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BaSO3 + 2HCl → BaCl2 + SO2 + H2O

The reaction of barium sulfite and hydrogen chloride yields barium chloride, sulfur dioxide, and water (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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
BaSO3Barium sulfite1
Brønsted base
Salt of weak acid
HClHydrogen chloride2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
BaCl2Barium chloride1
Conjugate base
Salt of strong acid
SO2Sulfur dioxide1
Acidic oxide
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of barium sulfite and hydrogen chloride
BaSO3Crystalline solid + 2HClGas
BaCl2Crystalline solid + SO2Gas + H2OLiquid
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
−77.1
per 1 mol of
−77.1
per 1 mol of
−38.5
per 1 mol of
−77.1
per 1 mol of
−77.1
per 1 mol of
−77.1

Changes in aqueous solution (1)

Reaction of barium sulfite and hydrogen chloride
BaSO3Crystalline solid + 2HClIonized aqueous solution
BaCl2Ionized aqueous solution + SO2Gas + H2OLiquid
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
59.2
per 1 mol of
59.2
per 1 mol of
29.6
per 1 mol of
59.2
per 1 mol of
59.2
per 1 mol of
59.2

Changes in aqueous solution (2)

Reaction of barium sulfite and hydrogen chloride
BaSO3Crystalline solid + 2HClIonized aqueous solution
BaCl2Ionized aqueous solution + SO2Un-ionized aqueous solution + H2OLiquid
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
33.1
per 1 mol of
33.1
per 1 mol of
16.6
per 1 mol of
33.1
per 1 mol of
33.1
per 1 mol of
33.1

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
BaSO3 (cr)-1179.5[1]
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
* (cr):Crystalline solid, (g):Gas, (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
BaCl2 (cr)-858.6[1]-810.4[1]123.68[1]75.14[1]
BaCl2 (g)-525.9[1]-537.6[1]325.29[1]56.19[1]
BaCl2 (ai)-871.95[1]-823.21[1]122.6[1]
BaCl2 (cr)
1 hydrate
-1160.6[1]-1055.63[1]166.9[1]
BaCl2 (cr)
2 hydrate
-1460.13[1]-1296.32[1]202.9[1]161.96[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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (ao):Un-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)