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14FeF2 + 44HNO3 + H^+ 🔥→ 14Fe(NO3)3 + N2H5^+ + 28HF↑ + 6H2O

14FeF₂ + 44HNO₃ + H⁺ 🔥→ 14Fe(NO₃)₃ + N₂H₅⁺ + 28HF↑ + 6H₂O

Last updated: June 13, 2022

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Iron(II) fluoride + 44HNO₃Nitric acid + H⁺Hydrogen ion
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14Fe(NO₃)₃Iron(III) nitrate + N₂H₅⁺Hydrazinium ion + 28HF↑Hydrogen fluoride + 6H₂OWater

The reaction of iron(II) fluoride, nitric acid, and hydrogen ion yields iron(III) nitrate, hydrazinium ion, 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 under acidic condition

Table of contents

Reaction data

Chemical equation

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Iron(II) fluoride + 44HNO₃Nitric acid + H⁺Hydrogen ion
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14Fe(NO₃)₃Iron(III) nitrate + N₂H₅⁺Hydrazinium ion + 28HF↑Hydrogen fluoride + 6H₂OWater

General equation

Reaction of oxidizable species and oxidizing species under acidic condition: Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H⁺Non-redox agent
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ProductOxidation product + ProductReduction product + H₂ONon-redox product

Oxidation state of each atom

Reaction of iron(II) fluoride and nitric acid under acidic condition

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
FeF₂	Iron(II) fluoride	14	Reducing	Oxidizable
HNO₃	Nitric acid	44	Oxidizing	Oxidizing under acidic condition
H⁺	Hydrogen ion	1	–	Hydrogen ion

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Fe(NO₃)₃	Iron(III) nitrate	14	Oxidized	–
N₂H₅⁺	Hydrazinium ion	1	Reduced	–
HF	Hydrogen fluoride	28	–	–
H₂O	Water	6	–	Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Gas + 6H₂OLiquid

	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	853.6	–	–	–
per 1 mol of Iron(II) fluoride	60.97	–	–	–
per 1 mol of Nitric acid	19.40	–	–	–
per 1 mol of Hydrogen ion	853.6	–	–	–
per 1 mol of Iron(III) nitrate	60.97	–	–	–
per 1 mol of Hydrazinium ion	853.6	–	–	–
per 1 mol of Hydrogen fluoride	30.49	–	–	–
per 1 mol of Water	142.3	–	–	–

Changes in standard condition (2)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−517.9	–	–	–
per 1 mol of Iron(II) fluoride	−36.99	–	–	–
per 1 mol of Nitric acid	−11.77	–	–	–
per 1 mol of Hydrogen ion	−517.9	–	–	–
per 1 mol of Iron(III) nitrate	−36.99	–	–	–
per 1 mol of Hydrazinium ion	−517.9	–	–	–
per 1 mol of Hydrogen fluoride	−18.50	–	–	–
per 1 mol of Water	−86.32	–	–	–

Changes in standard condition (3)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−517.9	–	–	–
per 1 mol of Iron(II) fluoride	−36.99	–	–	–
per 1 mol of Nitric acid	−11.77	–	–	–
per 1 mol of Hydrogen ion	−517.9	–	–	–
per 1 mol of Iron(III) nitrate	−36.99	–	–	–
per 1 mol of Hydrazinium ion	−517.9	–	–	–
per 1 mol of Hydrogen fluoride	−18.50	–	–	–
per 1 mol of Water	−86.32	–	–	–

Changes in standard condition (4)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Gas + 6H₂OLiquid

	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	794.8	–	–	–
per 1 mol of Iron(II) fluoride	56.77	–	–	–
per 1 mol of Nitric acid	18.06	–	–	–
per 1 mol of Hydrogen ion	794.8	–	–	–
per 1 mol of Iron(III) nitrate	56.77	–	–	–
per 1 mol of Hydrazinium ion	794.8	–	–	–
per 1 mol of Hydrogen fluoride	28.39	–	–	–
per 1 mol of Water	132.5	–	–	–

Changes in standard condition (5)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−576.7	–	–	–
per 1 mol of Iron(II) fluoride	−41.19	–	–	–
per 1 mol of Nitric acid	−13.11	–	–	–
per 1 mol of Hydrogen ion	−576.7	–	–	–
per 1 mol of Iron(III) nitrate	−41.19	–	–	–
per 1 mol of Hydrazinium ion	−576.7	–	–	–
per 1 mol of Hydrogen fluoride	−20.60	–	–	–
per 1 mol of Water	−96.12	–	–	–

Changes in standard condition (6)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−576.7	–	–	–
per 1 mol of Iron(II) fluoride	−41.19	–	–	–
per 1 mol of Nitric acid	−13.11	–	–	–
per 1 mol of Hydrogen ion	−576.7	–	–	–
per 1 mol of Iron(III) nitrate	−41.19	–	–	–
per 1 mol of Hydrazinium ion	−576.7	–	–	–
per 1 mol of Hydrogen fluoride	−20.60	–	–	–
per 1 mol of Water	−96.12	–	–	–

Changes in standard condition (7)

Reaction of iron(II) fluoride and nitric acid under acidic condition ◆ Δ_rG 529.3 kJ/mol K 0.19 × 10⁻⁹² pK 92.73: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Gas + 6H₂OLiquid

	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	379.0	529.3	−496	–
per 1 mol of Iron(II) fluoride	27.07	37.81	−35.4	–
per 1 mol of Nitric acid	8.614	12.03	−11.3	–
per 1 mol of Hydrogen ion	379.0	529.3	−496	–
per 1 mol of Iron(III) nitrate	27.07	37.81	−35.4	–
per 1 mol of Hydrazinium ion	379.0	529.3	−496	–
per 1 mol of Hydrogen fluoride	13.54	18.90	−17.7	–
per 1 mol of Water	63.17	88.22	−82.7	–

Changes in standard condition (8)

Reaction of iron(II) fluoride and nitric acid under acidic condition ◆ Δ_rG −132.0 kJ/mol K 1.33 × 10²³ pK −23.13: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−992.5	−132.0	−2878	–
per 1 mol of Iron(II) fluoride	−70.89	−9.429	−205.6	–
per 1 mol of Nitric acid	−22.56	−3.000	−65.41	–
per 1 mol of Hydrogen ion	−992.5	−132.0	−2878	–
per 1 mol of Iron(III) nitrate	−70.89	−9.429	−205.6	–
per 1 mol of Hydrazinium ion	−992.5	−132.0	−2878	–
per 1 mol of Hydrogen fluoride	−35.45	−4.714	−102.8	–
per 1 mol of Water	−165.4	−22.00	−479.7	–

Changes in standard condition (9)

Reaction of iron(II) fluoride and nitric acid under acidic condition ◆ Δ_rG −132.0 kJ/mol K 1.33 × 10²³ pK −23.13: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
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⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−992.5	−132.0	−2878	–
per 1 mol of Iron(II) fluoride	−70.89	−9.429	−205.6	–
per 1 mol of Nitric acid	−22.56	−3.000	−65.41	–
per 1 mol of Hydrogen ion	−992.5	−132.0	−2878	–
per 1 mol of Iron(III) nitrate	−70.89	−9.429	−205.6	–
per 1 mol of Hydrazinium ion	−992.5	−132.0	−2878	–
per 1 mol of Hydrogen fluoride	−35.45	−4.714	−102.8	–
per 1 mol of Water	−165.4	−22.00	−479.7	–

Changes in standard condition (10)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Gas + 6H₂OLiquid

	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	320.2	–	–	–
per 1 mol of Iron(II) fluoride	22.87	–	–	–
per 1 mol of Nitric acid	7.277	–	–	–
per 1 mol of Hydrogen ion	320.2	–	–	–
per 1 mol of Iron(III) nitrate	22.87	–	–	–
per 1 mol of Hydrazinium ion	320.2	–	–	–
per 1 mol of Hydrogen fluoride	11.44	–	–	–
per 1 mol of Water	53.37	–	–	–

Changes in standard condition (11)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−1051.3	–	–	–
per 1 mol of Iron(II) fluoride	−75.093	–	–	–
per 1 mol of Nitric acid	−23.893	–	–	–
per 1 mol of Hydrogen ion	−1051.3	–	–	–
per 1 mol of Iron(III) nitrate	−75.093	–	–	–
per 1 mol of Hydrazinium ion	−1051.3	–	–	–
per 1 mol of Hydrogen fluoride	−37.546	–	–	–
per 1 mol of Water	−175.22	–	–	–

Changes in standard condition (12)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Un-ionized aqueous solution + 6H₂OLiquid

	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	−1051.3	–	–	–
per 1 mol of Iron(II) fluoride	−75.093	–	–	–
per 1 mol of Nitric acid	−23.893	–	–	–
per 1 mol of Hydrogen ion	−1051.3	–	–	–
per 1 mol of Iron(III) nitrate	−75.093	–	–	–
per 1 mol of Hydrazinium ion	−1051.3	–	–	–
per 1 mol of Hydrogen fluoride	−37.546	–	–	–
per 1 mol of Water	−175.22	–	–	–

Changes in standard condition (13)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Ionized aqueous solution + 6H₂OLiquid

	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	−869.3	–	–	–
per 1 mol of Iron(II) fluoride	−62.09	–	–	–
per 1 mol of Nitric acid	−19.76	–	–	–
per 1 mol of Hydrogen ion	−869.3	–	–	–
per 1 mol of Iron(III) nitrate	−62.09	–	–	–
per 1 mol of Hydrazinium ion	−869.3	–	–	–
per 1 mol of Hydrogen fluoride	−31.05	–	–	–
per 1 mol of Water	−144.9	–	–	–

Changes in standard condition (14)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Aqueous solution + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Ionized aqueous solution + 6H₂OLiquid

	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	−928.1	–	–	–
per 1 mol of Iron(II) fluoride	−66.29	–	–	–
per 1 mol of Nitric acid	−21.09	–	–	–
per 1 mol of Hydrogen ion	−928.1	–	–	–
per 1 mol of Iron(III) nitrate	−66.29	–	–	–
per 1 mol of Hydrazinium ion	−928.1	–	–	–
per 1 mol of Hydrogen fluoride	−33.15	–	–	–
per 1 mol of Water	−154.7	–	–	–

Changes in standard condition (15)

Reaction of iron(II) fluoride and nitric acid under acidic condition ◆ Δ_rG 372.8 kJ/mol K 0.49 × 10⁻⁶⁵ pK 65.31: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Ionized aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Ionized aqueous solution + 6H₂OLiquid

	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	−1343.9	372.8	−5748	–
per 1 mol of Iron(II) fluoride	−95.993	26.63	−410.6	–
per 1 mol of Nitric acid	−30.543	8.473	−130.6	–
per 1 mol of Hydrogen ion	−1343.9	372.8	−5748	–
per 1 mol of Iron(III) nitrate	−95.993	26.63	−410.6	–
per 1 mol of Hydrazinium ion	−1343.9	372.8	−5748	–
per 1 mol of Hydrogen fluoride	−47.996	13.31	−205.3	–
per 1 mol of Water	−223.98	62.13	−958.0	–

Changes in standard condition (16)

Reaction of iron(II) fluoride and nitric acid under acidic condition: 14FeF₂Crystalline solid + 44HNO₃Ionized aqueous solution + H⁺Un-ionized aqueous solution
🔥
⟶
14Fe(NO₃)₃Aqueous solution + N₂H₅⁺Un-ionized aqueous solution + 28HF↑Ionized aqueous solution + 6H₂OLiquid

	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	−1402.7	–	–	–
per 1 mol of Iron(II) fluoride	−100.19	–	–	–
per 1 mol of Nitric acid	−31.880	–	–	–
per 1 mol of Hydrogen ion	−1402.7	–	–	–
per 1 mol of Iron(III) nitrate	−100.19	–	–	–
per 1 mol of Hydrazinium ion	−1402.7	–	–	–
per 1 mol of Hydrogen fluoride	−50.096	–	–	–
per 1 mol of Water	−233.78	–	–	–

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]
H⁺ (g)	1536.202^[1]	–	–	–
H⁺ (ao)	0^[1]	0^[1]	0^[1]	0^[1]

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

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]	–	–	–
N₂H₅⁺ (ao)	-7.5^[1]	82.5^[1]	151^[1]	70.3^[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, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas

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	529.3 kJ/mol
K	0.19 × 10⁻⁹²
pK	92.73

Δ_rG	−132.0 kJ/mol
K	1.33 × 10²³
pK	−23.13

Δ_rG	−132.0 kJ/mol
K	1.33 × 10²³
pK	−23.13

Δ_rG	372.8 kJ/mol
K	0.49 × 10⁻⁶⁵
pK	65.31

14FeF2 + 44HNO3 + H+ 🔥→ 14Fe(NO3)3 + N2H5+ + 28HF↑ + 6H2O

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition (1)

Changes in standard condition (2)

Changes in standard condition (3)

Changes in standard condition (4)

Changes in standard condition (5)

Changes in standard condition (6)

Changes in standard condition (7)

Changes in standard condition (8)

Changes in standard condition (9)

Changes in standard condition (10)

Changes in standard condition (11)

Changes in standard condition (12)

Changes in standard condition (13)

Changes in standard condition (14)

Changes in standard condition (15)

Changes in standard condition (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

14FeF₂ + 44HNO₃ + H⁺ 🔥→ 14Fe(NO₃)₃ + N₂H₅⁺ + 28HF↑ + 6H₂O