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11KI + 3Sr(NO3)2 🔥→ 5KIO3 + 3K2O + 3N2↑ + 3SrI2

The reaction of potassium iodide and strontium nitrate yields potassium iodate, potassium oxide, nitrogen, and strontium iodide (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 oxidizable species and oxidizing species
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide11
Reducing
Oxidizable
Sr(NO3)2Strontium nitrate3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
KIO3Potassium iodate5
Oxidized
K2OPotassium oxide3
N2Nitrogen3
Reduced
SrI2Strontium iodide3

Thermodynamic changes

Changes in standard condition

Reaction of potassium iodide and strontium nitrate
11KICrystalline solid + 3Sr(NO3)2Crystalline solid
🔥
5KIO3Crystalline solid + 3K2OCrystalline solid + 3N2Gas + 3SrI2Crystalline solid
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
1275.983.7
per 1 mol of
115.997.61
per 1 mol of
425.3027.9
per 1 mol of
255.1816.7
per 1 mol of
425.3027.9
per 1 mol of
425.3027.9
per 1 mol of
425.3027.9

Changes in aqueous solution

Reaction of potassium iodide and strontium nitrate
ΔrG1019.1 kJ/mol
K0.29 × 10−178
pK178.54
11KIIonized aqueous solution + 3Sr(NO3)2Ionized aqueous solution
🔥
5KIO3Ionized aqueous solution + 3K2OCrystalline solid + 3N2Gas + 3SrI2Ionized 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
843.81019.1−600.8
per 1 mol of
76.7192.645−54.62
per 1 mol of
281.3339.70−200.3
per 1 mol of
168.8203.82−120.2
per 1 mol of
281.3339.70−200.3
per 1 mol of
281.3339.70−200.3
per 1 mol of
281.3339.70−200.3

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
KI (cr)-327.900[1]-324.892[1]106.32[1]52.93[1]
KI (g)-125.5[1]-166.1[1]258.3[1]37.11[1]
KI (ai)-307.57[1]-334.85[1]213.8[1]-120.5[1]
Sr(NO3)2 (cr)-978.22[1]-780.02[1]194.56[1]149.91[1]
Sr(NO3)2 (ai)-960.52[1]-781.98[1]260.2[1]
Sr(NO3)2 (cr)
4 hydrate
-2154.8[1]-1730.39[1]369.0[1]
* (cr):Crystalline solid, (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
KIO3 (cr)-501.37[1]-418.35[1]151.46[1]106.48[1]
KIO3 (ai)-473.6[1]-411.2[1]220.9[1]
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
N2 (g)0[1]0[1]191.61[1]29.125[1]
SrI2 (cr)-558.1[1]81.6[1]
SrI2 (g)-272[1]
SrI2 (ai)-656.18[1]-662.62[1]190.0[1]
SrI2 (cr)
1 hydrate
-886.6[1]119.2[1]
SrI2 (cr)
2 hydrate
-1182.4[1]163.6[1]
SrI2 (cr)
6 hydrate
-2388.6[1]355.2[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)

  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education