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10NaCl + 11Ni(NO3)2 + 22H+ 🔥→ 10NaNO3 + 10HClO3 + 6N2↑ + 11Ni2+ + 6H2O

Reaction of sodium chloride and nickel(II) nitrate under acidic condition
10NaClSodium chloride + 11Ni(NO3)2Nickel(II) nitrate + 22H+Hydrogen ion
🔥
10NaNO3Sodium nitrate + 10HClO3Chloric acid + 6N2Nitrogen + 11Ni2+Nickel(II) ion + 6H2OWater

The reaction of sodium chloride, nickel(II) nitrate, and hydrogen ion yields sodium nitrate, chloric acid, 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 sodium chloride and nickel(II) nitrate under acidic condition
10NaClSodium chloride + 11Ni(NO3)2Nickel(II) nitrate + 22H+Hydrogen ion
🔥
10NaNO3Sodium nitrate + 10HClO3Chloric acid + 6N2Nitrogen + 11Ni2+Nickel(II) ion + 6H2OWater

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 sodium chloride and nickel(II) nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride10
Reducing
Hardly oxidizable
Ni(NO3)2Nickel(II) nitrate11
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion22
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaNO3Sodium nitrate10
HClO3Chloric acid10
Oxidized
N2Nitrogen6
Reduced
Ni2+Nickel(II) ion11
H2OWater6
Water

Thermodynamic changes

Changes in standard condition

Reaction of sodium chloride and nickel(II) nitrate under acidic condition
ΔrG1149.5 kJ/mol
K0.41 × 10−201
pK201.38
10NaClIonized aqueous solution + 11Ni(NO3)2Ionized aqueous solution + 22H+Un-ionized aqueous solution
🔥
10NaNO3Ionized aqueous solution + 10HClO3Ionized aqueous solution + 6N2Gas + 11Ni2+Un-ionized aqueous solution + 6H2OLiquid
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
1403.81149.5869.2
per 1 mol of
140.38114.9586.92
per 1 mol of
127.62104.5079.02
per 1 mol of
Hydrogen ion
63.80952.25039.51
per 1 mol of
140.38114.9586.92
per 1 mol of
140.38114.9586.92
per 1 mol of
233.97191.58144.9
per 1 mol of
Nickel(II) ion
127.62104.5079.02
per 1 mol of
233.97191.58144.9

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
NaCl (cr)-411.153[1]-384.138[1]72.13[1]50.50[1]
NaCl (g)-176.65[1]-196.66[1]229.81[1]35.77[1]
NaCl (ai)-407.27[1]-393.133[1]115.5[1]-90.0[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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
NaNO3 (cr)-467.85[1]-367.00[1]116.52[1]92.88[1]
NaNO3 (ai)-447.48[1]-373.15[1]205.4[1]-40.2[1]
HClO3 (ai)-103.97[1]-7.95[1]162.3[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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (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)