2Be + Mg(OH)2 → 2BeO + Mg + H2↑
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- Reaction of and magnesium hydroxide
The reaction of and magnesium hydroxide yields beryllium oxide, , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and magnesium hydroxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and magnesium hydroxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
2 | Reducing | Reducing | ||
Mg(OH)2 | Magnesium hydroxide | 1 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BeO | Beryllium oxide | 2 | Oxidized | – |
1 | Reduced | – | ||
1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and magnesium hydroxide◆
ΔrG −327.1 kJ/mol K 2.02 × 1057 pK −57.31
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 | −294.7 | −327.1 | 109.46 | −5.16 |
−147.3 | −163.6 | 54.730 | −2.58 | |
per 1 mol of | −294.7 | −327.1 | 109.46 | −5.16 |
per 1 mol of | −147.3 | −163.6 | 54.730 | −2.58 |
−294.7 | −327.1 | 109.46 | −5.16 | |
−294.7 | −327.1 | 109.46 | −5.16 |
Changes in standard condition (2)
- Reaction of 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 | −298.7 | – | – | – |
−149.3 | – | – | – | |
per 1 mol of | −298.7 | – | – | – |
per 1 mol of | −149.3 | – | – | – |
−298.7 | – | – | – | |
−298.7 | – | – | – |
Changes in aqueous solution (1)
- Reaction of and magnesium hydroxide◆
ΔrG −327.1 kJ/mol K 2.02 × 1057 pK −57.31
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 | −294.7 | −327.1 | 109.46 | −5.16 |
−147.3 | −163.6 | 54.730 | −2.58 | |
per 1 mol of | −294.7 | −327.1 | 109.46 | −5.16 |
per 1 mol of | −147.3 | −163.6 | 54.730 | −2.58 |
−294.7 | −327.1 | 109.46 | −5.16 | |
−294.7 | −327.1 | 109.46 | −5.16 |
Changes in aqueous solution (2)
- Reaction of and magnesium hydroxide◆
ΔrG −309.5 kJ/mol K 1.67 × 1054 pK −54.22
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 | −298.9 | −309.5 | 556 | – |
−149.4 | −154.8 | 278 | – | |
per 1 mol of | −298.9 | −309.5 | 556 | – |
per 1 mol of | −149.4 | −154.8 | 278 | – |
−298.9 | −309.5 | 556 | – | |
−298.9 | −309.5 | 556 | – |
Changes in aqueous solution (3)
- Reaction of 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 | −298.7 | – | – | – |
−149.3 | – | – | – | |
per 1 mol of | −298.7 | – | – | – |
per 1 mol of | −149.3 | – | – | – |
−298.7 | – | – | – | |
−298.7 | – | – | – |
Changes in aqueous solution (4)
- Reaction of 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 | −302.9 | – | – | – |
−151.4 | – | – | – | |
per 1 mol of | −302.9 | – | – | – |
per 1 mol of | −151.4 | – | – | – |
−302.9 | – | – | – | |
−302.9 | – | – | – |
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 |
---|---|---|---|---|
(cr) | 0[1] | 0[1] | 9.50[1] | 16.44[1] |
(g) | 324.3[1] | 286.6[1] | 136.269[1] | 20.786[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 |
---|---|---|---|---|
BeO (cr) | -609.6[1] | -580.3[1] | 14.14[1] | 25.52[1] |
BeO (g) | 117[1] | – | – | – |
(cr) | 0[1] | 0[1] | 32.68[1] | 24.89[1] |
(g) | 147.70[1] | 113.10[1] | 148.650[1] | 20.786[1] |
(g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
(ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 9.50 J · K−1 · mol−1
- ^ Cp°, 16.44 J · K−1 · mol−1
- ^ ΔfH°, 324.3 kJ · mol−1
- ^ ΔfG°, 286.6 kJ · mol−1
- ^ S°, 136.269 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · 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°, -609.6 kJ · mol−1
- ^ ΔfG°, -580.3 kJ · mol−1
- ^ S°, 14.14 J · K−1 · mol−1
- ^ Cp°, 25.52 J · K−1 · mol−1
- ^ ΔfH°, 117. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 32.68 J · K−1 · mol−1
- ^ Cp°, 24.89 J · K−1 · mol−1
- ^ ΔfH°, 147.70 kJ · mol−1
- ^ ΔfG°, 113.10 kJ · mol−1
- ^ S°, 148.650 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1