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2K3[Fe(CN)6] + 24HNO3 → 3K2CO3 + 15N2O↑ + 2Fe(NO3)3 + 9CO2↑ + 12H2O

2K₃[Fe(CN)₆] + 24HNO₃ → 3K₂CO₃ + 15N₂O↑ + 2Fe(NO₃)₃ + 9CO₂↑ + 12H₂O

Last updated: May 12, 2022

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Potassium hexacyanidoferrate(III) + 24HNO₃Nitric acid
⟶
3K₂CO₃Potassium carbonate + 15N₂O↑Dinitrotgen monoxide + 2Fe(NO₃)₃Iron(III) nitrate + 9CO₂↑Carbon dioxide + 12H₂OWater

The reaction of potassium hexacyanidoferrate(III) and nitric acid yields potassium carbonate, dinitrotgen monoxide, iron(III) nitrate, carbon dioxide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of reducing species and oxidizing species

Table of contents

Reaction data

Chemical equation

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Potassium hexacyanidoferrate(III) + 24HNO₃Nitric acid
⟶
3K₂CO₃Potassium carbonate + 15N₂O↑Dinitrotgen monoxide + 2Fe(NO₃)₃Iron(III) nitrate + 9CO₂↑Carbon dioxide + 12H₂OWater

General equation

Reaction of reducing species and oxidizing species: Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium hexacyanidoferrate(III) and nitric acid

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
K₃[Fe(CN)₆]	Potassium hexacyanidoferrate(III)	2	Reducing	Reducing
HNO₃	Nitric acid	24	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
K₂CO₃	Potassium carbonate	3	Oxidized	–
N₂O	Dinitrotgen monoxide	15	Redoxed product	–
Fe(NO₃)₃	Iron(III) nitrate	2	–	–
CO₂	Carbon dioxide	9	Oxidized	–
H₂O	Water	12	–	–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hexacyanidoferrate(III) and nitric acid ◆ Δ_rG −5880.7 kJ/mol K 1.80 × 10¹⁰³⁰ pK −1030.25: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Gas + 2Fe(NO₃)₃Ionized aqueous solution + 9CO₂↑Gas + 12H₂OLiquid

	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	−5260.5	−5880.7	2082.2	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2630.3	−2940.3	1041.1	–
per 1 mol of Nitric acid	−219.19	−245.03	86.758	–
per 1 mol of Potassium carbonate	−1753.5	−1960.2	694.07	–
per 1 mol of Dinitrotgen monoxide	−350.70	−392.05	138.81	–
per 1 mol of Iron(III) nitrate	−2630.3	−2940.3	1041.1	–
per 1 mol of Carbon dioxide	−584.50	−653.41	231.36	–
per 1 mol of Water	−438.38	−490.06	173.52	–

Changes in aqueous solution (2)

Reaction of potassium hexacyanidoferrate(III) and nitric acid ◆ Δ_rG −5805.2 kJ/mol K 1.06 × 10¹⁰¹⁷ pK −1017.03: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Gas + 2Fe(NO₃)₃Ionized aqueous solution + 9CO₂↑Un-ionized aqueous solution + 12H₂OLiquid

	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	−5443.1	−5805.2	1217.0	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2721.6	−2902.6	608.50	–
per 1 mol of Nitric acid	−226.80	−241.88	50.708	–
per 1 mol of Potassium carbonate	−1814.4	−1935.1	405.67	–
per 1 mol of Dinitrotgen monoxide	−362.87	−387.01	81.133	–
per 1 mol of Iron(III) nitrate	−2721.6	−2902.6	608.50	–
per 1 mol of Carbon dioxide	−604.79	−645.02	135.22	–
per 1 mol of Water	−453.59	−483.77	101.42	–

Changes in aqueous solution (3)

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Gas + 2Fe(NO₃)₃Aqueous solution + 9CO₂↑Gas + 12H₂OLiquid

	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	−5268.9	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2634.4	–	–	–
per 1 mol of Nitric acid	−219.54	–	–	–
per 1 mol of Potassium carbonate	−1756.3	–	–	–
per 1 mol of Dinitrotgen monoxide	−351.26	–	–	–
per 1 mol of Iron(III) nitrate	−2634.4	–	–	–
per 1 mol of Carbon dioxide	−585.43	–	–	–
per 1 mol of Water	−439.07	–	–	–

Changes in aqueous solution (4)

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Gas + 2Fe(NO₃)₃Aqueous solution + 9CO₂↑Un-ionized aqueous solution + 12H₂OLiquid

	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	−5451.5	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2725.8	–	–	–
per 1 mol of Nitric acid	−227.15	–	–	–
per 1 mol of Potassium carbonate	−1817.2	–	–	–
per 1 mol of Dinitrotgen monoxide	−363.43	–	–	–
per 1 mol of Iron(III) nitrate	−2725.8	–	–	–
per 1 mol of Carbon dioxide	−605.72	–	–	–
per 1 mol of Water	−454.29	–	–	–

Changes in aqueous solution (5)

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Aqueous solution + 2Fe(NO₃)₃Ionized aqueous solution + 9CO₂↑Gas + 12H₂OLiquid

	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	−5649.7	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2824.8	–	–	–
per 1 mol of Nitric acid	−235.40	–	–	–
per 1 mol of Potassium carbonate	−1883.2	–	–	–
per 1 mol of Dinitrotgen monoxide	−376.65	–	–	–
per 1 mol of Iron(III) nitrate	−2824.8	–	–	–
per 1 mol of Carbon dioxide	−627.74	–	–	–
per 1 mol of Water	−470.81	–	–	–

Changes in aqueous solution (6)

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Aqueous solution + 2Fe(NO₃)₃Ionized aqueous solution + 9CO₂↑Un-ionized aqueous solution + 12H₂OLiquid

	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	−5832.3	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2916.2	–	–	–
per 1 mol of Nitric acid	−243.01	–	–	–
per 1 mol of Potassium carbonate	−1944.1	–	–	–
per 1 mol of Dinitrotgen monoxide	−388.82	–	–	–
per 1 mol of Iron(III) nitrate	−2916.2	–	–	–
per 1 mol of Carbon dioxide	−648.03	–	–	–
per 1 mol of Water	−486.03	–	–	–

Changes in aqueous solution (7)

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Aqueous solution + 2Fe(NO₃)₃Aqueous solution + 9CO₂↑Gas + 12H₂OLiquid

	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	−5658.1	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2829.1	–	–	–
per 1 mol of Nitric acid	−235.75	–	–	–
per 1 mol of Potassium carbonate	−1886.0	–	–	–
per 1 mol of Dinitrotgen monoxide	−377.21	–	–	–
per 1 mol of Iron(III) nitrate	−2829.1	–	–	–
per 1 mol of Carbon dioxide	−628.68	–	–	–
per 1 mol of Water	−471.51	–	–	–

Changes in aqueous solution (8)

Reaction of potassium hexacyanidoferrate(III) and nitric acid: 2K₃[Fe(CN)₆]Ionized aqueous solution + 24HNO₃Ionized aqueous solution
⟶
3K₂CO₃Ionized aqueous solution + 15N₂O↑Aqueous solution + 2Fe(NO₃)₃Aqueous solution + 9CO₂↑Un-ionized aqueous solution + 12H₂OLiquid

	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	−5840.7	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	−2920.3	–	–	–
per 1 mol of Nitric acid	−243.36	–	–	–
per 1 mol of Potassium carbonate	−1946.9	–	–	–
per 1 mol of Dinitrotgen monoxide	−389.38	–	–	–
per 1 mol of Iron(III) nitrate	−2920.3	–	–	–
per 1 mol of Carbon dioxide	−648.97	–	–	–
per 1 mol of Water	−486.72	–	–	–

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
K₃[Fe(CN)₆] (cr)	-249.8^[1]	-129.6^[1]	426.06^[1]	–
K₃[Fe(CN)₆] (ai)	-195.4^[1]	-120.4^[1]	577.8^[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, (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
K₂CO₃ (cr)	-1151.02^[1]	-1063.5^[1]	155.52^[1]	114.43^[1]
K₂CO₃ (ai)	-1181.90^[1]	-1094.36^[1]	148.1^[1]	–
K₂CO₃ (cr) 1.5 hydrate	-1609.2^[1]	-1432.5^[1]	203.3^[1]	–
N₂O (g)	82.05^[1]	104.20^[1]	219.85^[1]	38.45^[1]
N₂O (aq)	56.1^[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]	–	–	–
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]

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

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