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2KI + HgSO4 + 4H+ ๐Ÿ”ฅโ†’ 2K+ + I2 + SO2โ†‘ + Hg2+ + 2H2O

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Reaction of potassium iodide and mercury(II) sulfate under acidic condition
2KIPotassium iodide + HgSO4Mercury(II) sulfate + 4H+Hydrogen ion
๐Ÿ”ฅ
โŸถ
2K+Potassium ion + I2Iodine + SO2โ†‘Sulfur dioxide + Hg2+Mercury(II) ion + 2H2OWater

The reaction of potassium iodide, mercury(II) sulfate, and hydrogen ion yields potassium ion, iodine, sulfur dioxide, mercury(II) ion, 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

Reaction of potassium iodide and mercury(II) sulfate under acidic condition
2KIPotassium iodide + HgSO4Mercury(II) sulfate + 4H+Hydrogen ion
๐Ÿ”ฅ
โŸถ
2K+Potassium ion + I2Iodine + SO2โ†‘Sulfur dioxide + Hg2+Mercury(II) ion + 2H2OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
โŸถ
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of potassium iodide and mercury(II) sulfate under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KIPotassium iodide2
Reducing
Oxidizable
HgSO4Mercury(II) sulfate1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion4
โ€“
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
K+Potassium ion2
โ€“
โ€“
I2Iodine1
Oxidized
โ€“
SO2Sulfur dioxide1
Reduced
โ€“
Hg2+Mercury(II) ion1
โ€“
โ€“
H2OWater2
โ€“
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium iodide and mercury(II) sulfate under acidic condition
โ—†
ฮ”rG97.7 kJ/mol
K0.77 ร— 10โˆ’17
pK17.12
2KIIonized aqueous solution + HgSO4Un-ionized aqueous solution + 4H+Un-ionized aqueous solution
๐Ÿ”ฅ
โŸถ
2K+Un-ionized aqueous solution + I2Un-ionized aqueous solution + SO2โ†‘Gas + Hg2+Un-ionized aqueous solution + 2H2OLiquid
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
โ€“97.7โ€“โ€“
per 1 mol of
โ€“48.9โ€“โ€“
โ€“97.7โ€“โ€“
per 1 mol of
Hydrogen ion
โ€“24.4โ€“โ€“
per 1 mol of
Potassium ion
โ€“48.9โ€“โ€“
per 1 mol of
โ€“97.7โ€“โ€“
per 1 mol of
โ€“97.7โ€“โ€“
per 1 mol of
Mercury(II) ion
โ€“97.7โ€“โ€“
per 1 mol of
โ€“48.9โ€“โ€“

Changes in standard condition (2)

Reaction of potassium iodide and mercury(II) sulfate under acidic condition
โ—†
ฮ”rG97.2 kJ/mol
K0.94 ร— 10โˆ’17
pK17.03
2KIIonized aqueous solution + HgSO4Un-ionized aqueous solution + 4H+Un-ionized aqueous solution
๐Ÿ”ฅ
โŸถ
2K+Un-ionized aqueous solution + I2Un-ionized aqueous solution + SO2โ†‘Un-ionized aqueous solution + Hg2+Un-ionized aqueous solution + 2H2OLiquid
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
โ€“97.2โ€“โ€“
per 1 mol of
โ€“48.6โ€“โ€“
โ€“97.2โ€“โ€“
per 1 mol of
Hydrogen ion
โ€“24.3โ€“โ€“
per 1 mol of
Potassium ion
โ€“48.6โ€“โ€“
per 1 mol of
โ€“97.2โ€“โ€“
per 1 mol of
โ€“97.2โ€“โ€“
per 1 mol of
Mercury(II) ion
โ€“97.2โ€“โ€“
per 1 mol of
โ€“48.6โ€“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
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]
HgSO4 (cr)-707.5[1]โ€“โ€“โ€“
HgSO4 (ao)โ€“-588.2[1]โ€“โ€“
H+ (g)1536.202[1]โ€“โ€“โ€“
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

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
K+ (g)514.26[1]โ€“โ€“โ€“
K+ (ao)-252.38[1]-283.27[1]102.5[1]21.8[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]โ€“
SO2 (l)-320.5[1]โ€“โ€“โ€“
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[1]โ€“
Hg2+ (g)2890.47[1]โ€“โ€“โ€“
Hg2+ (ao)171.1[1]164.40[1]-32.2[1]โ€“
H2O (cr)โ€“โ€“โ€“โ€“
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]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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)