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2HCN + 3O2 → N2O3 + 2CO + H2O

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Reaction of hydrogen cyanide and oxygen
2HCNHydrogen cyanide + 3O2Oxygen
⟶
N2O3Dinitrogen trioxide + 2COCarbon monoxide + H2OWater

The reaction of hydrogen cyanide and oxygen yields dinitrogen trioxide, carbon monoxide, 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 cyanide and oxygen
2HCNHydrogen cyanide + 3O2Oxygen
⟶
N2O3Dinitrogen trioxide + 2COCarbon monoxide + H2OWater

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen cyanide and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HCNHydrogen cyanide2
Reducing
Reducing
O2Oxygen3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2O3Dinitrogen trioxide1
Redoxed product
–
COCarbon monoxide2
Reduced
–
H2OWater1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen cyanide and oxygen
◆
ΔrG−621.95 kJ/mol
K9.14 × 10108
pK−108.96
2HCNLiquid + 3O2Gas
⟶
N2O3Gas + 2COGas + H2OLiquid
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
−640.90−621.95−63.56−30.14
per 1 mol of
−320.45−310.98−31.78−15.07
per 1 mol of
−213.63−207.32−21.19−10.05
−640.90−621.95−63.56−30.14
per 1 mol of
−320.45−310.98−31.78−15.07
per 1 mol of
−640.90−621.95−63.56−30.14

Changes in aqueous solution (1)

Reaction of hydrogen cyanide and oxygen
◆
ΔrG−766.0 kJ/mol
K1.58 × 10134
pK−134.20
2HCNIonized aqueous solution + 3O2Un-ionized aqueous solution
⟶
N2O3Gas + 2COGas + H2OLiquid
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
−689.3−766.0256.6–
per 1 mol of
−344.6−383.0128.3–
per 1 mol of
−229.8−255.385.53–
−689.3−766.0256.6–
per 1 mol of
−344.6−383.0128.3–
per 1 mol of
−689.3−766.0256.6–

Changes in aqueous solution (2)

Reaction of hydrogen cyanide and oxygen
◆
ΔrG−731.5 kJ/mol
K1.42 × 10128
pK−128.15
2HCNIonized aqueous solution + 3O2Un-ionized aqueous solution
⟶
N2O3Gas + 2COUn-ionized aqueous solution + H2OLiquid
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
−710.1−731.570.5–
per 1 mol of
−355.1−365.835.3–
per 1 mol of
−236.7−243.823.5–
−710.1−731.570.5–
per 1 mol of
−355.1−365.835.3–
per 1 mol of
−710.1−731.570.5–

Changes in aqueous solution (3)

Reaction of hydrogen cyanide and oxygen
◆
ΔrG−660.6 kJ/mol
K5.40 × 10115
pK−115.73
2HCNUn-ionized aqueous solution + 3O2Un-ionized aqueous solution
⟶
N2O3Gas + 2COGas + H2OLiquid
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
−602.3−660.6195.4–
per 1 mol of
−301.1−330.397.70–
per 1 mol of
−200.8−220.265.13–
−602.3−660.6195.4–
per 1 mol of
−301.1−330.397.70–
per 1 mol of
−602.3−660.6195.4–

Changes in aqueous solution (4)

Reaction of hydrogen cyanide and oxygen
◆
ΔrG−626.1 kJ/mol
K4.87 × 10109
pK−109.69
2HCNUn-ionized aqueous solution + 3O2Un-ionized aqueous solution
⟶
N2O3Gas + 2COUn-ionized aqueous solution + H2OLiquid
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
−623.1−626.19.3–
per 1 mol of
−311.6−313.14.7–
per 1 mol of
−207.7−208.73.1–
−623.1−626.19.3–
per 1 mol of
−311.6−313.14.7–
per 1 mol of
−623.1−626.19.3–

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]–
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[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
N2O3 (l)50.29[1]–––
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[1]
CO (g)-110.525[1]-137.168[1]197.674[1]29.142[1]
CO (ao)-120.96[1]-119.90[1]104.6[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]
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (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)