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3KClO + H2SO4 → KClO3 + K2SO4 + 2HCl↑

The reaction of potassium hypochlorite and sulfuric acid yields potassium chlorate, potassium sulfate, and hydrogen chloride (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

General equation

Reaction of self redoxing species and acid
Self-redoxing speciesSelf redox agent + AcidNon-redox agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KClOPotassium hypochlorite3
Self redoxing
H2SO4Sulfuric acid1
Acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
KClO3Potassium chlorate1
Oxidized
K2SO4Potassium sulfate1
HClHydrogen chloride2
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hypochlorite and sulfuric acid
ΔrG−88.4 kJ/mol
K3.07 × 1015
pK−15.49
3KClOIonized aqueous solution + H2SO4Ionized aqueous solution
KClO3Ionized aqueous solution + K2SO4Ionized aqueous solution + 2HClGas
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
32.5−88.4406
10.8−29.5135
per 1 mol of
32.5−88.4406
per 1 mol of
32.5−88.4406
per 1 mol of
32.5−88.4406
per 1 mol of
16.3−44.2203

Changes in aqueous solution (2)

Reaction of potassium hypochlorite and sulfuric acid
ΔrG−160.2 kJ/mol
K1.16 × 1028
pK−28.07
3KClOIonized aqueous solution + H2SO4Ionized aqueous solution
KClO3Ionized aqueous solution + K2SO4Ionized aqueous solution + 2HClIonized aqueous solution
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
−117.2−160.2145
−39.07−53.4048.3
per 1 mol of
−117.2−160.2145
per 1 mol of
−117.2−160.2145
per 1 mol of
−117.2−160.2145
per 1 mol of
−58.60−80.1072.5

Thermodynamic data of reactants

Chemical formulaStandard 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]
H2SO4 (cr)
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[1]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (l):Liquid

Thermodynamic data of products

Chemical formulaStandard 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
KClO3 (cr)-397.73[1]-296.25[1]143.1[1]100.25[1]
KClO3 (ai)-356.35[1]-291.22[1]264.8[1]
K2SO4 (cr)-1437.79[1]-1321.37[1]175.56[1]131.46[1]
K2SO4 (g)-1096[1]-1033[1]364[1]108.8[1]
K2SO4 (ai)-1414.02[1]-1311.07[1]225.1[1]-251[1]
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

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)