Fe(OH)2 + SrO → FeO + Sr(OH)2
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The reaction of iron(II) hydroxide and strontium oxide yields iron(II) oxide and strontium hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(II) hydroxide and strontium oxide
General equation
- Hydroxide baseLewis base + Dehydrating basic oxideLewis acid ⟶ Basic oxide + Hydroxide baseLewis conjugate
Oxidation state of each atom
- Reaction of iron(II) hydroxide and strontium oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(OH)2 | Iron(II) hydroxide | 1 | Lewis base | Hydroxide base |
| SrO | Strontium oxide | 1 | Lewis acid | Dehydrating basic oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeO | Iron(II) oxide | 1 | – | Basic oxide |
| Sr(OH)2 | Strontium hydroxide | 1 | Lewis conjugate | Hydroxide base |
Thermodynamic changes
Changes in standard condition
- Reaction of iron(II) hydroxide and strontium oxide
| 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 | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
Changes in aqueous solution
- Reaction of iron(II) hydroxide and strontium oxide
| 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 | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
per 1 mol of | −70.0 | – | – | – |
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 |
|---|---|---|---|---|
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[1] | – | – | – |
| SrO (cr) | -592.0[1] | -561.9[1] | 54.4[1] | 45.02[1] |
| SrO (g) | -8[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas
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 |
|---|---|---|---|---|
| FeO (cr) | -272.0[1] | – | – | – |
| Sr(OH)2 (cr) | -959.0[1] | – | – | – |
| Sr(OH)2 (g) | -565[1] | – | – | – |
| Sr(OH)2 (cr) 1 hydrate | -1264.8[1] | – | – | – |
| Sr(OH)2 (cr) 8 hydrate | -3352.2[1] | – | – | – |
* (cr):Crystalline solid, (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°, -569.0 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, 88. J · K−1 · mol−1
- ^ ΔfH°, -372. kJ · mol−1
- ^ ΔfH°, -592.0 kJ · mol−1
- ^ ΔfG°, -561.9 kJ · mol−1
- ^ S°, 54.4 J · K−1 · mol−1
- ^ Cp°, 45.02 J · K−1 · mol−1
- ^ ΔfH°, -8. kJ · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1
- ^ ΔfH°, -959.0 kJ · mol−1
- ^ ΔfH°, -565. kJ · mol−1
- ^ ΔfH°, -1264.8 kJ · mol−1
- ^ ΔfH°, -3352.2 kJ · mol−1