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3Ca(ClO)2 + 6HNO3 → 3Ca(NO2)2 + 4ClO2↑ + 2HClO + 2H2O

The reaction of calcium hypochlorite and nitric acid yields calcium nitrite, chlorine dioxide, hypochlorous acid, and water (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 hardly oxidizable species and oxidizing species
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Ca(ClO)2Calcium hypochlorite3
Reducing
Hardly oxidizable
HNO3Nitric acid6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ca(NO2)2Calcium nitrite3
Reduced
ClO2Chlorine dioxide4
Oxidized
HClOHypochlorous acid2
H2OWater2

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of calcium hypochlorite and nitric acid
3Ca(ClO)2Aqueous solution + 6HNO3Ionized aqueous solution
3Ca(NO2)2Crystalline solid + 4ClO2Gas + 2HClOUn-ionized aqueous solution + 2H2OLiquid
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
879.7
293.2
per 1 mol of
146.6
per 1 mol of
293.2
per 1 mol of
219.9
per 1 mol of
439.9
per 1 mol of
439.9

Changes in aqueous solution (2)

Reaction of calcium hypochlorite and nitric acid
3Ca(ClO)2Aqueous solution + 6HNO3Ionized aqueous solution
3Ca(NO2)2Crystalline solid + 4ClO2Un-ionized aqueous solution + 2HClOUn-ionized aqueous solution + 2H2OLiquid
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
769.3
256.4
per 1 mol of
128.2
per 1 mol of
256.4
per 1 mol of
192.3
per 1 mol of
384.6
per 1 mol of
384.6

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
Ca(ClO)2 (aq)-754.4[1]
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (aq):Aqueous solution, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution

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
Ca(NO2)2 (cr)-741.4[1]
Ca(NO2)2 (cr)
4 hydrate
-1885.7[1]
ClO2 (g)102.5[1]120.5[1]256.84[1]41.97[1]
ClO2 (ao)74.9[1]120.1[1]164.8[1]
HClO (g)-78.7[1]-66.1[1]236.67[1]37.15[1]
HClO (ao)-120.9[1]-79.9[1]142[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, (ao):Un-ionized aqueous solution, (l):Liquid

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)