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6FeI2 + 12HNO3 + 15H+ → Fe(NO3)3 + 5Fe3+ + 6I2 + 9HNO2 + 9H2O

Reaction of iron(II) iodide and nitric acid under acidic condition
6FeI2Iron(II) iodide + 12HNO3Nitric acid + 15H+Hydrogen ion
Fe(NO3)3Iron(III) nitrate + 5Fe3+Iron(III) ion + 6I2Iodine + 9HNO2Nitrous acid + 9H2OWater

The reaction of iron(II) iodide, nitric acid, and hydrogen ion yields iron(III) nitrate, iron(III) ion, iodine, nitrous 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

Reaction of iron(II) iodide and nitric acid under acidic condition
6FeI2Iron(II) iodide + 12HNO3Nitric acid + 15H+Hydrogen ion
Fe(NO3)3Iron(III) nitrate + 5Fe3+Iron(III) ion + 6I2Iodine + 9HNO2Nitrous acid + 9H2OWater

General equation

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

Oxidation state of each atom

Reaction of iron(II) iodide and nitric acid under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeI2Iron(II) iodide6
Reducing
Oxidizable
HNO3Nitric acid12
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion15
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate1
Oxidized
Fe3+Iron(III) ion5
Oxidized
I2Iodine6
Oxidized
HNO2Nitrous acid9
Reduced
H2OWater9
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) iodide and nitric acid under acidic condition
ΔrG−425.7 kJ/mol
K3.80 × 1074
pK−74.58
6FeI2Ionized aqueous solution + 12HNO3Ionized aqueous solution + 15H+Un-ionized aqueous solution
Fe(NO3)3Ionized aqueous solution + 5Fe3+Un-ionized aqueous solution + 6I2Un-ionized aqueous solution + 9HNO2Un-ionized aqueous solution + 9H2OLiquid
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
−737.0−425.7−1049.5
per 1 mol of
−122.8−70.95−174.92
per 1 mol of
−61.42−35.48−87.458
per 1 mol of
Hydrogen ion
−49.13−28.38−69.967
per 1 mol of
−737.0−425.7−1049.5
per 1 mol of
Iron(III) ion
−147.4−85.14−209.90
per 1 mol of
−122.8−70.95−174.92
per 1 mol of
−81.89−47.30−116.61
per 1 mol of
−81.89−47.30−116.61

Changes in standard condition (2)

Reaction of iron(II) iodide and nitric acid under acidic condition
6FeI2Ionized aqueous solution + 12HNO3Ionized aqueous solution + 15H+Un-ionized aqueous solution
Fe(NO3)3Aqueous solution + 5Fe3+Un-ionized aqueous solution + 6I2Un-ionized aqueous solution + 9HNO2Un-ionized aqueous solution + 9H2OLiquid
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
−741.2
per 1 mol of
−123.5
per 1 mol of
−61.77
per 1 mol of
Hydrogen ion
−49.41
per 1 mol of
−741.2
per 1 mol of
Iron(III) ion
−148.2
per 1 mol of
−123.5
per 1 mol of
−82.36
per 1 mol of
−82.36

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
FeI2 (cr)-113.0[1]
FeI2 (g)60.7[1]
FeI2 (ai)-199.6[1]-182.05[1]84.9[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]
H+ (g)1536.202[1]
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (ao):Un-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
Fe(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]
Fe(NO3)3 (aq)-674.9[1]
Fe(NO3)3 (cr)
9 hydrate
-3285.3[1]
Fe3+ (g)5712.8[1]
Fe3+ (ao)-48.5[1]-4.7[1]-315.9[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]
HNO2 (g)
cis
-77.99[1]-42.94[1]248.76[1]44.77[1]
HNO2 (g)
trans
-80.12[1]-45.24[1]249.22[1]46.07[1]
HNO2 (g)-79.5[1]-46.0[1]254.1[1]45.6[1]
HNO2 (ao)-119.2[1]-50.6[1]135.6[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]
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (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)