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Na2SO3 🔥→ Na2O + SO2

Decomposition of sodium sulfite yields sodium oxide and sulfur dioxide (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

General equation

Thermal decomposition without redox
Thermally decomposable substanceLewis conjugate
🔥
ProductLewis acid + ProductLewis base

Oxidation state of each atom

Decomposition of sodium sulfite

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO3Sodium sulfite1
Lewis conjugate
Thermally decomposable
Oxoacid salt
Salt of oxoacid and hydroxide base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide1
Lewis acid
Lewis base
Basic oxide
SO2Sulfur dioxide1
Lewis acid
Acidic oxide

Thermodynamic changes

Changes in standard condition

Decomposition of sodium sulfite
ΔrG336.8 kJ/mol
K0.99 × 10−59
pK59.00
Na2SO3Crystalline solid
🔥
Na2OCrystalline solid + SO2Gas
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
389.8336.8177.34−11.26
per 1 mol of
389.8336.8177.34−11.26
per 1 mol of
389.8336.8177.34−11.26
per 1 mol of
389.8336.8177.34−11.26

Changes in aqueous solution (1)

Decomposition of sodium sulfite
ΔrG334.74 kJ/mol
K0.23 × 10−58
pK58.64
Na2SO3Ionized aqueous solution
🔥
Na2OCrystalline solid + SO2Gas
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
404.82334.74235.4
per 1 mol of
404.82334.74235.4
per 1 mol of
404.82334.74235.4
per 1 mol of
404.82334.74235.4

Changes in aqueous solution (2)

Decomposition of sodium sulfite
ΔrG334.25 kJ/mol
K0.28 × 10−58
pK58.56
Na2SO3Ionized aqueous solution
🔥
Na2OCrystalline solid + SO2Un-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
378.67334.25149.1
per 1 mol of
378.67334.25149.1
per 1 mol of
378.67334.25149.1
per 1 mol of
378.67334.25149.1

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
Na2SO3 (cr)-1100.8[1]-1012.5[1]145.94[1]120.25[1]
Na2SO3 (ai)-1115.87[1]-1010.39[1]87.9[1]
Na2SO3 (cr)
7 hydrate
-3162.3[1]-2676.1[1]444[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
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[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]
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ao):Un-ionized aqueous solution

References

List of references

  1. 1