8KClO + Mg(OH)2 → 6KCl + 2KOH + Mg(ClO4)2
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The reaction of potassium hypochlorite and magnesium hydroxide yields potassium chloride, potassium hydroxide, and magnesium perchlorate (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 potassium hypochlorite and magnesium hydroxide
General equation
- Reaction of self redoxing species and base
- Self-redoxing speciesSelf redox agent + BaseNon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium hypochlorite and magnesium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO | Potassium hypochlorite | 8 | – | Self redoxing |
| Mg(OH)2 | Magnesium hydroxide | 1 | – | Base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KCl | Potassium chloride | 6 | Reduced | – |
| KOH | Potassium hydroxide | 2 | – | – |
| Mg(ClO4)2 | Magnesium perchlorate | 1 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hypochlorite and magnesium hydroxide◆
ΔrG −446.2 kJ/mol K 1.48 × 1078 pK −78.17
| 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 | −407.7 | −446.2 | 132 | – |
per 1 mol of | −50.96 | −55.77 | 16.5 | – |
per 1 mol of | −407.7 | −446.2 | 132 | – |
per 1 mol of | −67.95 | −74.37 | 22.0 | – |
per 1 mol of | −203.8 | −223.1 | 66.0 | – |
per 1 mol of | −407.7 | −446.2 | 132 | – |
Changes in aqueous solution (2)
- Reaction of potassium hypochlorite 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 | −411.7 | – | – | – |
per 1 mol of | −51.46 | – | – | – |
per 1 mol of | −411.7 | – | – | – |
per 1 mol of | −68.62 | – | – | – |
per 1 mol of | −205.8 | – | – | – |
per 1 mol of | −411.7 | – | – | – |
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 |
|---|---|---|---|---|
| KClO (ai) | -359.4[1] | -320.0[1] | 146[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] | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous 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 |
|---|---|---|---|---|
| KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
| KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
| KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[1] |
| KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
| KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
| KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
| KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
| KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[1] | – |
| Mg(ClO4)2 (cr) | -568.90[1] | – | – | – |
| Mg(ClO4)2 (ai) | -725.51[1] | -471.8[1] | 225.9[1] | – |
| Mg(ClO4)2 (cr) 2 hydrate | -1218.8[1] | – | – | – |
| Mg(ClO4)2 (cr) 4 hydrate | -1837.2[1] | – | – | – |
| Mg(ClO4)2 (cr) 6 hydrate | -2445.5[1] | -1862.7[1] | 520.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):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°, -359.4 kJ · mol−1
- ^ ΔfG°, -320.0 kJ · mol−1
- ^ S°, 146. 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°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1
- ^ ΔfH°, -568.90 kJ · mol−1
- ^ ΔfH°, -725.51 kJ · mol−1
- ^ ΔfG°, -471.8 kJ · mol−1
- ^ S°, 225.9 J · K−1 · mol−1
- ^ ΔfH°, -1218.8 kJ · mol−1
- ^ ΔfH°, -1837.2 kJ · mol−1
- ^ ΔfH°, -2445.5 kJ · mol−1
- ^ ΔfG°, -1862.7 kJ · mol−1
- ^ S°, 520.9 J · K−1 · mol−1