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2NaCl + Co3O4 + 4H2O 🔥→ 2NaOH + Cl2↑ + 3Co(OH)2

2NaCl + Co₃O₄ + 4H₂O 🔥→ 2NaOH + Cl₂↑ + 3Co(OH)₂

Last updated: May 12, 2022

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition: 2NaClSodium chloride + Co₃O₄Cobalt(II,III) oxide + 4H₂OWater
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2NaOHSodium hydroxide + Cl₂↑Chlorine + 3Co(OH)₂Cobalt(II) hydroxide

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

Reaction of hardly oxidizable species and oxidizing species under neutral condition

Table of contents

Reaction data

Chemical equation

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition: 2NaClSodium chloride + Co₃O₄Cobalt(II,III) oxide + 4H₂OWater
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2NaOHSodium hydroxide + Cl₂↑Chlorine + 3Co(OH)₂Cobalt(II) hydroxide

General equation

Reaction of hardly oxidizable species and oxidizing species under neutral condition: Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H₂ONon-redox agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NaCl	Sodium chloride	2	Reducing	Hardly oxidizable
Co₃O₄	Cobalt(II,III) oxide	1	Oxidizing	Oxidizing
H₂O	Water	4	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
NaOH	Sodium hydroxide	2	–	–
Cl₂	Chlorine	1	Oxidized	–
Co(OH)₂	Cobalt(II) hydroxide	3	Reduced	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 382 kJ/mol K 0.12 × 10⁻⁶⁶ pK 66.92: 2NaClCrystalline solid + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHCrystalline solid + Cl₂↑Gas + 3Co(OH)₂Crystalline solidblue, precipitated

	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	–	382	–	–
per 1 mol of Sodium chloride	–	191	–	–
per 1 mol of Cobalt(II,III) oxide	–	382	–	–
per 1 mol of Water	–	95.5	–	–
per 1 mol of Sodium hydroxide	–	191	–	–
per 1 mol of Chlorine	–	382	–	–
per 1 mol of Cobalt(II) hydroxide	–	127	–	–

Changes in standard condition (2)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 369 kJ/mol K 0.23 × 10⁻⁶⁴ pK 64.65: 2NaClCrystalline solid + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHCrystalline solid + Cl₂↑Gas + 3Co(OH)₂Crystalline solidpink, precipitated

	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	386	369	63	–
per 1 mol of Sodium chloride	193	185	32	–
per 1 mol of Cobalt(II,III) oxide	386	369	63	–
per 1 mol of Water	96.5	92.3	16	–
per 1 mol of Sodium hydroxide	193	185	32	–
per 1 mol of Chlorine	386	369	63	–
per 1 mol of Cobalt(II) hydroxide	129	123	21	–

Changes in standard condition (3)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 358 kJ/mol K 0.19 × 10⁻⁶² pK 62.72: 2NaClCrystalline solid + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHCrystalline solid + Cl₂↑Gas + 3Co(OH)₂Crystalline solidpink, precipitated, aged

	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	–	358	–	–
per 1 mol of Sodium chloride	–	179	–	–
per 1 mol of Cobalt(II,III) oxide	–	358	–	–
per 1 mol of Water	–	89.5	–	–
per 1 mol of Sodium hydroxide	–	179	–	–
per 1 mol of Chlorine	–	358	–	–
per 1 mol of Cobalt(II) hydroxide	–	119	–	–

Changes in aqueous solution (1)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 405 kJ/mol K 0.11 × 10⁻⁷⁰ pK 70.95: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Gas + 3Co(OH)₂Un-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	–	405	–	–
per 1 mol of Sodium chloride	–	203	–	–
per 1 mol of Cobalt(II,III) oxide	–	405	–	–
per 1 mol of Water	–	101	–	–
per 1 mol of Sodium hydroxide	–	203	–	–
per 1 mol of Chlorine	–	405	–	–
per 1 mol of Cobalt(II) hydroxide	–	135	–	–

Changes in aqueous solution (2)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 320 kJ/mol K 0.87 × 10⁻⁵⁶ pK 56.06: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Gas + 3Co(OH)₂Crystalline solidblue, precipitated

	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	–	–
per 1 mol of Sodium chloride	–	160	–	–
per 1 mol of Cobalt(II,III) oxide	–	320	–	–
per 1 mol of Water	–	80.0	–	–
per 1 mol of Sodium hydroxide	–	160	–	–
per 1 mol of Chlorine	–	320	–	–
per 1 mol of Cobalt(II) hydroxide	–	107	–	–

Changes in aqueous solution (3)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 308 kJ/mol K 0.11 × 10⁻⁵³ pK 53.96: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Gas + 3Co(OH)₂Crystalline solidpink, precipitated

	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	290	308	−57	–
per 1 mol of Sodium chloride	145	154	−29	–
per 1 mol of Cobalt(II,III) oxide	290	308	−57	–
per 1 mol of Water	72.5	77.0	−14	–
per 1 mol of Sodium hydroxide	145	154	−29	–
per 1 mol of Chlorine	290	308	−57	–
per 1 mol of Cobalt(II) hydroxide	96.7	103	−19	–

Changes in aqueous solution (4)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 296 kJ/mol K 0.14 × 10⁻⁵¹ pK 51.86: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Gas + 3Co(OH)₂Crystalline solidpink, precipitated, aged

	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	–	296	–	–
per 1 mol of Sodium chloride	–	148	–	–
per 1 mol of Cobalt(II,III) oxide	–	296	–	–
per 1 mol of Water	–	74.0	–	–
per 1 mol of Sodium hydroxide	–	148	–	–
per 1 mol of Chlorine	–	296	–	–
per 1 mol of Cobalt(II) hydroxide	–	98.7	–	–

Changes in aqueous solution (5)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 412 kJ/mol K 0.66 × 10⁻⁷² pK 72.18: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Un-ionized aqueous solution + 3Co(OH)₂Un-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	–	412	–	–
per 1 mol of Sodium chloride	–	206	–	–
per 1 mol of Cobalt(II,III) oxide	–	412	–	–
per 1 mol of Water	–	103	–	–
per 1 mol of Sodium hydroxide	–	206	–	–
per 1 mol of Chlorine	–	412	–	–
per 1 mol of Cobalt(II) hydroxide	–	137	–	–

Changes in aqueous solution (6)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 327 kJ/mol K 0.52 × 10⁻⁵⁷ pK 57.29: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Un-ionized aqueous solution + 3Co(OH)₂Crystalline solidblue, precipitated

	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	–	327	–	–
per 1 mol of Sodium chloride	–	164	–	–
per 1 mol of Cobalt(II,III) oxide	–	327	–	–
per 1 mol of Water	–	81.8	–	–
per 1 mol of Sodium hydroxide	–	164	–	–
per 1 mol of Chlorine	–	327	–	–
per 1 mol of Cobalt(II) hydroxide	–	109	–	–

Changes in aqueous solution (7)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 315 kJ/mol K 0.65 × 10⁻⁵⁵ pK 55.19: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Un-ionized aqueous solution + 3Co(OH)₂Crystalline solidpink, precipitated

	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	266	315	−159	–
per 1 mol of Sodium chloride	133	158	−79.5	–
per 1 mol of Cobalt(II,III) oxide	266	315	−159	–
per 1 mol of Water	66.5	78.8	−39.8	–
per 1 mol of Sodium hydroxide	133	158	−79.5	–
per 1 mol of Chlorine	266	315	−159	–
per 1 mol of Cobalt(II) hydroxide	88.7	105	−53.0	–

Changes in aqueous solution (8)

Reaction of sodium chloride and cobalt(II,III) oxide under neutral condition ◆ Δ_rG 303 kJ/mol K 0.83 × 10⁻⁵³ pK 53.08: 2NaClIonized aqueous solution + Co₃O₄Crystalline solid + 4H₂OLiquid
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2NaOHIonized aqueous solution + Cl₂↑Un-ionized aqueous solution + 3Co(OH)₂Crystalline solidpink, precipitated, aged

	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	–	303	–	–
per 1 mol of Sodium chloride	–	152	–	–
per 1 mol of Cobalt(II,III) oxide	–	303	–	–
per 1 mol of Water	–	75.8	–	–
per 1 mol of Sodium hydroxide	–	152	–	–
per 1 mol of Chlorine	–	303	–	–
per 1 mol of Cobalt(II) hydroxide	–	101	–	–

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
NaCl (cr)	-411.153^[1]	-384.138^[1]	72.13^[1]	50.50^[1]
NaCl (g)	-176.65^[1]	-196.66^[1]	229.81^[1]	35.77^[1]
NaCl (ai)	-407.27^[1]	-393.133^[1]	115.5^[1]	-90.0^[1]
Co₃O₄ (cr)	-891^[1]	-774^[1]	102.5^[1]	123.4^[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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
NaOH (cr)	-425.609^[1]	-379.494^[1]	64.455^[1]	59.54^[1]
NaOH (g)	-207.1^[1]	-210.0^[1]	228.43^[1]	48.37^[1]
NaOH (ai)	-470.114^[1]	-419.150^[1]	48.1^[1]	-102.1^[1]
NaOH (cr) 1 hydrate	-734.543^[1]	-629.338^[1]	99.50^[1]	90.17^[1]
NaOH (l) 2 hydrate	-1019.076^[1]	-873.091^[1]	195.979^[1]	239.41^[1]
NaOH (l) 3.5 hydrate	-1459.798^[1]	-1236.356^[1]	286.089^[1]	354.43^[1]
NaOH (l) 4 hydrate	-1605.15^[1]	-1356.64^[1]	318.70^[1]	–
NaOH (l) 5 hydrate	-1894.31^[1]	-1596.34^[1]	386.06^[1]	–
NaOH (l) 7 hydrate	-2469.02^[1]	-2073.80^[1]	526.31^[1]	–
Cl₂ (g)	0^[1]	0^[1]	223.066^[1]	33.907^[1]
Cl₂ (ao)	-23.4^[1]	6.94^[1]	121^[1]	–
Co(OH)₂ (cr) blue, precipitated	–	-450.1^[1]	–	–
Co(OH)₂ (cr) pink, precipitated	-539.7^[1]	-454.3^[1]	79^[1]	–
Co(OH)₂ (cr) pink, precipitated, aged	–	-458.1^[1]	–	–
Co(OH)₂ (ai)	-518.0^[1]	-369.0^[1]	-134^[1]	–
Co(OH)₂ (ao)	–	-421.7^[1]	–	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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	382 kJ/mol
K	0.12 × 10⁻⁶⁶
pK	66.92

Δ_rG	369 kJ/mol
K	0.23 × 10⁻⁶⁴
pK	64.65

Δ_rG	358 kJ/mol
K	0.19 × 10⁻⁶²
pK	62.72

Δ_rG	405 kJ/mol
K	0.11 × 10⁻⁷⁰
pK	70.95

2NaCl + Co3O4 + 4H2O 🔥→ 2NaOH + Cl2↑ + 3Co(OH)2

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 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)

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

2NaCl + Co₃O₄ + 4H₂O 🔥→ 2NaOH + Cl₂↑ + 3Co(OH)₂