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  3. 9FeCO3 + 6HNO3 + 24H^+ → Fe(NO3)3 + 8Fe^3+ + 3NO↑ + 9CO2↑ + 15H2O

9FeCO3 + 6HNO3 + 24H+ → Fe(NO3)3 + 8Fe3+ + 3NO↑ + 9CO2↑ + 15H2O

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Reaction of iron(II) carbonate and nitric acid under acidic condition
9FeCO3Iron(II) carbonate + 6HNO3Nitric acid + 24H+Hydrogen ion
⟶
Fe(NO3)3Iron(III) nitrate + 8Fe3+Iron(III) ion + 3NO↑Nitrogen monoxide + 9CO2↑Carbon dioxide + 15H2OWater

The reaction of iron(II) carbonate, nitric acid, and hydrogen ion yields iron(III) nitrate, iron(III) ion, nitrogen monoxide, carbon dioxide, 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) carbonate and nitric acid under acidic condition
9FeCO3Iron(II) carbonate + 6HNO3Nitric acid + 24H+Hydrogen ion
⟶
Fe(NO3)3Iron(III) nitrate + 8Fe3+Iron(III) ion + 3NO↑Nitrogen monoxide + 9CO2↑Carbon dioxide + 15H2OWater

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) carbonate and nitric acid under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeCO3Iron(II) carbonate9
Reducing
Oxidizable
HNO3Nitric acid6
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion24
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate1
Oxidized
–
Fe3+Iron(III) ion8
Oxidized
–
NONitrogen monoxide3
Reduced
–
CO2Carbon dioxide9
–
–
H2OWater15
–
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) carbonate and nitric acid under acidic condition
◆
ΔrG−554.9 kJ/mol
K1.64 × 1097
pK−97.21
9FeCO3Crystalline solidsiderite + 6HNO3Ionized aqueous solution + 24H+Un-ionized aqueous solution
⟶
Fe(NO3)3Ionized aqueous solution + 8Fe3+Un-ionized aqueous solution + 3NO↑Gas + 9CO2↑Gas + 15H2OLiquid
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
−707.7−554.9−513.7–
per 1 mol of
−78.63−61.66−57.08–
per 1 mol of
−118.0−92.48−85.62–
per 1 mol of
Hydrogen ion
−29.49−23.12−21.40–
per 1 mol of
−707.7−554.9−513.7–
per 1 mol of
Iron(III) ion
−88.46−69.36−64.21–
per 1 mol of
−235.9−185.0−171.2–
per 1 mol of
−78.63−61.66−57.08–
per 1 mol of
−47.18−36.99−34.25–

Changes in standard condition (2)

Reaction of iron(II) carbonate and nitric acid under acidic condition
◆
ΔrG−479.5 kJ/mol
K1.01 × 1084
pK−84.00
9FeCO3Crystalline solidsiderite + 6HNO3Ionized aqueous solution + 24H+Un-ionized aqueous solution
⟶
Fe(NO3)3Ionized aqueous solution + 8Fe3+Un-ionized aqueous solution + 3NO↑Gas + 9CO2↑Un-ionized aqueous solution + 15H2OLiquid
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
−890.3−479.5−1379.0–
per 1 mol of
−98.92−53.28−153.22–
per 1 mol of
−148.4−79.92−229.83–
per 1 mol of
Hydrogen ion
−37.10−19.98−57.458–
per 1 mol of
−890.3−479.5−1379.0–
per 1 mol of
Iron(III) ion
−111.3−59.94−172.38–
per 1 mol of
−296.8−159.8−459.67–
per 1 mol of
−98.92−53.28−153.22–
per 1 mol of
−59.35−31.97−91.933–

Changes in standard condition (3)

Reaction of iron(II) carbonate and nitric acid under acidic condition
9FeCO3Crystalline solidsiderite + 6HNO3Ionized aqueous solution + 24H+Un-ionized aqueous solution
⟶
Fe(NO3)3Aqueous solution + 8Fe3+Un-ionized aqueous solution + 3NO↑Gas + 9CO2↑Gas + 15H2OLiquid
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
−711.9–––
per 1 mol of
−79.10–––
per 1 mol of
−118.6–––
per 1 mol of
Hydrogen ion
−29.66–––
per 1 mol of
−711.9–––
per 1 mol of
Iron(III) ion
−88.99–––
per 1 mol of
−237.3–––
per 1 mol of
−79.10–––
per 1 mol of
−47.46–––

Changes in standard condition (4)

Reaction of iron(II) carbonate and nitric acid under acidic condition
9FeCO3Crystalline solidsiderite + 6HNO3Ionized aqueous solution + 24H+Un-ionized aqueous solution
⟶
Fe(NO3)3Aqueous solution + 8Fe3+Un-ionized aqueous solution + 3NO↑Gas + 9CO2↑Un-ionized aqueous solution + 15H2OLiquid
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
−894.5–––
per 1 mol of
−99.39–––
per 1 mol of
−149.1–––
per 1 mol of
Hydrogen ion
−37.27–––
per 1 mol of
−894.5–––
per 1 mol of
Iron(III) ion
−111.8–––
per 1 mol of
−298.2–––
per 1 mol of
−99.39–––
per 1 mol of
−59.63–––

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
FeCO3 (cr)
siderite
-740.57[1]-666.67[1]92.9[1]82.13[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, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (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]–
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[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)