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2FeCl2 + 6MnO2 🔥→ Fe2O3 + 2Cl2↑ + 3Mn2O3

2FeCl₂ + 6MnO₂ 🔥→ Fe₂O₃ + 2Cl₂↑ + 3Mn₂O₃

Last updated: June 13, 2022

Reaction of iron(II) chloride and manganese(IV) oxide: 2FeCl₂Iron(II) chloride + 6MnO₂Manganese(IV) oxide
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Fe₂O₃Iron(III) oxide + 2Cl₂↑Chlorine + 3Mn₂O₃Manganese(III) oxide

The reaction of iron(II) chloride and manganese(IV) oxide yields iron(III) oxide, chlorine, and manganese(III) oxide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of oxidizable species and reducible species

Table of contents

Reaction data

Chemical equation

Reaction of iron(II) chloride and manganese(IV) oxide: 2FeCl₂Iron(II) chloride + 6MnO₂Manganese(IV) oxide
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Fe₂O₃Iron(III) oxide + 2Cl₂↑Chlorine + 3Mn₂O₃Manganese(III) oxide

General equation

Reaction of oxidizable species and reducible species: Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of iron(II) chloride and manganese(IV) oxide

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
FeCl₂	Iron(II) chloride	2	Reducing	Oxidizable
MnO₂	Manganese(IV) oxide	6	Oxidizing	Reducible

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Fe₂O₃	Iron(III) oxide	1	Oxidized	–
Cl₂	Chlorine	2	Oxidized	–
Mn₂O₃	Manganese(III) oxide	3	Reduced	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) chloride and manganese(IV) oxide ◆ Δ_rG 9.9 kJ/mol K 0.18 × 10⁻¹ pK 1.73: 2FeCl₂Crystalline solid + 6MnO₂Crystalline solid
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Fe₂O₃Crystalline solid + 2Cl₂↑Gas + 3Mn₂O₃Crystalline solid

	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	102.6	9.9	310.8	16.47
per 1 mol of Iron(II) chloride	51.30	5.0	155.4	8.235
per 1 mol of Manganese(IV) oxide	17.10	1.7	51.80	2.745
per 1 mol of Iron(III) oxide	102.6	9.9	310.8	16.47
per 1 mol of Chlorine	51.30	5.0	155.4	8.235
per 1 mol of Manganese(III) oxide	34.20	3.3	103.6	5.490

Changes in standard condition (2)

Reaction of iron(II) chloride and manganese(IV) oxide: 2FeCl₂Crystalline solid + 6MnO₂Amorphous solidprecipitated
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Fe₂O₃Crystalline solid + 2Cl₂↑Gas + 3Mn₂O₃Crystalline solid

	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	−2.6	–	–	–
per 1 mol of Iron(II) chloride	−1.3	–	–	–
per 1 mol of Manganese(IV) oxide	−0.43	–	–	–
per 1 mol of Iron(III) oxide	−2.6	–	–	–
per 1 mol of Chlorine	−1.3	–	–	–
per 1 mol of Manganese(III) oxide	−0.87	–	–	–

Changes in aqueous solution (1)

Reaction of iron(II) chloride and manganese(IV) oxide ◆ Δ_rG −36.5 kJ/mol K 2.48 × 10⁶ pK −6.39: 2FeCl₂Un-ionized aqueous solution + 6MnO₂Crystalline solid
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Fe₂O₃Crystalline solid + 2Cl₂↑Gas + 3Mn₂O₃Crystalline solid

	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	–	−36.5	–	–
per 1 mol of Iron(II) chloride	–	−18.3	–	–
per 1 mol of Manganese(IV) oxide	–	−6.08	–	–
per 1 mol of Iron(III) oxide	–	−36.5	–	–
per 1 mol of Chlorine	–	−18.3	–	–
per 1 mol of Manganese(III) oxide	–	−12.2	–	–

Changes in aqueous solution (2)

Reaction of iron(II) chloride and manganese(IV) oxide ◆ Δ_rG −22.6 kJ/mol K 9.11 × 10³ pK −3.96: 2FeCl₂Un-ionized aqueous solution + 6MnO₂Crystalline solid
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Fe₂O₃Crystalline solid + 2Cl₂↑Un-ionized aqueous solution + 3Mn₂O₃Crystalline solid

	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	–	−22.6	–	–
per 1 mol of Iron(II) chloride	–	−11.3	–	–
per 1 mol of Manganese(IV) oxide	–	−3.77	–	–
per 1 mol of Iron(III) oxide	–	−22.6	–	–
per 1 mol of Chlorine	–	−11.3	–	–
per 1 mol of Manganese(III) oxide	–	−7.53	–	–

Changes in aqueous solution (3)

Reaction of iron(II) chloride and manganese(IV) oxide ◆ Δ_rG 88.0 kJ/mol K 0.38 × 10⁻¹⁵ pK 15.42: 2FeCl₂Ionized aqueous solution + 6MnO₂Crystalline solid
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Fe₂O₃Crystalline solid + 2Cl₂↑Gas + 3Mn₂O₃Crystalline solid

	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	265.8	88.0	596.1	–
per 1 mol of Iron(II) chloride	132.9	44.0	298.1	–
per 1 mol of Manganese(IV) oxide	44.30	14.7	99.35	–
per 1 mol of Iron(III) oxide	265.8	88.0	596.1	–
per 1 mol of Chlorine	132.9	44.0	298.1	–
per 1 mol of Manganese(III) oxide	88.60	29.3	198.7	–

Changes in aqueous solution (4)

Reaction of iron(II) chloride and manganese(IV) oxide ◆ Δ_rG 101.9 kJ/mol K 0.14 × 10⁻¹⁷ pK 17.85: 2FeCl₂Ionized aqueous solution + 6MnO₂Crystalline solid
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Fe₂O₃Crystalline solid + 2Cl₂↑Un-ionized aqueous solution + 3Mn₂O₃Crystalline solid

	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	219.0	101.9	392	–
per 1 mol of Iron(II) chloride	109.5	50.95	196	–
per 1 mol of Manganese(IV) oxide	36.50	16.98	65.3	–
per 1 mol of Iron(III) oxide	219.0	101.9	392	–
per 1 mol of Chlorine	109.5	50.95	196	–
per 1 mol of Manganese(III) oxide	73.00	33.97	131	–

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
FeCl₂ (cr)	-341.79^[1]	-302.30^[1]	117.95^[1]	76.65^[1]
FeCl₂ (g)	-148.5^[1]	–	–	–
FeCl₂ (ai)	-423.4^[1]	-341.34^[1]	-24.7^[1]	–
FeCl₂ (ao)	–	-279.1^[1]	–	–
FeCl₂ (cr) 2 hydrate	-953.1^[1]	–	–	–
FeCl₂ (cr) 4 hydrate	-1549.3^[1]	–	–	–
MnO₂ (cr)	-520.03^[1]	-465.14^[1]	53.05^[1]	54.14^[1]
MnO₂ (am) precipitated	-502.5^[1]	–	–	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (am):Amorphous solid

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
Fe₂O₃ (cr)	-824.2^[1]	-742.2^[1]	87.40^[1]	103.85^[1]
Cl₂ (g)	0^[1]	0^[1]	223.066^[1]	33.907^[1]
Cl₂ (ao)	-23.4^[1]	6.94^[1]	121^[1]	–
Mn₂O₃ (cr)	-959.0^[1]	-881.1^[1]	110.5^[1]	107.65^[1]

* (cr):Crystalline solid, (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	9.9 kJ/mol
K	0.18 × 10⁻¹
pK	1.73

Δ_rG	−36.5 kJ/mol
K	2.48 × 10⁶
pK	−6.39

Δ_rG	−22.6 kJ/mol
K	9.11 × 10³
pK	−3.96

Δ_rG	88.0 kJ/mol
K	0.38 × 10⁻¹⁵
pK	15.42

2FeCl2 + 6MnO2 🔥→ Fe2O3 + 2Cl2↑ + 3Mn2O3

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 aqueous solution (1)

Changes in aqueous solution (2)

Changes in aqueous solution (3)

Changes in aqueous solution (4)

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

2FeCl₂ + 6MnO₂ 🔥→ Fe₂O₃ + 2Cl₂↑ + 3Mn₂O₃