BaS + K2SO3 💧→ BaSO3↓ + K2S
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The reaction of barium sulfide and potassium sulfite yields barium sulfite and potassium sulfide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of barium sulfide and potassium sulfite
General equation
- 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 sulfide and potassium sulfite
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BaS | Barium sulfide | 1 | Lewis acid | Soluble in water |
K2SO3 | Potassium sulfite | 1 | Lewis base | Very soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BaSO3 | Barium sulfite | 1 | Lewis conjugate | Very slightly soluble in water |
K2S | Potassium sulfide | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of barium sulfide and potassium sulfite
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 | 25 | – | – | – |
per 1 mol of | 25 | – | – | – |
per 1 mol of | 25 | – | – | – |
per 1 mol of | 25 | – | – | – |
per 1 mol of | 25 | – | – | – |
Changes in aqueous solution
- Reaction of barium sulfide and potassium sulfite
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 | −17.6 | – | – | – |
per 1 mol of | −17.6 | – | – | – |
per 1 mol of | −17.6 | – | – | – |
per 1 mol of | −17.6 | – | – | – |
per 1 mol of | −17.6 | – | – | – |
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 |
---|---|---|---|---|
BaS (cr) | -460[1] | -456[1] | 78.2[1] | 49.37[1] |
BaS (g) | 50[1] | – | – | – |
BaS (aq) | -493.3[1] | – | – | – |
K2SO3 (cr) | -1125.5[1] | – | – | – |
K2SO3 (ai) | -1140.1[1] | -1053.1[1] | 176[1] | – |
* (cr):Crystalline solid, (g):Gas, (aq):Aqueous solution, (ai):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] | – | – | – |
K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution
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°, -460. kJ · mol−1
- ^ ΔfG°, -456. kJ · mol−1
- ^ S°, 78.2 J · K−1 · mol−1
- ^ Cp°, 49.37 J · K−1 · mol−1
- ^ ΔfH°, 50. kJ · mol−1
- ^ ΔfH°, -493.3 kJ · mol−1
- ^ ΔfH°, -1125.5 kJ · mol−1
- ^ ΔfH°, -1140.1 kJ · mol−1
- ^ ΔfG°, -1053.1 kJ · mol−1
- ^ S°, 176. J · K−1 · mol−1
- ^ ΔfH°, -1179.5 kJ · mol−1
- ^ ΔfH°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1