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2K3[Fe(CN)6] + 26Fe2O3 🔥→ 6KCN + 3N2↑ + 18Fe3O4 + 6CO↑

2K₃[Fe(CN)₆] + 26Fe₂O₃ 🔥→ 6KCN + 3N₂↑ + 18Fe₃O₄ + 6CO↑

Last updated: June 13, 2022

Reaction of potassium hexacyanidoferrate(III) and iron(III) oxide: 2K₃[Fe(CN)₆]Potassium hexacyanidoferrate(III) + 26Fe₂O₃Iron(III) oxide
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6KCNPotassium cyanide + 3N₂↑Nitrogen + 18Fe₃O₄Iron(II,III) oxide + 6CO↑Carbon monoxide

The reaction of potassium hexacyanidoferrate(III) and iron(III) oxide yields potassium cyanide, nitrogen, iron(II,III) oxide, and carbon monoxide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of reducing species and reducible species

Table of contents

Reaction data

Chemical equation

Reaction of potassium hexacyanidoferrate(III) and iron(III) oxide: 2K₃[Fe(CN)₆]Potassium hexacyanidoferrate(III) + 26Fe₂O₃Iron(III) oxide
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6KCNPotassium cyanide + 3N₂↑Nitrogen + 18Fe₃O₄Iron(II,III) oxide + 6CO↑Carbon monoxide

General equation

Reaction of reducing species and reducible species: Reducing speciesReducing agent + Reducible speciesOxidizing agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium hexacyanidoferrate(III) and iron(III) oxide

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
K₃[Fe(CN)₆]	Potassium hexacyanidoferrate(III)	2	Reducing	Reducing
Fe₂O₃	Iron(III) oxide	26	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
KCN	Potassium cyanide	6	–	–
N₂	Nitrogen	3	Oxidized	–
Fe₃O₄	Iron(II,III) oxide	18	Reduced	–
CO	Carbon monoxide	6	–	–

Thermodynamic changes

Changes in standard condition

Reaction of potassium hexacyanidoferrate(III) and iron(III) oxide ◆ Δ_rG −155.0 kJ/mol K 1.43 × 10²⁷ pK −27.15: 2K₃[Fe(CN)₆]Crystalline solid + 26Fe₂O₃Crystalline solid
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6KCNCrystalline solid + 3N₂↑Gas + 18Fe₃O₄Crystalline solid + 6CO↑Gas

	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	456.4	−155.0	2042.5	–
per 1 mol of Potassium hexacyanidoferrate(III)	228.2	−77.50	1021.3	–
per 1 mol of Iron(III) oxide	17.55	−5.962	78.558	–
per 1 mol of Potassium cyanide	76.07	−25.83	340.42	–
per 1 mol of Nitrogen	152.1	−51.67	680.83	–
per 1 mol of Iron(II,III) oxide	25.36	−8.611	113.47	–
per 1 mol of Carbon monoxide	76.07	−25.83	340.42	–

Changes in aqueous solution (1)

Reaction of potassium hexacyanidoferrate(III) and iron(III) oxide ◆ Δ_rG −227.6 kJ/mol K 7.48 × 10³⁹ pK −39.87: 2K₃[Fe(CN)₆]Ionized aqueous solution + 26Fe₂O₃Crystalline solid
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6KCNIonized aqueous solution + 3N₂↑Gas + 18Fe₃O₄Crystalline solid + 6CO↑Gas

	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	415.4	−227.6	2147.7	–
per 1 mol of Potassium hexacyanidoferrate(III)	207.7	−113.8	1073.8	–
per 1 mol of Iron(III) oxide	15.98	−8.754	82.604	–
per 1 mol of Potassium cyanide	69.23	−37.93	357.95	–
per 1 mol of Nitrogen	138.5	−75.87	715.90	–
per 1 mol of Iron(II,III) oxide	23.08	−12.64	119.32	–
per 1 mol of Carbon monoxide	69.23	−37.93	357.95	–

Changes in aqueous solution (2)

Reaction of potassium hexacyanidoferrate(III) and iron(III) oxide ◆ Δ_rG −124.0 kJ/mol K 5.29 × 10²¹ pK −21.72: 2K₃[Fe(CN)₆]Ionized aqueous solution + 26Fe₂O₃Crystalline solid
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6KCNIonized aqueous solution + 3N₂↑Gas + 18Fe₃O₄Crystalline solid + 6CO↑Un-ionized aqueous solution

	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	352.8	−124.0	1589.2	–
per 1 mol of Potassium hexacyanidoferrate(III)	176.4	−62.00	794.60	–
per 1 mol of Iron(III) oxide	13.57	−4.769	61.123	–
per 1 mol of Potassium cyanide	58.80	−20.67	264.87	–
per 1 mol of Nitrogen	117.6	−41.33	529.73	–
per 1 mol of Iron(II,III) oxide	19.60	−6.889	88.289	–
per 1 mol of Carbon monoxide	58.80	−20.67	264.87	–

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]	–
Fe₂O₃ (cr)	-824.2^[1]	-742.2^[1]	87.40^[1]	103.85^[1]

* (cr):Crystalline solid, (ai):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
KCN (cr)	-113.0^[1]	-101.86^[1]	128.49^[1]	66.27^[1]
KCN (g)	90.8^[1]	64.17^[1]	261.90^[1]	52.34^[1]
KCN (ai)	-101.7^[1]	-110.9^[1]	196.6^[1]	–
N₂ (g)	0^[1]	0^[1]	191.61^[1]	29.125^[1]
Fe₃O₄ (cr)	-1118.4^[1]	-1015.4^[1]	146.4^[1]	143.43^[1]
CO (g)	-110.525^[1]	-137.168^[1]	197.674^[1]	29.142^[1]
CO (ao)	-120.96^[1]	-119.90^[1]	104.6^[1]	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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