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NH4SCN + 4O2 → 2HNO3 + CO2 + H2S

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Reaction of ammonium thiocyanate and oxygen
NH4SCNAmmonium thiocyanate + 4O2Oxygen
⟶
2HNO3Nitric acid + CO2Carbon dioxide + H2SHydrogen sulfide

The reaction of ammonium thiocyanate and oxygen yields nitric acid, carbon dioxide, and hydrogen sulfide (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 ammonium thiocyanate and oxygen
NH4SCNAmmonium thiocyanate + 4O2Oxygen
⟶
2HNO3Nitric acid + CO2Carbon dioxide + H2SHydrogen sulfide

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 ammonium thiocyanate and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4SCNAmmonium thiocyanate1
Reducing
Reducing
O2Oxygen4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
HNO3Nitric acid2
Redoxed product
–
CO2Carbon dioxide1
Reduced
–
H2SHydrogen sulfide1
–
–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium thiocyanate and oxygen
NH4SCNCrystalline solid + 4O2Gas
⟶
2HNO3Liquid + CO2Gas + H2SGas
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
−683.6–––
−683.6–––
per 1 mol of
−170.9–––
per 1 mol of
−341.8–––
per 1 mol of
−683.6–––
per 1 mol of
−683.6–––

Changes in aqueous solution (1)

Reaction of ammonium thiocyanate and oxygen
◆
ΔrG−729.4 kJ/mol
K6.10 × 10127
pK−127.79
NH4SCNIonized aqueous solution + 4O2Un-ionized aqueous solution
⟶
2HNO3Ionized aqueous solution + CO2Gas + H2SGas
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
−726.0−729.411.0–
−726.0−729.411.0–
per 1 mol of
−181.5−182.32.75–
per 1 mol of
−363.0−364.75.50–
per 1 mol of
−726.0−729.411.0–
per 1 mol of
−726.0−729.411.0–

Changes in aqueous solution (2)

Reaction of ammonium thiocyanate and oxygen
◆
ΔrG−723.7 kJ/mol
K6.12 × 10126
pK−126.79
NH4SCNIonized aqueous solution + 4O2Un-ionized aqueous solution
⟶
2HNO3Ionized aqueous solution + CO2Gas + H2SUn-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
−745.1−723.7−74–
−745.1−723.7−74–
per 1 mol of
−186.3−180.9−19–
per 1 mol of
−372.6−361.9−37–
per 1 mol of
−745.1−723.7−74–
per 1 mol of
−745.1−723.7−74–

Changes in aqueous solution (3)

Reaction of ammonium thiocyanate and oxygen
◆
ΔrG−721.0 kJ/mol
K2.06 × 10126
pK−126.31
NH4SCNIonized aqueous solution + 4O2Un-ionized aqueous solution
⟶
2HNO3Ionized aqueous solution + CO2Un-ionized aqueous solution + H2SGas
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
−746.3−721.0−85.1–
−746.3−721.0−85.1–
per 1 mol of
−186.6−180.3−21.3–
per 1 mol of
−373.1−360.5−42.5–
per 1 mol of
−746.3−721.0−85.1–
per 1 mol of
−746.3−721.0−85.1–

Changes in aqueous solution (4)

Reaction of ammonium thiocyanate and oxygen
◆
ΔrG−715.3 kJ/mol
K2.07 × 10125
pK−125.32
NH4SCNIonized aqueous solution + 4O2Un-ionized aqueous solution
⟶
2HNO3Ionized aqueous solution + CO2Un-ionized aqueous solution + H2SUn-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
−765.4−715.3−170–
−765.4−715.3−170–
per 1 mol of
−191.3−178.8−42.5–
per 1 mol of
−382.7−357.6−85.0–
per 1 mol of
−765.4−715.3−170–
per 1 mol of
−765.4−715.3−170–

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
NH4SCN (cr)-78.7[1]–––
NH4SCN (ai)-56.07[1]13.40[1]257.7[1]39.7[1]
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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
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]
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[1]–
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]–
* (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (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)