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Ni + 4HNO3 → Ni(NO3)2 + 2NO2↑ + 2H2O

Reaction of nickel and nitric acid
⚠️
This reaction may not proceed due to the formation of passive/insoluble surface layer.

The reaction of nickel and nitric acid yields nickel(II) nitrate, nitrogen dioxide, and water (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

Reaction of nickel and nitric acid
⚠️
This reaction may not proceed due to the formation of passive/insoluble surface layer.

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of nickel and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NiNickel1
Reducing
Reducing
HNO3Nitric acid4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ni(NO3)2Nickel(II) nitrate1
Oxidized
NO2Nitrogen dioxide2
Reduced
H2OWater2

Thermodynamic changes

Changes in standard condition

Reaction of nickel and nitric acid
⚠️
This reaction may not proceed due to the formation of passive/insoluble surface layer.
NiCrystalline solid + 4HNO3Liquid
Ni(NO3)2Crystalline solid + 2NO2Gas + 2H2OLiquid
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
−224.0
per 1 mol of
−224.0
per 1 mol of
−56.00
per 1 mol of
−224.0
per 1 mol of
−112.0
per 1 mol of
−112.0

Changes in aqueous solution

Reaction of nickel and nitric acid
⚠️
This reaction may not proceed due to the formation of passive/insoluble surface layer.
ΔrG−195.1 kJ/mol
K1.51 × 1034
pK−34.18
NiCrystalline solid + 4HNO3Ionized aqueous solution
Ni(NO3)2Ionized aqueous solution + 2NO2Gas + 2H2OLiquid
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
−144.5−195.1168.5
per 1 mol of
−144.5−195.1168.5
per 1 mol of
−36.13−48.7742.13
per 1 mol of
−144.5−195.1168.5
per 1 mol of
−72.25−97.5584.25
per 1 mol of
−72.25−97.5584.25

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 (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]
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, (ai):Ionized aqueous solution

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(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]
NO2 (g)33.18[1]51.31[1]240.06[1]37.20[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, (g):Gas, (l):Liquid

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)