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6NaCl + 2Al(NO3)3 + 12H+ 🔥→ 6Na+ + 3Cl2↑ + 6NO2↑ + 2Al3+ + 6H2O

Reaction of sodium chloride and aluminium nitrate under acidic condition
6NaClSodium chloride + 2Al(NO3)3Aluminium nitrate + 12H+Hydrogen ion
🔥
6Na+Sodium ion + 3Cl2Chlorine + 6NO2Nitrogen dioxide + 2Al3+Aluminium ion + 6H2OWater

The reaction of sodium chloride, aluminium nitrate, and hydrogen ion yields sodium ion, chlorine, nitrogen dioxide, aluminium 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 aluminium nitrate under acidic condition
6NaClSodium chloride + 2Al(NO3)3Aluminium nitrate + 12H+Hydrogen ion
🔥
6Na+Sodium ion + 3Cl2Chlorine + 6NO2Nitrogen dioxide + 2Al3+Aluminium 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 aluminium nitrate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaClSodium chloride6
Reducing
Hardly oxidizable
Al(NO3)3Aluminium nitrate2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion12
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na+Sodium ion6
Cl2Chlorine3
Oxidized
NO2Nitrogen dioxide6
Reduced
Al3+Aluminium ion2
H2OWater6
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium chloride and aluminium nitrate under acidic condition
ΔrG342 kJ/mol
K0.12 × 10−59
pK59.92
6NaClIonized aqueous solution + 2Al(NO3)3Ionized aqueous solution + 12H+Un-ionized aqueous solution
🔥
6Na+Un-ionized aqueous solution + 3Cl2Gas + 6NO2Gas + 2Al3+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
7353421311.4
per 1 mol of
12357.0218.57
per 1 mol of
368171655.70
per 1 mol of
Hydrogen ion
61.328.5109.28
per 1 mol of
Sodium ion
12357.0218.57
per 1 mol of
245114437.13
per 1 mol of
12357.0218.57
per 1 mol of
Aluminium ion
368171655.70
per 1 mol of
12357.0218.57

Changes in standard condition (2)

Reaction of sodium chloride and aluminium nitrate under acidic condition
ΔrG363 kJ/mol
K0.25 × 10−63
pK63.59
6NaClIonized aqueous solution + 2Al(NO3)3Ionized aqueous solution + 12H+Un-ionized aqueous solution
🔥
6Na+Un-ionized aqueous solution + 3Cl2Un-ionized aqueous solution + 6NO2Gas + 2Al3+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
6653631005
per 1 mol of
11160.5167.5
per 1 mol of
333182502.5
per 1 mol of
Hydrogen ion
55.430.383.75
per 1 mol of
Sodium ion
11160.5167.5
per 1 mol of
222121335.0
per 1 mol of
11160.5167.5
per 1 mol of
Aluminium ion
333182502.5
per 1 mol of
11160.5167.5

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]
Al(NO3)3 (ai)-1155[1]-820[1]117.6[1]
Al(NO3)3 (cr)
6 hydrate
-2850.48[1]-2203.39[1]467.8[1]433.0[1]
Al(NO3)3 (cr)
9 hydrate
-3757.06[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
Na+ (g)609.358[1]
Na+ (ao)-240.12[1]-261.905[1]59.0[1]46.4[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]
NO2 (g)33.18[1]51.31[1]240.06[1]37.20[1]
Al3+ (g)5483.17[1]
Al3+ (ao)-531[1]-485[1]-321.7[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)