SnS + Mg(OH)2 🔥→ MgS + Sn(OH)2
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The reaction of tin(II) sulfide and magnesium hydroxide yields magnesium sulfide and tin(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of tin(II) sulfide and magnesium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of tin(II) sulfide and magnesium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SnS | Tin(II) sulfide | 1 | Brønsted acid | Salt of weak base |
| Mg(OH)2 | Magnesium hydroxide | 1 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgS | Magnesium sulfide | 1 | Conjugate acid | Salt of strong base |
| Sn(OH)2 | Tin(II) hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of tin(II) sulfide and magnesium hydroxide◆
ΔrG 98.4 kJ/mol K 0.58 × 10−17 pK 17.24
| 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 | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
Changes in standard condition (2)
- Reaction of tin(II) sulfide and magnesium hydroxide
| 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 | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
Changes in aqueous solution (1)
- Reaction of tin(II) sulfide and magnesium hydroxide◆
ΔrG 98.4 kJ/mol K 0.58 × 10−17 pK 17.24
| 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 | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
per 1 mol of | 117 | 98.4 | 65 | – |
Changes in aqueous solution (2)
- Reaction of tin(II) sulfide and magnesium hydroxide
| 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 | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
per 1 mol of | 113 | – | – | – |
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 |
|---|---|---|---|---|
| SnS (cr) | -100[1] | -98.3[1] | 77.0[1] | 49.25[1] |
| SnS (g) | 119.2[1] | – | – | – |
| Mg(OH)2 (cr) | -924.54[1] | -833.51[1] | 63.18[1] | 77.03[1] |
| Mg(OH)2 (am) precipitated | -920.5[1] | – | – | – |
| Mg(OH)2 (g) | -561[1] | – | – | – |
| Mg(OH)2 (ai) | -926.84[1] | -769.4[1] | -159.4[1] | – |
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid, (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 |
|---|---|---|---|---|
| MgS (cr) | -346.0[1] | -341.8[1] | 50.33[1] | 45.56[1] |
| Sn(OH)2 (cr) precipitated | -561.1[1] | -491.6[1] | 155[1] | – |
* (cr):Crystalline solid
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°, -100. kJ · mol−1
- ^ ΔfG°, -98.3 kJ · mol−1
- ^ S°, 77.0 J · K−1 · mol−1
- ^ Cp°, 49.25 J · K−1 · mol−1
- ^ ΔfH°, 119.2 kJ · mol−1
- ^ ΔfH°, -924.54 kJ · mol−1
- ^ ΔfG°, -833.51 kJ · mol−1
- ^ S°, 63.18 J · K−1 · mol−1
- ^ Cp°, 77.03 J · K−1 · mol−1
- ^ ΔfH°, -920.5 kJ · mol−1
- ^ ΔfH°, -561. kJ · mol−1
- ^ ΔfH°, -926.84 kJ · mol−1
- ^ ΔfG°, -769.4 kJ · mol−1
- ^ S°, -159.4 J · K−1 · mol−1
- ^ ΔfH°, -346.0 kJ · mol−1
- ^ ΔfG°, -341.8 kJ · mol−1
- ^ S°, 50.33 J · K−1 · mol−1
- ^ Cp°, 45.56 J · K−1 · mol−1
- ^ ΔfH°, -561.1 kJ · mol−1
- ^ ΔfG°, -491.6 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1