Ni(NO3)2 + 2H2O 💧⚡→ Ni + H2O2 + 2HNO3
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- Electrolysis of aqueous nickel(II) nitrate with water as non-redox agent
Electrolysis of aqueous nickel(II) nitrate yields , , and nitric acid (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 nickel(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 nickel(II) nitrate with water as non-redox agent
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Ni(NO3)2 | Nickel(II) nitrate | 1 | Oxidizing | Very soluble in water |
H2O | Water | 2 | – | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
1 | Reduced | – | ||
1 | – | – | ||
HNO3 | Nitric acid | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous nickel(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 | 450.8 | – | – | – |
per 1 mol of | 450.8 | – | – | – |
per 1 mol of | 225.4 | – | – | – |
450.8 | – | – | – | |
450.8 | – | – | – | |
per 1 mol of | 225.4 | – | – | – |
Changes in aqueous solution
- Electrolysis of aqueous nickel(II) nitrate with water as non-redox agent◆
ΔrG 386.2 kJ/mol K 0.22 × 10−67 pK 67.66
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 | 434.4 | 386.2 | 162.8 | – |
per 1 mol of | 434.4 | 386.2 | 162.8 | – |
per 1 mol of | 217.2 | 193.1 | 81.40 | – |
434.4 | 386.2 | 162.8 | – | |
434.4 | 386.2 | 162.8 | – | |
per 1 mol of | 217.2 | 193.1 | 81.40 | – |
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 |
---|---|---|---|---|
Ni(NO3)2 (cr) | -415.1[1] | – | – | – |
Ni(NO3)2 (ai) | -468.6[1] | -268.5[1] | 164.0[1] | – |
Ni(NO3)2 (cr) 3 hydrate | -1326.3[1] | – | – | – |
Ni(NO3)2 (cr) 6 hydrate | -2211.7[1] | – | – | 464[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 |
---|---|---|---|---|
(cr) | 0[1] | 0[1] | 29.87[1] | 26.07[1] |
(g) | 429.7[1] | 384.5[1] | 182.193[1] | 23.359[1] |
(l) | -187.78[1] | -120.35[1] | 109.6[1] | 89.1[1] |
(g) | -136.31[1] | -105.57[1] | 232.7[1] | 43.1[1] |
(ao) | -191.17[1] | -134.03[1] | 143.9[1] | – |
HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ao):Un-ionized aqueous solution, (ai):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°, -415.1 kJ · mol−1
- ^ ΔfH°, -468.6 kJ · mol−1
- ^ ΔfG°, -268.5 kJ · mol−1
- ^ S°, 164.0 J · K−1 · mol−1
- ^ ΔfH°, -1326.3 kJ · mol−1
- ^ ΔfH°, -2211.7 kJ · mol−1
- ^ Cp°, 464. 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 29.87 J · K−1 · mol−1
- ^ Cp°, 26.07 J · K−1 · mol−1
- ^ ΔfH°, 429.7 kJ · mol−1
- ^ ΔfG°, 384.5 kJ · mol−1
- ^ S°, 182.193 J · K−1 · mol−1
- ^ Cp°, 23.359 J · K−1 · mol−1
- ^ ΔfH°, -187.78 kJ · mol−1
- ^ ΔfG°, -120.35 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ Cp°, 89.1 J · K−1 · mol−1
- ^ ΔfH°, -136.31 kJ · mol−1
- ^ ΔfG°, -105.57 kJ · mol−1
- ^ S°, 232.7 J · K−1 · mol−1
- ^ Cp°, 43.1 J · K−1 · mol−1
- ^ ΔfH°, -191.17 kJ · mol−1
- ^ ΔfG°, -134.03 kJ · mol−1
- ^ S°, 143.9 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1