You-iggy

2FeI2 + HNO3 + 6H+ 🔥→ 2Fe3+ + HNO2 + 4HI↑ + H2O

Reaction of iron(II) iodide and nitric acid under acidic condition
2FeI2Iron(II) iodide + HNO3Nitric acid + 6H+Hydrogen ion
🔥
2Fe3+Iron(III) ion + HNO2Nitrous acid + 4HIHydrogen iodide + H2OWater

The reaction of iron(II) iodide, nitric acid, and hydrogen ion yields iron(III) ion, nitrous acid, hydrogen iodide, 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
2FeI2Iron(II) iodide + HNO3Nitric acid + 6H+Hydrogen ion
🔥
2Fe3+Iron(III) ion + HNO2Nitrous acid + 4HIHydrogen iodide + H2OWater

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) iodide2
Reducing
Oxidizable
HNO3Nitric acid1
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion6
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe3+Iron(III) ion2
Oxidized
HNO2Nitrous acid1
Reduced
HIHydrogen iodide4
H2OWater1
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) iodide and nitric acid under acidic condition
ΔrG185.0 kJ/mol
K0.39 × 10−32
pK32.41
2FeI2Ionized aqueous solution + HNO3Ionized aqueous solution + 6H+Un-ionized aqueous solution
🔥
2Fe3+Un-ionized aqueous solution + HNO2Un-ionized aqueous solution + 4HIGas + H2OLiquid
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
210.5185.083.9
per 1 mol of
105.392.5042.0
per 1 mol of
210.5185.083.9
per 1 mol of
Hydrogen ion
35.0830.8314.0
per 1 mol of
Iron(III) ion
105.392.5042.0
per 1 mol of
210.5185.083.9
per 1 mol of
52.6346.2521.0
per 1 mol of
210.5185.083.9

Changes in standard condition (2)

Reaction of iron(II) iodide and nitric acid under acidic condition
ΔrG−28.1 kJ/mol
K8.37 × 104
pK−4.92
2FeI2Ionized aqueous solution + HNO3Ionized aqueous solution + 6H+Un-ionized aqueous solution
🔥
2Fe3+Un-ionized aqueous solution + HNO2Un-ionized aqueous solution + 4HIIonized aqueous solution + H2OLiquid
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
−116.2−28.1−297.3
per 1 mol of
−58.10−14.1−148.7
per 1 mol of
−116.2−28.1−297.3
per 1 mol of
Hydrogen ion
−19.37−4.68−49.55
per 1 mol of
Iron(III) ion
−58.10−14.1−148.7
per 1 mol of
−116.2−28.1−297.3
per 1 mol of
−29.05−7.03−74.33
per 1 mol of
−116.2−28.1−297.3

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
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
Fe3+ (g)5712.8[1]
Fe3+ (ao)-48.5[1]-4.7[1]-315.9[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]
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[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]
* (g):Gas, (ao):Un-ionized aqueous solution, (ai):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)