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14FeI2 + 2HNO3 + 42H+ 🔥→ 14Fe3+ + N2H4 + 28HI↑ + 6H2O

Reaction of iron(II) iodide and nitric acid under acidic condition
14FeI2Iron(II) iodide + 2HNO3Nitric acid + 42H+Hydrogen ion
🔥
14Fe3+Iron(III) ion + N2H4Hydrazine + 28HIHydrogen iodide + 6H2OWater

The reaction of iron(II) iodide, nitric acid, and hydrogen ion yields iron(III) ion, hydrazine, 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
14FeI2Iron(II) iodide + 2HNO3Nitric acid + 42H+Hydrogen ion
🔥
14Fe3+Iron(III) ion + N2H4Hydrazine + 28HIHydrogen iodide + 6H2OWater

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) iodide14
Reducing
Oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion42
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe3+Iron(III) ion14
Oxidized
N2H4Hydrazine1
Reduced
HIHydrogen iodide28
H2OWater6
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) iodide and nitric acid under acidic condition
ΔrG1458.3 kJ/mol
K0.33 × 10−255
pK255.48
14FeI2Ionized aqueous solution + 2HNO3Ionized aqueous solution + 42H+Un-ionized aqueous solution
🔥
14Fe3+Un-ionized aqueous solution + N2H4Un-ionized aqueous solution + 28HIGas + 6H2OLiquid
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
1590.91458.3438
per 1 mol of
113.64104.1631.3
per 1 mol of
795.45729.15219
per 1 mol of
Hydrogen ion
37.87934.72110.4
per 1 mol of
Iron(III) ion
113.64104.1631.3
per 1 mol of
1590.91458.3438
per 1 mol of
56.81852.08215.6
per 1 mol of
265.15243.0573.0

Changes in standard condition (2)

Reaction of iron(II) iodide and nitric acid under acidic condition
ΔrG−33.2 kJ/mol
K6.55 × 105
pK−5.82
14FeI2Ionized aqueous solution + 2HNO3Ionized aqueous solution + 42H+Un-ionized aqueous solution
🔥
14Fe3+Un-ionized aqueous solution + N2H4Un-ionized aqueous solution + 28HIIonized aqueous solution + 6H2OLiquid
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
−695.9−33.2−2230
per 1 mol of
−49.71−2.37−159.3
per 1 mol of
−347.9−16.6−1115
per 1 mol of
Hydrogen ion
−16.57−0.790−53.10
per 1 mol of
Iron(III) ion
−49.71−2.37−159.3
per 1 mol of
−695.9−33.2−2230
per 1 mol of
−24.85−1.19−79.64
per 1 mol of
−116.0−5.53−371.7

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]
N2H4 (l)50.63[1]149.34[1]121.21[1]98.87[1]
N2H4 (g)95.40[1]159.35[1]238.47[1]49.58[1]
N2H4 (ao)34.31[1]128.1[1]138[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, (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid

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)