Mg(OH)2 + 2B2O3 → MgB4O7 + H2O
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The reaction of magnesium hydroxide and diboron trioxide yields magnesium tetraborate and water. This reaction is an acid-base reaction and is classified as follows:
- Reaction of base and acidic oxide
- Reaction of hydroxide base and acidic oxide
- Reaction of strong hydroxide base and weakly acidic oxide
Table of contents
Reaction data
Chemical equation
- Reaction of magnesium hydroxide and diboron trioxide
General equation
- Reaction of base and acidic oxide
- BaseLewis base + Acidic oxideLewis acid + H2O ⟶ Oxoacid saltLewis conjugate + (H2O)
- Reaction of hydroxide base and acidic oxide
- Hydroxide baseLewis base + Acidic oxideLewis acid ⟶ Oxoacid saltLewis conjugate + H2O
- Reaction of strong hydroxide base and weakly acidic oxide
- Strong hydroxide baseLewis base + Weakly acidic oxideLewis acid ⟶ Salt of weak acid and strong baseLewis conjugate + H2O
Oxidation state of each atom
- Reaction of magnesium hydroxide and diboron trioxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mg(OH)2 | Magnesium hydroxide | 1 | Lewis base | Base Hydroxide base Strong hydroxide base |
| B2O3 | Diboron trioxide | 2 | Lewis acid | Acidic oxide Weakly acidic oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgB4O7 | Magnesium tetraborate | 1 | Lewis conjugate | Oxoacid salt Salt of weak acid and strong base |
| H2O | Water | 1 | – | Water |
Thermodynamic changes
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 |
|---|---|---|---|---|
| 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] | – |
| B2O3 (cr) | -1272.77[1] | -1193.65[1] | 53.97[1] | 62.93[1] |
| B2O3 (am) | -1254.53[1] | -1182.3[1] | 77.8[1] | 61.1[1] |
| B2O3 (g) | -843.79[1] | -831.97[1] | 279.81[1] | 66.86[1] |
* (cr):Crystalline solid, (am):Amorphous 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 |
|---|---|---|---|---|
| MgB4O7 | – | – | – | – |
| 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°, -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°, -1272.77 kJ · mol−1
- ^ ΔfG°, -1193.65 kJ · mol−1
- ^ S°, 53.97 J · K−1 · mol−1
- ^ Cp°, 62.93 J · K−1 · mol−1
- ^ ΔfH°, -1254.53 kJ · mol−1
- ^ ΔfG°, -1182.3 kJ · mol−1
- ^ S°, 77.8 J · K−1 · mol−1
- ^ Cp°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -843.79 kJ · mol−1
- ^ ΔfG°, -831.97 kJ · mol−1
- ^ S°, 279.81 J · K−1 · mol−1
- ^ Cp°, 66.86 J · K−1 · 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