BaO + H2SO3 → BaSO3↓ + H2O
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- Reaction of barium oxide and sulfurous acid
The reaction of barium oxide and sulfurous acid yields barium sulfite and water. This reaction is an acid-base reaction and is classified as follows:
- Reaction of basic oxide and acid
- Reaction of strongly basic oxide and weak acid
- Precipitation reaction
Table of contents
Reaction data
Chemical equation
- Reaction of barium oxide and sulfurous acid
General equation
- Reaction of basic oxide and acid
- Basic oxideBrønsted base + AcidBrønsted acid ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of strongly basic oxide and weak acid
- Strongly basic oxideBrønsted base + Weak acidBrønsted acid ⟶ Salt of weak acid and strong baseConjugate base + H2OConjugate acid
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of barium oxide and sulfurous acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaO | Barium oxide | 1 | Brønsted base Lewis acid | Basic oxide Strongly basic oxide Soluble in water |
| H2SO3 | Sulfurous acid | 1 | Brønsted acid Lewis base | Acid Weak acid Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaSO3 | Barium sulfite | 1 | Conjugate base Lewis conjugate | Salt Salt of weak acid and strong base Very slightly soluble in water |
| H2O | Water | 1 | Conjugate acid Non-redox product | Water – |
Thermodynamic changes
Changes in standard condition
- Reaction of barium oxide and sulfurous acid
| 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 | −303.0 | – | – | – |
per 1 mol of | −303.0 | – | – | – |
per 1 mol of | −303.0 | – | – | – |
per 1 mol of | −303.0 | – | – | – |
per 1 mol of | −303.0 | – | – | – |
Thermodynamic data of reactants
| Chemical formula | Standard 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 |
|---|---|---|---|---|
| BaO (cr) | -553.5[1] | -525.1[1] | 70.42[1] | 47.78[1] |
| BaO (g) | -117[1] | – | – | 33.1[1] |
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution
Thermodynamic data of products
| Chemical formula | Standard 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] | – | – | – |
| 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, (l):Liquid, (g):Gas
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -553.5 kJ · mol−1
- ^ ΔfG°, -525.1 kJ · mol−1
- ^ S°, 70.42 J · K−1 · mol−1
- ^ Cp°, 47.78 J · K−1 · mol−1
- ^ ΔfH°, -117. kJ · mol−1
- ^ Cp°, 33.1 J · K−1 · mol−1
- ^ ΔfH°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1
- ^ ΔfH°, -1179.5 kJ · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1