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NiO + 2HNO3 → Ni(NO3)2 + H2O

The reaction of nickel(II) oxide and nitric acid yields nickel(II) nitrate and water. This reaction is an acid-base reaction and is classified as follows:

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

Reaction data

Chemical equation

General equation

Reaction of basic oxide and acid
Basic oxideBrønsted base + AcidBrønsted acid
SaltConjugate base + H2OConjugate acid

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NiONickel(II) oxide1
Brønsted base
Basic oxide
Weakly basic oxide
HNO3Nitric acid2
Brønsted acid
Acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ni(NO3)2Nickel(II) nitrate1
Conjugate base
Salt
Salt of strong acid and weak base
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of nickel(II) oxide and nitric acid
NiOCrystalline solid + 2HNO3Liquid
Ni(NO3)2Crystalline solid + H2OLiquid
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
−113.0
per 1 mol of
−113.0
per 1 mol of
−56.50
per 1 mol of
−113.0
per 1 mol of
−113.0

Changes in aqueous solution

Reaction of nickel(II) oxide and nitric acid
ΔrG−71.4 kJ/mol
K3.23 × 1012
pK−12.51
NiOCrystalline solid + 2HNO3Ionized aqueous solution
Ni(NO3)2Ionized aqueous solution + H2OLiquid
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
−100.0−71.4−96.9
per 1 mol of
−100.0−71.4−96.9
per 1 mol of
−50.00−35.7−48.5
per 1 mol of
−100.0−71.4−96.9
per 1 mol of
−100.0−71.4−96.9

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
NiO (cr)-239.7[1]-211.7[1]37.99[1]44.31[1]
NiO (g)314[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]
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

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)