | – | – |
N2H4 | Hydrazine | 3 | Reduced | – |
7 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Electrolysis of aqueous aluminium nitrate with water as reducing agent◆
ΔrG 2689 kJ/mol K 0.81 × 10−471 pK 471.09
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 | 3416 | 2689 | 1364 | – |
per 1 mol of | 1708 | 1345 | 682.0 | – |
per 1 mol of | 379.6 | 298.8 | 151.6 | – |
per 1 mol of | 1708 | 1345 | 682.0 | – |
per 1 mol of | 1139 | 896.3 | 454.7 | – |
488.0 | 384.1 | 194.9 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous aluminium nitrate with water as reducing agent◆
ΔrG 2765 kJ/mol K 0.39 × 10−484 pK 484.41
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 | 3299 | 2765 | 714 | – |
per 1 mol of | 1650 | 1383 | 357 | – |
per 1 mol of | 366.6 | 307.2 | 79.3 | – |
per 1 mol of | 1650 | 1383 | 357 | – |
per 1 mol of | 1100 | 921.7 | 238 | – |
471.3 | 395.0 | 102 | – |
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 |
---|---|---|---|---|
Al(NO3)3 (ai) | -1155[1] | -820[1] | 117.6[1] | – |
Al(NO3)3 (cr) 6 hydrate | -2850.48[1] | -2203.39[1] | 467.8[1] | 433.0[1] |
Al(NO3)3 (cr) 9 hydrate | -3757.06[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] |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (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 |
---|---|---|---|---|
Al(OH)3 (cr) | -1284[2] | -1306[2] | 71[2] | 93.1[2] |
Al(OH)3 (am) | -1276[1] | – | – | – |
N2H4 (l) | 50.63[1] | 149.34[1] | 121.21[1] | 98.87[1] |
N2H4 (g) | 95.40[1] | 159.35[1] | 238.47[1] | 49.58[1] |
N2H4 (ao) | 34.31[1] | 128.1[1] | 138[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, (am):Amorphous solid, (l):Liquid, (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°, -1155. kJ · mol−1
- ^ ΔfG°, -820. kJ · mol−1
- ^ S°, 117.6 J · K−1 · mol−1
- ^ ΔfH°, -2850.48 kJ · mol−1
- ^ ΔfG°, -2203.39 kJ · mol−1
- ^ S°, 467.8 J · K−1 · mol−1
- ^ Cp°, 433.0 J · K−1 · mol−1
- ^ ΔfH°, -3757.06 kJ · 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°, -1276. kJ · mol−1
- ^ ΔfH°, 50.63 kJ · mol−1
- ^ ΔfG°, 149.34 kJ · mol−1
- ^ S°, 121.21 J · K−1 · mol−1
- ^ Cp°, 98.87 J · K−1 · mol−1
- ^ ΔfH°, 95.40 kJ · mol−1
- ^ ΔfG°, 159.35 kJ · mol−1
- ^ S°, 238.47 J · K−1 · mol−1
- ^ Cp°, 49.58 J · K−1 · mol−1
- ^ ΔfH°, 34.31 kJ · mol−1
- ^ ΔfG°, 128.1 kJ · mol−1
- ^ S°, 138. 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
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfH°, -1284 kJ · mol−1 - p.254
- ^ ΔfG°, -1306 kJ · mol−1 - p.254
- ^ S°, 71 J · K−1 · mol−1 - p.254
- ^ Cp°, 93.1 J · K−1 · mol−1 - p.254