2HI + Mg(OH)2 → MgI2 + 2H2O
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The reaction of hydrogen iodide and magnesium hydroxide yields magnesium iodide and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen iodide and magnesium hydroxide
General equation
- Reaction of acid and base
- AcidBrønsted acid + BaseBrønsted base ⟶ SaltConjugate base + (H2O)(Conjugate acid)
- Reaction of acid and hydroxide base
- AcidBrønsted acid + Hydroxide baseBrønsted base ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of strong acid and strong base
- Strong acidBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong acid and strong baseConjugate base + (H2O)(Conjugate acid)
Oxidation state of each atom
- Reaction of hydrogen iodide and magnesium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HI | Hydrogen iodide | 2 | Brønsted acid | Acid Strong acid |
| Mg(OH)2 | Magnesium hydroxide | 1 | Brønsted base | Base Hydroxide base Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MgI2 | Magnesium iodide | 1 | Conjugate base | Salt Salt of strong acid and strong base |
| H2O | Water | 2 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen iodide and magnesium hydroxide◆
ΔrG −2.3 kJ/mol K 2.53 × 100 pK −0.40
| 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 | −64.1 | −2.3 | −206.8 | – |
per 1 mol of | −32.0 | −1.1 | −103.4 | – |
per 1 mol of | −64.1 | −2.3 | −206.8 | – |
per 1 mol of | −64.1 | −2.3 | −206.8 | – |
per 1 mol of | −32.0 | −1.1 | −103.4 | – |
Changes in standard condition (2)
- Reaction of hydrogen iodide 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 | −68.1 | – | – | – |
per 1 mol of | −34.0 | – | – | – |
per 1 mol of | −68.1 | – | – | – |
per 1 mol of | −68.1 | – | – | – |
per 1 mol of | −34.0 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen iodide and magnesium hydroxide◆
ΔrG −95.7 kJ/mol K 5.83 × 1016 pK −16.77
| 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 | −113.96 | −95.7 | −61.5 | – |
per 1 mol of | −56.980 | −47.9 | −30.8 | – |
per 1 mol of | −113.96 | −95.7 | −61.5 | – |
per 1 mol of | −113.96 | −95.7 | −61.5 | – |
per 1 mol of | −56.980 | −47.9 | −30.8 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen iodide 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 | −118.0 | – | – | – |
per 1 mol of | −59.00 | – | – | – |
per 1 mol of | −118.0 | – | – | – |
per 1 mol of | −118.0 | – | – | – |
per 1 mol of | −59.00 | – | – | – |
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 |
|---|---|---|---|---|
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[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] | – |
* (g):Gas, (ai):Ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid
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 |
|---|---|---|---|---|
| MgI2 (cr) | -364.0[1] | -358.2[1] | 129.7[1] | – |
| MgI2 (g) | -172[1] | – | – | – |
| MgI2 (ai) | -577.22[1] | -558.1[1] | 84.5[1] | – |
| 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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid
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°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 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°, -364.0 kJ · mol−1
- ^ ΔfG°, -358.2 kJ · mol−1
- ^ S°, 129.7 J · K−1 · mol−1
- ^ ΔfH°, -172. kJ · mol−1
- ^ ΔfH°, -577.22 kJ · mol−1
- ^ ΔfG°, -558.1 kJ · mol−1
- ^ S°, 84.5 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