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2HCN + 6HNO3 → NH4NO3 + 3N2O3↑ + 2H2CO3

The reaction of hydrogen cyanide and nitric acid yields ammonium nitrate, dinitrogen trioxide, and carbonic acid (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 reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HCNHydrogen cyanide2
Reducing
Reducing
HNO3Nitric acid6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH4NO3Ammonium nitrate1
N2O3Dinitrogen trioxide3
Redoxed product
H2CO3Carbonic acid2
Oxidized

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen cyanide and nitric acid
ΔrG−695.6 kJ/mol
K7.31 × 10121
pK−121.86
2HCNIonized aqueous solution + 6HNO3Ionized aqueous solution
NH4NO3Ionized aqueous solution + 3N2O3Gas + 2H2CO3Un-ionized aqueous solution
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
−545.1−695.6504.8
per 1 mol of
−272.6−347.8252.4
per 1 mol of
−90.85−115.984.13
per 1 mol of
−545.1−695.6504.8
−181.7−231.9168.3
per 1 mol of
−272.6−347.8252.4

Changes in standard condition (2)

Reaction of hydrogen cyanide and nitric acid
ΔrG−590.2 kJ/mol
K2.50 × 10103
pK−103.40
2HCNUn-ionized aqueous solution + 6HNO3Ionized aqueous solution
NH4NO3Ionized aqueous solution + 3N2O3Gas + 2H2CO3Un-ionized aqueous solution
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
−458.1−590.2443.6
per 1 mol of
−229.1−295.1221.8
per 1 mol of
−76.35−98.3773.93
per 1 mol of
−458.1−590.2443.6
−152.7−196.7147.9
per 1 mol of
−229.1−295.1221.8

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
HCN (l)108.87[1]124.97[1]112.84[1]70.63[1]
HCN (g)135.1[1]124.7[1]201.78[1]35.86[1]
HCN (ai)150.6[1]172.4[1]94.1[1]
HCN (ao)107.1[1]119.7[1]124.7[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]
* (l):Liquid, (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
NH4NO3 (cr)-365.56[1]-183.87[1]151.08[1]139.3[1]
NH4NO3 (ai)-339.87[1]-190.56[1]259.8[1]-6.7[1]
N2O3 (l)50.29[1]
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[1]
H2CO3 (ao)-699.65[1]-623.08[1]187.4[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution

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)