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2NH3 + SO3 + H2O → (NH4)2SO4

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Reaction of ammonia, sulfur trioxide, and water
2NH3Ammonia + SO3Sulfur trioxide + H2OWater
⟶
(NH4)2SO4Ammonium sulfate

The reaction of ammonia, sulfur trioxide, and water yields ammonium sulfate (Other reactions are here). This reaction is an acid-base 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 ammonia, sulfur trioxide, and water
2NH3Ammonia + SO3Sulfur trioxide + H2OWater
⟶
(NH4)2SO4Ammonium sulfate

General equation

Reaction of base and acidic oxide
BaseLewis base + Acidic oxideLewis acid + H2O
⟶
Oxoacid saltLewis conjugate + (H2O)
Reaction of non hydroxide base and acidic oxide with generating oxoacid salt
Non hydroxide baseBrønsted base + Acidic oxideLewis acid + H2O
⟶
Oxoacid salt

Oxidation state of each atom

Reaction of ammonia, sulfur trioxide, and water

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH3Ammonia2
Lewis base
Brønsted base
Base
Non hydroxide base
SO3Sulfur trioxide1
Lewis acid
Acidic oxide
H2OWater1
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO4Ammonium sulfate1
Lewis conjugate
–
Oxoacid salt

Thermodynamic changes

Changes in standard condition

Reaction of ammonia, sulfur trioxide, and water
◆
ΔrG−257.89 kJ/mol
K1.51 × 1045
pK−45.18
2NH3Gas + SO3Liquid + H2OLiquid
⟶
(NH4)2SO4Crystalline solid
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
−361.76−257.89−348.5–
per 1 mol of
−180.88−128.94−174.3–
per 1 mol of
−361.76−257.89−348.5–
per 1 mol of
−361.76−257.89−348.5–
per 1 mol of
−361.76−257.89−348.5–

Changes in aqueous solution

Reaction of ammonia, sulfur trioxide, and water
◆
ΔrG−238.80 kJ/mol
K6.85 × 1041
pK−41.84
2NH3Un-ionized aqueous solution + SO3Crystalline solidβ + H2OLiquid
⟶
(NH4)2SO4Ionized 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
−273.36−238.80−116.3–
per 1 mol of
−136.68−119.40−58.15–
per 1 mol of
−273.36−238.80−116.3–
per 1 mol of
−273.36−238.80−116.3–
per 1 mol of
−273.36−238.80−116.3–

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
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[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, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

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
(NH4)2SO4 (cr)-1180.85[1]-901.67[1]220.1[1]187.49[1]
(NH4)2SO4 (ai)-1174.28[1]-903.14[1]246.9[1]-133.1[1]
* (cr):Crystalline solid, (ai):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)