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(NH4)2S + 3O2 → 2HNO2 + 2H2O + H2S

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Reaction of ammonium sulfide and oxygen
(NH4)2SAmmonium sulfide + 3O2Oxygen
⟶
2HNO2Nitrous acid + 2H2OWater + H2SHydrogen sulfide

The reaction of ammonium sulfide and oxygen yields nitrous acid, water, 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 sulfide and oxygen
(NH4)2SAmmonium sulfide + 3O2Oxygen
⟶
2HNO2Nitrous acid + 2H2OWater + 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 sulfide and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SAmmonium sulfide1
Reducing
Reducing
O2Oxygen3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
HNO2Nitrous acid2
Redoxed product
–
H2OWater2
Reduced
–
H2SHydrogen sulfide1
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium sulfide and oxygen
◆
ΔrG−585.6 kJ/mol
K3.91 × 10102
pK−102.59
(NH4)2SIonized aqueous solution + 3O2Un-ionized aqueous solution
⟶
2HNO2Un-ionized aqueous solution + 2H2OLiquid + 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
−563.8−585.672.0–
per 1 mol of
−563.8−585.672.0–
per 1 mol of
−187.9−195.224.0–
per 1 mol of
−281.9−292.836.0–
per 1 mol of
−281.9−292.836.0–
per 1 mol of
−563.8−585.672.0–

Changes in aqueous solution (2)

Reaction of ammonium sulfide and oxygen
◆
ΔrG−579.9 kJ/mol
K3.93 × 10101
pK−101.59
(NH4)2SIonized aqueous solution + 3O2Un-ionized aqueous solution
⟶
2HNO2Un-ionized aqueous solution + 2H2OLiquid + 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
−582.9−579.9−13–
per 1 mol of
−582.9−579.9−13–
per 1 mol of
−194.3−193.3−4.3–
per 1 mol of
−291.4−289.9−6.5–
per 1 mol of
−291.4−289.9−6.5–
per 1 mol of
−582.9−579.9−13–

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
(NH4)2S (ai)-231.8[1]-72.6[1]212.1[1]–
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (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
HNO2 (g)
cis
-77.99[1]-42.94[1]248.76[1]44.77[1]
HNO2 (g)
trans
-80.12[1]-45.24[1]249.22[1]46.07[1]
HNO2 (g)-79.5[1]-46.0[1]254.1[1]45.6[1]
HNO2 (ao)-119.2[1]-50.6[1]135.6[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]
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[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)