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3(NH4)2SO4 🔥→ HNO2 + 3SO2↑ + 4H2O + 5NH3

Decomposition of ammonium sulfate yields nitrous acid, sulfur dioxide, water, and ammonia (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

General equation

Thermal decomposition with redox
Thermally decomposable substanceSelf redox agent
🔥
ProductOxidation product + ProductReduction product
Thermal decomposition of oxoacid salt with redox
Oxoacid saltSelf redox agent
🔥
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Decomposition of ammonium sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO4Ammonium sulfate3
Self redox agent
Thermally decomposable
Oxoacid salt

Products

Chemical formulaNameCoefficientTypeType in general
equation
HNO2Nitrous acid1
Oxidized
SO2Sulfur dioxide3
Reduced
H2OWater4
NH3Ammonia5

Thermodynamic changes

Changes in standard condition (1)

Decomposition of ammonium sulfate
ΔrG727.5 kJ/mol
K0.35 × 10−127
pK127.45
3(NH4)2SO4Ionized aqueous solution
🔥
HNO2Un-ionized aqueous solution + 3SO2Gas + 4H2OLiquid + 5NH3Gas
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
1139.3727.51381.5
per 1 mol of
379.77242.5460.50
per 1 mol of
1139.3727.51381.5
per 1 mol of
379.77242.5460.50
per 1 mol of
284.82181.9345.38
per 1 mol of
227.86145.5276.30

Changes in standard condition (2)

Decomposition of ammonium sulfate
ΔrG677.2 kJ/mol
K0.23 × 10−118
pK118.64
3(NH4)2SO4Ionized aqueous solution
🔥
HNO2Un-ionized aqueous solution + 3SO2Gas + 4H2OLiquid + 5NH3Un-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
968.4677.2975.7
per 1 mol of
322.8225.7325.2
per 1 mol of
968.4677.2975.7
per 1 mol of
322.8225.7325.2
per 1 mol of
242.1169.3243.9
per 1 mol of
193.7135.4195.1

Changes in standard condition (3)

Decomposition of ammonium sulfate
ΔrG726.0 kJ/mol
K0.65 × 10−127
pK127.19
3(NH4)2SO4Ionized aqueous solution
🔥
HNO2Un-ionized aqueous solution + 3SO2Un-ionized aqueous solution + 4H2OLiquid + 5NH3Gas
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
1060.8726.01122.5
per 1 mol of
353.60242.0374.17
per 1 mol of
1060.8726.01122.5
per 1 mol of
353.60242.0374.17
per 1 mol of
265.20181.5280.63
per 1 mol of
212.16145.2224.50

Changes in standard condition (4)

Decomposition of ammonium sulfate
ΔrG675.8 kJ/mol
K0.40 × 10−118
pK118.40
3(NH4)2SO4Ionized aqueous solution
🔥
HNO2Un-ionized aqueous solution + 3SO2Un-ionized aqueous solution + 4H2OLiquid + 5NH3Un-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
889.9675.8716.7
per 1 mol of
296.6225.3238.9
per 1 mol of
889.9675.8716.7
per 1 mol of
296.6225.3238.9
per 1 mol of
222.5168.9179.2
per 1 mol of
178.0135.2143.3

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
(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

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]
SO2 (l)-320.5[1]
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[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]
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]
* (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid, (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)