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10HCl + 2Ni(NO3)2 + 4H+ 🔥→ 5Cl2O + 2N2 + 2Ni2+ + 7H2O

Reaction of hydrogen chloride and nickel(II) nitrate under acidic condition
10HClHydrogen chloride + 2Ni(NO3)2Nickel(II) nitrate + 4H+Hydrogen ion
🔥
5Cl2ODichlorine monoxide + 2N2Nitrogen + 2Ni2+Nickel(II) ion + 7H2OWater

The reaction of hydrogen chloride, nickel(II) nitrate, and hydrogen ion yields dichlorine monoxide, nitrogen, nickel(II) ion, 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 hydrogen chloride and nickel(II) nitrate under acidic condition
10HClHydrogen chloride + 2Ni(NO3)2Nickel(II) nitrate + 4H+Hydrogen ion
🔥
5Cl2ODichlorine monoxide + 2N2Nitrogen + 2Ni2+Nickel(II) ion + 7H2OWater

General equation

Reaction of hardly oxidizable species and oxidizing species under acidic condition
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of hydrogen chloride and nickel(II) nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HClHydrogen chloride10
Reducing
Hardly oxidizable
Ni(NO3)2Nickel(II) nitrate2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion4
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cl2ODichlorine monoxide5
Oxidized
N2Nitrogen2
Reduced
Ni2+Nickel(II) ion2
H2OWater7
Water

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen chloride and nickel(II) nitrate under acidic condition
ΔrG587.7 kJ/mol
K0.11 × 10−102
pK102.96
10HClIonized aqueous solution + 2Ni(NO3)2Ionized aqueous solution + 4H+Un-ionized aqueous solution
🔥
5Cl2OGas + 2N2Gas + 2Ni2+Un-ionized aqueous solution + 7H2OLiquid
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
901.5587.71052.8
per 1 mol of
90.1558.77105.28
per 1 mol of
450.8293.9526.40
per 1 mol of
Hydrogen ion
225.4146.9263.20
180.3117.5210.56
per 1 mol of
450.8293.9526.40
per 1 mol of
Nickel(II) ion
450.8293.9526.40
per 1 mol of
128.883.96150.40

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
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[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]
H+ (g)1536.202[1]
H+ (ao)0[1]0[1]0[1]0[1]
* (g):Gas, (ai):Ionized aqueous solution, (cr):Crystalline solid, (ao):Un-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
Cl2O (g)80.3[1]97.9[1]266.21[1]45.40[1]
N2 (g)0[1]0[1]191.61[1]29.125[1]
Ni2+ (g)2931.390[1]
Ni2+ (ao)-54.0[1]-45.6[1]-128.9[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]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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)