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  3. Ni(NO3)2 + 4H2O 💧⚡→ Ni(OH)2 + 2NH3↑ + 4O2↑

Ni(NO3)2 + 4H2O 💧⚡→ Ni(OH)2 + 2NH3↑ + 4O2↑

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Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
Ni(NO3)2Nickel(II) nitrate + 4H2OWater
💧⚡
⟶
Ni(OH)2Nickel(II) hydroxide + 2NH3↑Ammonia + 4O2↑Oxygen

Electrolysis of aqueous nickel(II) nitrate yields nickel(II) hydroxide, ammonia, and oxygen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
Ni(NO3)2Nickel(II) nitrate + 4H2OWater
💧⚡
⟶
Ni(OH)2Nickel(II) hydroxide + 2NH3↑Ammonia + 4O2↑Oxygen

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 nickel(II) nitrate with water as reducing agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Ni(NO3)2Nickel(II) nitrate1
Oxidizing
Very soluble in water
H2OWater4
Reducing
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ni(OH)2Nickel(II) hydroxide1
–
–
NH3Ammonia2
Reduced
–
O2Oxygen4
Oxidized
–

Thermodynamic changes

Changes in standard condition

Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
Ni(NO3)2Crystalline solid + 4H2OLiquid
💧⚡
⟶
Ni(OH)2Crystalline solid + 2NH3↑Gas + 4O2↑Gas
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
936.5–––
per 1 mol of
936.5–––
per 1 mol of
234.1–––
936.5–––
per 1 mol of
468.3–––
per 1 mol of
234.1–––

Changes in aqueous solution (1)

Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
◆
ΔrG736.9 kJ/mol
K0.80 × 10−129
pK129.10
Ni(NO3)2Ionized aqueous solution + 4H2OLiquid
💧⚡
⟶
Ni(OH)2Crystalline solid + 2NH3↑Gas + 4O2↑Gas
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
990.0736.9850–
per 1 mol of
990.0736.9850–
per 1 mol of
247.5184.2213–
990.0736.9850–
per 1 mol of
495.0368.4425–
per 1 mol of
247.5184.2213–

Changes in aqueous solution (2)

Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
◆
ΔrG802.5 kJ/mol
K0.26 × 10−140
pK140.59
Ni(NO3)2Ionized aqueous solution + 4H2OLiquid
💧⚡
⟶
Ni(OH)2Crystalline solid + 2NH3↑Gas + 4O2↑Un-ionized aqueous solution
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
943.2802.5473–
per 1 mol of
943.2802.5473–
per 1 mol of
235.8200.6118–
943.2802.5473–
per 1 mol of
471.6401.3237–
per 1 mol of
235.8200.6118–

Changes in aqueous solution (3)

Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
◆
ΔrG716.8 kJ/mol
K0.26 × 10−125
pK125.58
Ni(NO3)2Ionized aqueous solution + 4H2OLiquid
💧⚡
⟶
Ni(OH)2Crystalline solid + 2NH3↑Un-ionized aqueous solution + 4O2↑Gas
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
921.6716.8688–
per 1 mol of
921.6716.8688–
per 1 mol of
230.4179.2172–
921.6716.8688–
per 1 mol of
460.8358.4344–
per 1 mol of
230.4179.2172–

Changes in aqueous solution (4)

Electrolysis of aqueous nickel(II) nitrate with water as reducing agent
◆
ΔrG782.4 kJ/mol
K0.85 × 10−137
pK137.07
Ni(NO3)2Ionized aqueous solution + 4H2OLiquid
💧⚡
⟶
Ni(OH)2Crystalline solid + 2NH3↑Un-ionized aqueous solution + 4O2↑Un-ionized aqueous solution
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
874.8782.4311–
per 1 mol of
874.8782.4311–
per 1 mol of
218.7195.677.8–
874.8782.4311–
per 1 mol of
437.4391.2156–
per 1 mol of
218.7195.677.8–

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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(OH)2 (cr)-529.7[1]-447.2[1]88[1]–
Ni(OH)2 (ai)-513.8[1]-360.2[1]-150.2[1]–
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]–
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)