MgBr2 + Li2SO3 💧→ MgSO3↓ + 2LiBr
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The reaction of magnesium bromide and lithium sulfite yields magnesium sulfite and lithium bromide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of magnesium bromide and lithium 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 magnesium bromide and lithium sulfite
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgBr2 | Magnesium bromide | 1 | Lewis acid | Very soluble in water |
Li2SO3 | Lithium sulfite | 1 | Lewis base | Soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgSO3 | Magnesium sulfite | 1 | Lewis conjugate | Slightly soluble in water |
LiBr | Lithium bromide | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of magnesium bromide and lithium 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 | −9.4 | – | – | – |
per 1 mol of | −9.4 | – | – | – |
per 1 mol of | −9.4 | – | – | – |
per 1 mol of | −9.4 | – | – | – |
per 1 mol of | −4.7 | – | – | – |
Changes in aqueous solution
- Reaction of magnesium bromide and lithium 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 | 78.6 | – | – | – |
per 1 mol of | 78.6 | – | – | – |
per 1 mol of | 78.6 | – | – | – |
per 1 mol of | 78.6 | – | – | – |
per 1 mol of | 39.3 | – | – | – |
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 |
---|---|---|---|---|
MgBr2 (cr) | -524.3[1] | -503.8[1] | 117.2[1] | – |
MgBr2 (g) | -309.6[1] | – | – | – |
MgBr2 (ai) | -709.94[1] | -662.7[1] | 26.8[1] | – |
MgBr2 (cr) 6 hydrate | -2410.0[1] | -2055.7[1] | 397[1] | – |
Li2SO3 (cr) | -1177.0[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (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 |
---|---|---|---|---|
MgSO3 (cr) | -1008.3[1] | -923.8[1] | 87.9[1] | – |
MgSO3 (cr) 3 hydrate | -1931.8[1] | -1674.7[1] | 209.2[1] | – |
MgSO3 (cr) 6 hydrate | -2817.5[1] | -2385.4[1] | 322.2[1] | – |
LiBr (cr) | -351.213[1] | -342.00[1] | 74.27[1] | – |
LiBr (g) | – | – | 224.33[1] | 33.93[1] |
LiBr (ai) | -400.041[1] | -397.27[1] | 95.8[1] | -73.2[1] |
LiBr (cr) 1 hydrate | -662.58[1] | -594.29[1] | 109.6[1] | – |
LiBr (cr) 2 hydrate | -962.7[1] | -840.5[1] | 162.3[1] | – |
* (cr):Crystalline solid, (g):Gas, (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°, -524.3 kJ · mol−1
- ^ ΔfG°, -503.8 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -309.6 kJ · mol−1
- ^ ΔfH°, -709.94 kJ · mol−1
- ^ ΔfG°, -662.7 kJ · mol−1
- ^ S°, 26.8 J · K−1 · mol−1
- ^ ΔfH°, -2410.0 kJ · mol−1
- ^ ΔfG°, -2055.7 kJ · mol−1
- ^ S°, 397. J · K−1 · mol−1
- ^ ΔfH°, -1177.0 kJ · mol−1
- ^ ΔfH°, -1008.3 kJ · mol−1
- ^ ΔfG°, -923.8 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -1931.8 kJ · mol−1
- ^ ΔfG°, -1674.7 kJ · mol−1
- ^ S°, 209.2 J · K−1 · mol−1
- ^ ΔfH°, -2817.5 kJ · mol−1
- ^ ΔfG°, -2385.4 kJ · mol−1
- ^ S°, 322.2 J · K−1 · mol−1
- ^ ΔfH°, -351.213 kJ · mol−1
- ^ ΔfG°, -342.00 kJ · mol−1
- ^ S°, 74.27 J · K−1 · mol−1
- ^ S°, 224.33 J · K−1 · mol−1
- ^ Cp°, 33.93 J · K−1 · mol−1
- ^ ΔfH°, -400.041 kJ · mol−1
- ^ ΔfG°, -397.27 kJ · mol−1
- ^ S°, 95.8 J · K−1 · mol−1
- ^ Cp°, -73.2 J · K−1 · mol−1
- ^ ΔfH°, -662.58 kJ · mol−1
- ^ ΔfG°, -594.29 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ ΔfH°, -962.7 kJ · mol−1
- ^ ΔfG°, -840.5 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1