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4NH4HSO4 + 3O2 → 2N2 + 4SO3 + 10H2O

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Reaction of ammonium hydrogensulfate and oxygen
4NH4HSO4Ammonium hydrogensulfate + 3O2Oxygen
⟶
2N2Nitrogen + 4SO3Sulfur trioxide + 10H2OWater

The reaction of ammonium hydrogensulfate and oxygen yields nitrogen, sulfur trioxide, 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 ammonium hydrogensulfate and oxygen
4NH4HSO4Ammonium hydrogensulfate + 3O2Oxygen
⟶
2N2Nitrogen + 4SO3Sulfur trioxide + 10H2OWater

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 hydrogensulfate and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4HSO4Ammonium hydrogensulfate4
Reducing
Reducing
O2Oxygen3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2Nitrogen2
Oxidized
–
SO3Sulfur trioxide4
–
–
H2OWater10
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium hydrogensulfate and oxygen
4NH4HSO4Crystalline solid + 3O2Gas
⟶
2N2Gas + 4SO3Liquid + 10H2OLiquid
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
−514.62–––
−128.66–––
per 1 mol of
−171.54–––
per 1 mol of
−257.31–––
per 1 mol of
−128.66–––
per 1 mol of
−51.462–––

Changes in aqueous solution

Reaction of ammonium hydrogensulfate and oxygen
◆
ΔrG−576.5 kJ/mol
K9.96 × 10100
pK−101.00
4NH4HSO4Ionized aqueous solution + 3O2Un-ionized aqueous solution
⟶
2N2Gas + 4SO3Crystalline solidβ + 10H2OLiquid
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
−561.8−576.551.6–
−140.4−144.112.9–
per 1 mol of
−187.3−192.217.2–
per 1 mol of
−280.9−288.325.8–
per 1 mol of
−140.4−144.112.9–
per 1 mol of
−56.18−57.655.16–

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
NH4HSO4 (cr)-1026.96[1]–––
NH4HSO4 (ai)-1019.85[1]-835.21[1]245.2[1]-3.8[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
N2 (g)0[1]0[1]191.61[1]29.125[1]
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]–
SO3 (l)-441.04[1]-373.75[1]113.8[1]–
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[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, (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)