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6FeCl2 + 3HNO3 + 6H+ → 4FeCl3 + 2Fe3+ + 3HNO2 + 3H2O

Reaction of iron(II) chloride and nitric acid under acidic condition
6FeCl2Iron(II) chloride + 3HNO3Nitric acid + 6H+Hydrogen ion
4FeCl3Iron(III) chloride + 2Fe3+Iron(III) ion + 3HNO2Nitrous acid + 3H2OWater

The reaction of iron(II) chloride, nitric acid, and hydrogen ion yields iron(III) chloride, iron(III) ion, 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) chloride and nitric acid under acidic condition
6FeCl2Iron(II) chloride + 3HNO3Nitric acid + 6H+Hydrogen ion
4FeCl3Iron(III) chloride + 2Fe3+Iron(III) ion + 3HNO2Nitrous acid + 3H2OWater

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) chloride and nitric acid under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeCl2Iron(II) chloride6
Reducing
Oxidizable
HNO3Nitric acid3
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion6
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
FeCl3Iron(III) chloride4
Oxidized
Fe3+Iron(III) ion2
Oxidized
HNO2Nitrous acid3
Reduced
H2OWater3
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) chloride and nitric acid under acidic condition
ΔrG−482.2 kJ/mol
K3.00 × 1084
pK−84.48
6FeCl2Un-ionized aqueous solution + 3HNO3Ionized aqueous solution + 6H+Un-ionized aqueous solution
4FeCl3Un-ionized aqueous solution + 2Fe3+Un-ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
−482.2
per 1 mol of
−80.37
per 1 mol of
−160.7
per 1 mol of
Hydrogen ion
−80.37
per 1 mol of
−120.5
per 1 mol of
Iron(III) ion
−241.1
per 1 mol of
−160.7
per 1 mol of
−160.7

Changes in standard condition (2)

Reaction of iron(II) chloride and nitric acid under acidic condition
ΔrG−457.4 kJ/mol
K1.36 × 1080
pK−80.13
6FeCl2Un-ionized aqueous solution + 3HNO3Ionized aqueous solution + 6H+Un-ionized aqueous solution
4FeCl3Ionized aqueous solution + 2Fe3+Un-ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
−457.4
per 1 mol of
−76.23
per 1 mol of
−152.5
per 1 mol of
Hydrogen ion
−76.23
per 1 mol of
−114.3
per 1 mol of
Iron(III) ion
−228.7
per 1 mol of
−152.5
per 1 mol of
−152.5

Changes in standard condition (3)

Reaction of iron(II) chloride and nitric acid under acidic condition
ΔrG−108.8 kJ/mol
K1.15 × 1019
pK−19.06
6FeCl2Ionized aqueous solution + 3HNO3Ionized aqueous solution + 6H+Un-ionized aqueous solution
4FeCl3Un-ionized aqueous solution + 2Fe3+Un-ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
−108.8
per 1 mol of
−18.13
per 1 mol of
−36.27
per 1 mol of
Hydrogen ion
−18.13
per 1 mol of
−27.20
per 1 mol of
Iron(III) ion
−54.40
per 1 mol of
−36.27
per 1 mol of
−36.27

Changes in standard condition (4)

Reaction of iron(II) chloride and nitric acid under acidic condition
ΔrG−84.0 kJ/mol
K5.20 × 1014
pK−14.72
6FeCl2Ionized aqueous solution + 3HNO3Ionized aqueous solution + 6H+Un-ionized aqueous solution
4FeCl3Ionized aqueous solution + 2Fe3+Un-ionized aqueous solution + 3HNO2Un-ionized aqueous solution + 3H2OLiquid
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
−350.4−84.0−891.9
per 1 mol of
−58.40−14.0−148.7
per 1 mol of
−116.8−28.0−297.3
per 1 mol of
Hydrogen ion
−58.40−14.0−148.7
per 1 mol of
−87.60−21.0−223.0
per 1 mol of
Iron(III) ion
−175.2−42.0−445.9
per 1 mol of
−116.8−28.0−297.3
per 1 mol of
−116.8−28.0−297.3

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
FeCl2 (cr)-341.79[1]-302.30[1]117.95[1]76.65[1]
FeCl2 (g)-148.5[1]
FeCl2 (ai)-423.4[1]-341.34[1]-24.7[1]
FeCl2 (ao)-279.1[1]
FeCl2 (cr)
2 hydrate
-953.1[1]
FeCl2 (cr)
4 hydrate
-1549.3[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, (ao):Un-ionized aqueous solution, (l):Liquid

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
FeCl3 (cr)-399.49[1]-334.00[1]142.3[1]96.65[1]
FeCl3 (g)-254.0[1]
FeCl3 (ai)-550.2[1]-398.3[1]-146.4[1]
FeCl3 (ao)-404.5[1]
FeCl3 (cr)
6 hydrate
-2223.8[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]
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]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)