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14KClO + Mg(OH)2 ๐Ÿ”ฅโ†’ 2KOH + 6K2O + Mg(ClO4)2 + 6Cl2โ†‘

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Reaction of potassium hypochlorite and magnesium hydroxide
14KClOPotassium hypochlorite + Mg(OH)2Magnesium hydroxide
๐Ÿ”ฅ
โŸถ
2KOHPotassium hydroxide + 6K2OPotassium oxide + Mg(ClO4)2Magnesium perchlorate + 6Cl2โ†‘Chlorine

The reaction of potassium hypochlorite and magnesium hydroxide yields potassium hydroxide, potassium oxide, magnesium perchlorate, and chlorine (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of potassium hypochlorite and magnesium hydroxide
14KClOPotassium hypochlorite + Mg(OH)2Magnesium hydroxide
๐Ÿ”ฅ
โŸถ
2KOHPotassium hydroxide + 6K2OPotassium oxide + Mg(ClO4)2Magnesium perchlorate + 6Cl2โ†‘Chlorine

General equation

Reaction of self redoxing species and base
Self-redoxing speciesSelf redox agent + BaseNon-redox agent
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium hypochlorite and magnesium hydroxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KClOPotassium hypochlorite14
โ€“
Self redoxing
Mg(OH)2Magnesium hydroxide1
โ€“
Base

Products

Chemical formulaNameCoefficientTypeType in general
equation
KOHPotassium hydroxide2
โ€“
โ€“
K2OPotassium oxide6
โ€“
โ€“
Mg(ClO4)2Magnesium perchlorate1
Oxidized
โ€“
Cl2Chlorine6
Reduced
โ€“

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hypochlorite and magnesium hydroxide
โ—†
ฮ”rG2028.1 kJ/mol
K0.49 ร— 10โˆ’355
pK355.31
14KClOIonized aqueous solution + Mg(OH)2Crystalline solid
๐Ÿ”ฅ
โŸถ
2KOHIonized aqueous solution + 6K2OCrystalline solid + Mg(ClO4)2Ionized aqueous solution + 6Cl2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
2096.92028.1205โ€“
149.78144.8614.6โ€“
2096.92028.1205โ€“
1048.51014.0103โ€“
per 1 mol of
349.48338.0234.2โ€“
2096.92028.1205โ€“
per 1 mol of
349.48338.0234.2โ€“

Changes in aqueous solution (2)

Reaction of potassium hypochlorite and magnesium hydroxide
โ—†
ฮ”rG2069.8 kJ/mol
K0.24 ร— 10โˆ’362
pK362.61
14KClOIonized aqueous solution + Mg(OH)2Crystalline solid
๐Ÿ”ฅ
โŸถ
2KOHIonized aqueous solution + 6K2OCrystalline solid + Mg(ClO4)2Ionized aqueous solution + 6Cl2โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
1956.52069.8โˆ’407โ€“
139.75147.84โˆ’29.1โ€“
1956.52069.8โˆ’407โ€“
978.251034.9โˆ’204โ€“
per 1 mol of
326.08344.97โˆ’67.8โ€“
1956.52069.8โˆ’407โ€“
per 1 mol of
326.08344.97โˆ’67.8โ€“

Changes in aqueous solution (3)

Reaction of potassium hypochlorite and magnesium hydroxide
14KClOIonized aqueous solution + Mg(OH)2Amorphous solidprecipitated
๐Ÿ”ฅ
โŸถ
2KOHIonized aqueous solution + 6K2OCrystalline solid + Mg(ClO4)2Ionized aqueous solution + 6Cl2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
2092.9โ€“โ€“โ€“
149.49โ€“โ€“โ€“
2092.9โ€“โ€“โ€“
1046.5โ€“โ€“โ€“
per 1 mol of
348.82โ€“โ€“โ€“
2092.9โ€“โ€“โ€“
per 1 mol of
348.82โ€“โ€“โ€“

Changes in aqueous solution (4)

Reaction of potassium hypochlorite and magnesium hydroxide
14KClOIonized aqueous solution + Mg(OH)2Amorphous solidprecipitated
๐Ÿ”ฅ
โŸถ
2KOHIonized aqueous solution + 6K2OCrystalline solid + Mg(ClO4)2Ionized aqueous solution + 6Cl2โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
1952.5โ€“โ€“โ€“
139.46โ€“โ€“โ€“
1952.5โ€“โ€“โ€“
976.25โ€“โ€“โ€“
per 1 mol of
325.42โ€“โ€“โ€“
1952.5โ€“โ€“โ€“
per 1 mol of
325.42โ€“โ€“โ€“

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
KClO (ai)-359.4[1]-320.0[1]146[1]โ€“
Mg(OH)2 (cr)-924.54[1]-833.51[1]63.18[1]77.03[1]
Mg(OH)2 (am)
precipitated
-920.5[1]โ€“โ€“โ€“
Mg(OH)2 (g)-561[1]โ€“โ€“โ€“
Mg(OH)2 (ai)-926.84[1]-769.4[1]-159.4[1]โ€“
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid, (g):Gas

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’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]โ€“
KOH (cr)
2 hydrate
-1051.0[1]-887.3[1]150.6[1]โ€“
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]โ€“โ€“โ€“
Mg(ClO4)2 (cr)-568.90[1]โ€“โ€“โ€“
Mg(ClO4)2 (ai)-725.51[1]-471.8[1]225.9[1]โ€“
Mg(ClO4)2 (cr)
2 hydrate
-1218.8[1]โ€“โ€“โ€“
Mg(ClO4)2 (cr)
4 hydrate
-1837.2[1]โ€“โ€“โ€“
Mg(ClO4)2 (cr)
6 hydrate
-2445.5[1]-1862.7[1]520.9[1]โ€“
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]โ€“
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education