You-iggy
  1. Home
  2. Chemical reactions
  3. 8KI + Ag2SO4 🔥→ 4K2O + 3I2 + S + 2AgI

8KI + Ag2SO4 🔥→ 4K2O + 3I2 + S + 2AgI

Last updated:
Reaction of potassium iodide and silver(I) sulfate
8KIPotassium iodide + Ag2SO4Silver(I) sulfate
🔥
⟶
4K2OPotassium oxide + 3I2Iodine + SSulfur + 2AgISilver(I) iodide

The reaction of potassium iodide and silver(I) sulfate yields potassium oxide, iodine, sulfur, and silver(I) 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

Reaction of potassium iodide and silver(I) sulfate
8KIPotassium iodide + Ag2SO4Silver(I) sulfate
🔥
⟶
4K2OPotassium oxide + 3I2Iodine + SSulfur + 2AgISilver(I) iodide

General equation

Reaction of oxidizable species and reducible species
Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
🔥
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium iodide and silver(I) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide8
Reducing
Oxidizable
Ag2SO4Silver(I) sulfate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide4
–
–
I2Iodine3
Oxidized
–
SSulfur1
Reduced
–
AgISilver(I) iodide2
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium iodide and silver(I) sulfate
◆
ΔrG1796.8 kJ/mol
K0.16 × 10−314
pK314.79
8KICrystalline solid + Ag2SO4Crystalline solid
🔥
⟶
4K2OCrystalline solid + 3I2Crystalline solid + SCrystalline solidrhombic + 2AgICrystalline 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
1769.41796.8−63.479.6
per 1 mol of
221.18224.60−7.929.95
per 1 mol of
1769.41796.8−63.479.6
per 1 mol of
442.35449.20−15.819.9
per 1 mol of
589.80598.93−21.126.5
per 1 mol of
1769.41796.8−63.479.6
per 1 mol of
884.70898.40−31.739.8

Changes in standard condition (2)

Reaction of potassium iodide and silver(I) sulfate
8KICrystalline solid + Ag2SO4Crystalline solid
🔥
⟶
4K2OCrystalline solid + 3I2Crystalline solid + SCrystalline solidmonoclinic + 2AgICrystalline 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
1769.7–––
per 1 mol of
221.21–––
per 1 mol of
1769.7–––
per 1 mol of
442.43–––
per 1 mol of
589.90–––
per 1 mol of
1769.7–––
per 1 mol of
884.85–––

Changes in aqueous solution (1)

Reaction of potassium iodide and silver(I) sulfate
◆
ΔrG2080.9 kJ/mol
K0.28 × 10−364
pK364.56
8KIIonized aqueous solution + Ag2SO4Ionized aqueous solution
🔥
⟶
4K2OCrystalline solid + 3I2Un-ionized aqueous solution + SCrystalline solidrhombic + 2AgIIonized 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
1881.22080.9−688.1–
per 1 mol of
235.15260.11−86.01–
per 1 mol of
1881.22080.9−688.1–
per 1 mol of
470.30520.23−172.0–
per 1 mol of
627.07693.63−229.4–
per 1 mol of
1881.22080.9−688.1–
per 1 mol of
940.601040.5−344.1–

Changes in aqueous solution (2)

Reaction of potassium iodide and silver(I) sulfate
◆
ΔrG2005.7 kJ/mol
K0.41 × 10−351
pK351.38
8KIIonized aqueous solution + Ag2SO4Ionized aqueous solution
🔥
⟶
4K2OCrystalline solid + 3I2Un-ionized aqueous solution + SCrystalline solidrhombic + 2AgIUn-ionized 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
–2005.7––
per 1 mol of
–250.71––
per 1 mol of
–2005.7––
per 1 mol of
–501.43––
per 1 mol of
–668.57––
per 1 mol of
–2005.7––
per 1 mol of
–1002.9––

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]
Ag2SO4 (cr)-715.88[1]-618.41[1]200.4[1]131.38[1]
Ag2SO4 (ai)-698.10[1]-590.30[1]165.7[1]-251[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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[1]–
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
AgI (cr)-61.84[1]-66.19[1]115.5[1]56.82[1]
AgI (ai)50.38[1]25.52[1]184.1[1]-120.5[1]
AgI (ao)–-12.1[1]––
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):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