SrBr2 + Li2S 💧→ SrS↓ + 2LiBr
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The reaction of strontium bromide and lithium sulfide yields strontium sulfide and lithium bromide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of strontium bromide and lithium sulfide
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 strontium bromide and lithium sulfide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SrBr2 | Strontium bromide | 1 | Lewis acid | Very soluble in water |
Li2S | Lithium sulfide | 1 | Lewis base | Very soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SrS | Strontium sulfide | 1 | Lewis conjugate | Slightly soluble in water |
LiBr | Lithium bromide | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of strontium bromide and lithium sulfide
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 | −15.8 | – | – | – |
per 1 mol of | −15.8 | – | – | – |
per 1 mol of | −15.8 | – | – | – |
per 1 mol of | −15.8 | – | – | – |
per 1 mol of | −7.90 | – | – | – |
Changes in aqueous solution
- Reaction of strontium bromide and lithium sulfide
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 | −42.2 | – | – | – |
per 1 mol of | −42.2 | – | – | – |
per 1 mol of | −42.2 | – | – | – |
per 1 mol of | −42.2 | – | – | – |
per 1 mol of | −21.1 | – | – | – |
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 |
---|---|---|---|---|
SrBr2 (cr) | -717.6[1] | -697.1[1] | 135.10[1] | 75.35[1] |
SrBr2 (g) | -410[1] | -444[1] | 323.5[1] | 60.7[1] |
SrBr2 (ai) | -788.89[1] | -767.39[1] | 132.2[1] | – |
SrBr2 (cr) 1 hydrate | -1031.4[1] | -954.3[1] | 180[1] | 120.9[1] |
SrBr2 (cr) 6 hydrate | -2531.3[1] | -2174.1[1] | 406[1] | 343.5[1] |
Li2S (cr) | -441.4[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 |
---|---|---|---|---|
SrS (cr) | -472.4[1] | -467.8[1] | 68.2[1] | 48.70[1] |
SrS (g) | 109[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°, -717.6 kJ · mol−1
- ^ ΔfG°, -697.1 kJ · mol−1
- ^ S°, 135.10 J · K−1 · mol−1
- ^ Cp°, 75.35 J · K−1 · mol−1
- ^ ΔfH°, -410. kJ · mol−1
- ^ ΔfG°, -444. kJ · mol−1
- ^ S°, 323.5 J · K−1 · mol−1
- ^ Cp°, 60.7 J · K−1 · mol−1
- ^ ΔfH°, -788.89 kJ · mol−1
- ^ ΔfG°, -767.39 kJ · mol−1
- ^ S°, 132.2 J · K−1 · mol−1
- ^ ΔfH°, -1031.4 kJ · mol−1
- ^ ΔfG°, -954.3 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ Cp°, 120.9 J · K−1 · mol−1
- ^ ΔfH°, -2531.3 kJ · mol−1
- ^ ΔfG°, -2174.1 kJ · mol−1
- ^ S°, 406. J · K−1 · mol−1
- ^ Cp°, 343.5 J · K−1 · mol−1
- ^ ΔfH°, -441.4 kJ · mol−1
- ^ ΔfH°, -472.4 kJ · mol−1
- ^ ΔfG°, -467.8 kJ · mol−1
- ^ S°, 68.2 J · K−1 · mol−1
- ^ Cp°, 48.70 J · K−1 · mol−1
- ^ ΔfH°, 109. kJ · 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