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Ni(NO3)2 + 2H2O 💧⚡→ Ni + H2O2 + 2HNO3

Electrolysis of aqueous nickel(II) nitrate with water as non-redox agent

Electrolysis of aqueous nickel(II) nitrate yields nickel, hydrogen peroxide, and nitric acid (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 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 formulaNameCoefficientTypeType in general
equation
Ni(NO3)2Nickel(II) nitrate1
Oxidizing
Very soluble in water
H2OWater2
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
NiNickel1
Reduced
H2O2Hydrogen peroxide1
HNO3Nitric acid2

Thermodynamic changes

Changes in standard condition

Electrolysis of aqueous nickel(II) nitrate with water as non-redox agent
Ni(NO3)2Crystalline solid + 2H2OLiquid
💧⚡
NiCrystalline solid + H2O2Liquid + 2HNO3Liquid
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
per 1 mol of
450.8
per 1 mol of
450.8
per 1 mol of
225.4

Changes in aqueous solution

Electrolysis of aqueous nickel(II) nitrate with water as non-redox agent
ΔrG386.2 kJ/mol
K0.22 × 10−67
pK67.66
Ni(NO3)2Ionized aqueous solution + 2H2OLiquid
💧⚡
NiCrystalline solid + H2O2Un-ionized aqueous solution + 2HNO3Ionized 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
434.4386.2162.8
per 1 mol of
434.4386.2162.8
per 1 mol of
217.2193.181.40
per 1 mol of
434.4386.2162.8
per 1 mol of
434.4386.2162.8
per 1 mol of
217.2193.181.40

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 (cr)0[1]0[1]29.87[1]26.07[1]
Ni (g)429.7[1]384.5[1]182.193[1]23.359[1]
H2O2 (l)-187.78[1]-120.35[1]109.6[1]89.1[1]
H2O2 (g)-136.31[1]-105.57[1]232.7[1]43.1[1]
H2O2 (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

  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)