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2HCl + 2HNO3 🔥→ Cl2 + N2O4 + 2H2O

The reaction of hydrogen chloride and nitric acid yields chlorine, dinitrogen tetraoxide, 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

General equation

Reaction of hardly oxidizable species and oxidizing species
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HClHydrogen chloride2
Reducing
Hardly oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cl2Chlorine1
Oxidized
N2O4Dinitrogen tetraoxide1
Reduced
H2OWater2

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen chloride and nitric acid
ΔrG−24.70 kJ/mol
K2.12 × 104
pK−4.33
2HClGas + 2HNO3Liquid
🔥
Cl2Gas + N2O4Liquid + 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
−58.35−24.70−112.949.2
per 1 mol of
−29.18−12.35−56.4524.6
per 1 mol of
−29.18−12.35−56.4524.6
per 1 mol of
−58.35−24.70−112.949.2
−58.35−24.70−112.949.2
per 1 mol of
−29.18−12.35−56.4524.6

Changes in aqueous solution (1)

Reaction of hydrogen chloride and nitric acid
ΔrG108.24 kJ/mol
K0.11 × 10−18
pK18.96
2HClIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
Cl2Gas + N2O4Liquid + 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
157.88108.24166.3773.2
per 1 mol of
78.94054.12083.15386.6
per 1 mol of
78.94054.12083.15386.6
per 1 mol of
157.88108.24166.3773.2
157.88108.24166.3773.2
per 1 mol of
78.94054.12083.15386.6

Changes in aqueous solution (2)

Reaction of hydrogen chloride and nitric acid
ΔrG115.18 kJ/mol
K0.66 × 10−20
pK20.18
2HClIonized aqueous solution + 2HNO3Ionized aqueous solution
🔥
Cl2Un-ionized aqueous solution + N2O4Liquid + 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
134.5115.1864
per 1 mol of
67.2557.59032
per 1 mol of
67.2557.59032
per 1 mol of
134.5115.1864
134.5115.1864
per 1 mol of
67.2557.59032

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]
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]
* (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]
N2O4 (l)-19.50[1]97.54[1]209.2[1]142.7[1]
N2O4 (g)9.16[1]97.89[1]304.29[1]77.28[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, (l):Liquid, (cr):Crystalline solid

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)