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8FeF2 + 26HNO3 🔥→ 8Fe(NO3)3 + NH4NO3 + 16HF↑ + 3H2O

8FeF₂ + 26HNO₃ 🔥→ 8Fe(NO₃)₃ + NH₄NO₃ + 16HF↑ + 3H₂O

Last updated: June 13, 2022

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Iron(II) fluoride + 26HNO₃Nitric acid
🔥
⟶
8Fe(NO₃)₃Iron(III) nitrate + NH₄NO₃Ammonium nitrate + 16HF↑Hydrogen fluoride + 3H₂OWater

The reaction of iron(II) fluoride and nitric acid yields iron(III) nitrate, ammonium nitrate, hydrogen fluoride, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of oxidizable species and oxidizing species

Table of contents

Reaction data

Chemical equation

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Iron(II) fluoride + 26HNO₃Nitric acid
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⟶
8Fe(NO₃)₃Iron(III) nitrate + NH₄NO₃Ammonium nitrate + 16HF↑Hydrogen fluoride + 3H₂OWater

General equation

Reaction of oxidizable species and oxidizing species: Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of iron(II) fluoride and nitric acid

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
FeF₂	Iron(II) fluoride	8	Reducing	Oxidizable
HNO₃	Nitric acid	26	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Fe(NO₃)₃	Iron(III) nitrate	8	Oxidized	–
NH₄NO₃	Ammonium nitrate	1	Reduced	–
HF	Hydrogen fluoride	16	–	–
H₂O	Water	3	–	–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Gas + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	452.4	–	–	–
per 1 mol of Iron(II) fluoride	56.55	–	–	–
per 1 mol of Nitric acid	17.40	–	–	–
per 1 mol of Iron(III) nitrate	56.55	–	–	–
per 1 mol of Ammonium nitrate	452.4	–	–	–
per 1 mol of Hydrogen fluoride	28.27	–	–	–
per 1 mol of Water	150.8	–	–	–

Changes in aqueous solution (2)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−331.3	–	–	–
per 1 mol of Iron(II) fluoride	−41.41	–	–	–
per 1 mol of Nitric acid	−12.74	–	–	–
per 1 mol of Iron(III) nitrate	−41.41	–	–	–
per 1 mol of Ammonium nitrate	−331.3	–	–	–
per 1 mol of Hydrogen fluoride	−20.71	–	–	–
per 1 mol of Water	−110.4	–	–	–

Changes in aqueous solution (3)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−331.3	–	–	–
per 1 mol of Iron(II) fluoride	−41.41	–	–	–
per 1 mol of Nitric acid	−12.74	–	–	–
per 1 mol of Iron(III) nitrate	−41.41	–	–	–
per 1 mol of Ammonium nitrate	−331.3	–	–	–
per 1 mol of Hydrogen fluoride	−20.71	–	–	–
per 1 mol of Water	−110.4	–	–	–

Changes in aqueous solution (4)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Gas + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	418.8	–	–	–
per 1 mol of Iron(II) fluoride	52.35	–	–	–
per 1 mol of Nitric acid	16.11	–	–	–
per 1 mol of Iron(III) nitrate	52.35	–	–	–
per 1 mol of Ammonium nitrate	418.8	–	–	–
per 1 mol of Hydrogen fluoride	26.18	–	–	–
per 1 mol of Water	139.6	–	–	–

Changes in aqueous solution (5)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−364.9	–	–	–
per 1 mol of Iron(II) fluoride	−45.61	–	–	–
per 1 mol of Nitric acid	−14.03	–	–	–
per 1 mol of Iron(III) nitrate	−45.61	–	–	–
per 1 mol of Ammonium nitrate	−364.9	–	–	–
per 1 mol of Hydrogen fluoride	−22.81	–	–	–
per 1 mol of Water	−121.6	–	–	–

Changes in aqueous solution (6)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−364.9	–	–	–
per 1 mol of Iron(II) fluoride	−45.61	–	–	–
per 1 mol of Nitric acid	−14.03	–	–	–
per 1 mol of Iron(III) nitrate	−45.61	–	–	–
per 1 mol of Ammonium nitrate	−364.9	–	–	–
per 1 mol of Hydrogen fluoride	−22.81	–	–	–
per 1 mol of Water	−121.6	–	–	–

Changes in aqueous solution (7)

Reaction of iron(II) fluoride and nitric acid ◆ Δ_rG 261.8 kJ/mol K 0.14 × 10⁻⁴⁵ pK 45.87: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Gas + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	181.2	261.8	−265.1	–
per 1 mol of Iron(II) fluoride	22.65	32.73	−33.14	–
per 1 mol of Nitric acid	6.969	10.07	−10.20	–
per 1 mol of Iron(III) nitrate	22.65	32.73	−33.14	–
per 1 mol of Ammonium nitrate	181.2	261.8	−265.1	–
per 1 mol of Hydrogen fluoride	11.32	16.36	−16.57	–
per 1 mol of Water	60.40	87.27	−88.37	–

Changes in aqueous solution (8)

Reaction of iron(II) fluoride and nitric acid ◆ Δ_rG −116.2 kJ/mol K 2.28 × 10²⁰ pK −20.36: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−602.5	−116.2	−1626.4	–
per 1 mol of Iron(II) fluoride	−75.31	−14.53	−203.30	–
per 1 mol of Nitric acid	−23.17	−4.469	−62.554	–
per 1 mol of Iron(III) nitrate	−75.31	−14.53	−203.30	–
per 1 mol of Ammonium nitrate	−602.5	−116.2	−1626.4	–
per 1 mol of Hydrogen fluoride	−37.66	−7.263	−101.65	–
per 1 mol of Water	−200.8	−38.73	−542.13	–

Changes in aqueous solution (9)

Reaction of iron(II) fluoride and nitric acid ◆ Δ_rG −116.2 kJ/mol K 2.28 × 10²⁰ pK −20.36: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−602.5	−116.2	−1626.4	–
per 1 mol of Iron(II) fluoride	−75.31	−14.53	−203.30	–
per 1 mol of Nitric acid	−23.17	−4.469	−62.554	–
per 1 mol of Iron(III) nitrate	−75.31	−14.53	−203.30	–
per 1 mol of Ammonium nitrate	−602.5	−116.2	−1626.4	–
per 1 mol of Hydrogen fluoride	−37.66	−7.263	−101.65	–
per 1 mol of Water	−200.8	−38.73	−542.13	–

Changes in aqueous solution (10)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Gas + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	147.6	–	–	–
per 1 mol of Iron(II) fluoride	18.45	–	–	–
per 1 mol of Nitric acid	5.677	–	–	–
per 1 mol of Iron(III) nitrate	18.45	–	–	–
per 1 mol of Ammonium nitrate	147.6	–	–	–
per 1 mol of Hydrogen fluoride	9.225	–	–	–
per 1 mol of Water	49.20	–	–	–

Changes in aqueous solution (11)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−636.1	–	–	–
per 1 mol of Iron(II) fluoride	−79.51	–	–	–
per 1 mol of Nitric acid	−24.47	–	–	–
per 1 mol of Iron(III) nitrate	−79.51	–	–	–
per 1 mol of Ammonium nitrate	−636.1	–	–	–
per 1 mol of Hydrogen fluoride	−39.76	–	–	–
per 1 mol of Water	−212.0	–	–	–

Changes in aqueous solution (12)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Un-ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−636.1	–	–	–
per 1 mol of Iron(II) fluoride	−79.51	–	–	–
per 1 mol of Nitric acid	−24.47	–	–	–
per 1 mol of Iron(III) nitrate	−79.51	–	–	–
per 1 mol of Ammonium nitrate	−636.1	–	–	–
per 1 mol of Hydrogen fluoride	−39.76	–	–	–
per 1 mol of Water	−212.0	–	–	–

Changes in aqueous solution (13)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−532.1	–	–	–
per 1 mol of Iron(II) fluoride	−66.51	–	–	–
per 1 mol of Nitric acid	−20.47	–	–	–
per 1 mol of Iron(III) nitrate	−66.51	–	–	–
per 1 mol of Ammonium nitrate	−532.1	–	–	–
per 1 mol of Hydrogen fluoride	−33.26	–	–	–
per 1 mol of Water	−177.4	–	–	–

Changes in aqueous solution (14)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Aqueous solution + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−565.7	–	–	–
per 1 mol of Iron(II) fluoride	−70.71	–	–	–
per 1 mol of Nitric acid	−21.76	–	–	–
per 1 mol of Iron(III) nitrate	−70.71	–	–	–
per 1 mol of Ammonium nitrate	−565.7	–	–	–
per 1 mol of Hydrogen fluoride	−35.36	–	–	–
per 1 mol of Water	−188.6	–	–	–

Changes in aqueous solution (15)

Reaction of iron(II) fluoride and nitric acid ◆ Δ_rG 172.3 kJ/mol K 0.65 × 10⁻³⁰ pK 30.19: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Ionized aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−803.3	172.3	−3266.4	–
per 1 mol of Iron(II) fluoride	−100.4	21.54	−408.30	–
per 1 mol of Nitric acid	−30.90	6.627	−125.63	–
per 1 mol of Iron(III) nitrate	−100.4	21.54	−408.30	–
per 1 mol of Ammonium nitrate	−803.3	172.3	−3266.4	–
per 1 mol of Hydrogen fluoride	−50.21	10.77	−204.15	–
per 1 mol of Water	−267.8	57.43	−1088.8	–

Changes in aqueous solution (16)

Reaction of iron(II) fluoride and nitric acid: 8FeF₂Crystalline solid + 26HNO₃Ionized aqueous solution
🔥
⟶
8Fe(NO₃)₃Aqueous solution + NH₄NO₃Ionized aqueous solution + 16HF↑Ionized aqueous solution + 3H₂OLiquid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−836.9	–	–	–
per 1 mol of Iron(II) fluoride	−104.6	–	–	–
per 1 mol of Nitric acid	−32.19	–	–	–
per 1 mol of Iron(III) nitrate	−104.6	–	–	–
per 1 mol of Ammonium nitrate	−836.9	–	–	–
per 1 mol of Hydrogen fluoride	−52.31	–	–	–
per 1 mol of Water	−279.0	–	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
FeF₂ (cr)	-711.3^[1]	-668.6^[1]	86.99^[1]	68.12^[1]
FeF₂ (ai)	-754.4^[1]	-636.48^[1]	-165.3^[1]	–
FeF₂ (aq)	-745.2^[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]

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (g):Gas

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° 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]	–	–	–
NH₄NO₃ (cr)	-365.56^[1]	-183.87^[1]	151.08^[1]	139.3^[1]
NH₄NO₃ (ai)	-339.87^[1]	-190.56^[1]	259.8^[1]	-6.7^[1]
HF (l) x denotes undetermined zero point entropy	-299.78^[1]	–	75.40+x^[1]	–
HF (g)	-271.1^[1]	-273.2^[1]	173.779^[1]	29.133^[1]
HF (ai)	-332.63^[1]	-278.79^[1]	-13.8^[1]	-106.7^[1]
HF (ao)	-320.08^[1]	-296.82^[1]	88.7^[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, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

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
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list

Δ_rG	261.8 kJ/mol
K	0.14 × 10⁻⁴⁵
pK	45.87

Δ_rG	−116.2 kJ/mol
K	2.28 × 10²⁰
pK	−20.36

Δ_rG	−116.2 kJ/mol
K	2.28 × 10²⁰
pK	−20.36

Δ_rG	172.3 kJ/mol
K	0.65 × 10⁻³⁰
pK	30.19

8FeF2 + 26HNO3 🔥→ 8Fe(NO3)3 + NH4NO3 + 16HF↑ + 3H2O

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in aqueous solution (1)

Changes in aqueous solution (2)

Changes in aqueous solution (3)

Changes in aqueous solution (4)

Changes in aqueous solution (5)

Changes in aqueous solution (6)

Changes in aqueous solution (7)

Changes in aqueous solution (8)

Changes in aqueous solution (9)

Changes in aqueous solution (10)

Changes in aqueous solution (11)

Changes in aqueous solution (12)

Changes in aqueous solution (13)

Changes in aqueous solution (14)

Changes in aqueous solution (15)

Changes in aqueous solution (16)

Thermodynamic data of reactants

Thermodynamic data of products

References

List of references

Related reactions

Reactions with same reactants

Related categories

Type of reaction

General equation

Reactant

Product

8FeF₂ + 26HNO₃ 🔥→ 8Fe(NO₃)₃ + NH₄NO₃ + 16HF↑ + 3H₂O