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Co(NO3)2 + H2O 💧⚡→ Co(OH)2 + 2NO↑ + O3↑

Co(NO₃)₂ + H₂O 💧⚡→ Co(OH)₂ + 2NO↑ + O₃↑

Last updated: June 13, 2022

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent: Co(NO₃)₂Cobalt(II) nitrate + H₂OWater
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Co(OH)₂Cobalt(II) hydroxide + 2NO↑Nitrogen monoxide + O₃↑Ozone

Electrolysis of aqueous cobalt(II) nitrate yields cobalt(II) hydroxide, nitrogen monoxide, and ozone (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Electrolysis of aqueous solution with water as non redox agent

Table of contents

Reaction data

Chemical equation

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent: Co(NO₃)₂Cobalt(II) nitrate + H₂OWater
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Co(OH)₂Cobalt(II) hydroxide + 2NO↑Nitrogen monoxide + O₃↑Ozone

General equation

Electrolysis of aqueous solution with water as non redox agent: Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H₂ONon-redox agent
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ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
Co(NO₃)₂	Cobalt(II) nitrate	1	Self redox agent	Very soluble in water
H₂O	Water	1	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Co(OH)₂	Cobalt(II) hydroxide	1	–	–
NO	Nitrogen monoxide	2	Reduced	–
O₃	Ozone	1	Oxidized	–

Thermodynamic changes

Changes in standard condition (1)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent: Co(NO₃)₂Crystalline solid + H₂OLiquid
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Co(OH)₂Crystalline solidblue, precipitated + 2NO↑Gas + O₃↑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	–	–	–	–
per 1 mol of Cobalt(II) nitrate	–	–	–	–
per 1 mol of Water	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–
per 1 mol of Nitrogen monoxide	–	–	–	–
per 1 mol of Ozone	–	–	–	–

Changes in standard condition (2)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent: Co(NO₃)₂Crystalline solid + H₂OLiquid
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Co(OH)₂Crystalline solidpink, precipitated + 2NO↑Gas + O₃↑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	489.8	–	–	–
per 1 mol of Cobalt(II) nitrate	489.8	–	–	–
per 1 mol of Water	489.8	–	–	–
per 1 mol of Cobalt(II) hydroxide	489.8	–	–	–
per 1 mol of Nitrogen monoxide	244.9	–	–	–
per 1 mol of Ozone	489.8	–	–	–

Changes in standard condition (3)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent: Co(NO₃)₂Crystalline solid + H₂OLiquid
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Co(OH)₂Crystalline solidpink, precipitated, aged + 2NO↑Gas + O₃↑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	–	–	–	–
per 1 mol of Cobalt(II) nitrate	–	–	–	–
per 1 mol of Water	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–
per 1 mol of Nitrogen monoxide	–	–	–	–
per 1 mol of Ozone	–	–	–	–

Changes in aqueous solution (1)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 428.6 kJ/mol K 0.82 × 10⁻⁷⁵ pK 75.09: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Un-ionized aqueous solution + 2NO↑Gas + O₃↑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	–	428.6	–	–
per 1 mol of Cobalt(II) nitrate	–	428.6	–	–
per 1 mol of Water	–	428.6	–	–
per 1 mol of Cobalt(II) hydroxide	–	428.6	–	–
per 1 mol of Nitrogen monoxide	–	214.3	–	–
per 1 mol of Ozone	–	428.6	–	–

Changes in aqueous solution (2)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 439.5 kJ/mol K 0.10 × 10⁻⁷⁶ pK 77.00: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Un-ionized aqueous solution + 2NO↑Gas + O₃↑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	–	439.5	–	–
per 1 mol of Cobalt(II) nitrate	–	439.5	–	–
per 1 mol of Water	–	439.5	–	–
per 1 mol of Cobalt(II) hydroxide	–	439.5	–	–
per 1 mol of Nitrogen monoxide	–	219.8	–	–
per 1 mol of Ozone	–	439.5	–	–

Changes in aqueous solution (3)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 400.2 kJ/mol K 0.77 × 10⁻⁷⁰ pK 70.11: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Crystalline solidblue, precipitated + 2NO↑Gas + O₃↑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	–	400.2	–	–
per 1 mol of Cobalt(II) nitrate	–	400.2	–	–
per 1 mol of Water	–	400.2	–	–
per 1 mol of Cobalt(II) hydroxide	–	400.2	–	–
per 1 mol of Nitrogen monoxide	–	200.1	–	–
per 1 mol of Ozone	–	400.2	–	–

Changes in aqueous solution (4)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 411.1 kJ/mol K 0.95 × 10⁻⁷² pK 72.02: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Crystalline solidblue, precipitated + 2NO↑Gas + O₃↑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	–	411.1	–	–
per 1 mol of Cobalt(II) nitrate	–	411.1	–	–
per 1 mol of Water	–	411.1	–	–
per 1 mol of Cobalt(II) hydroxide	–	411.1	–	–
per 1 mol of Nitrogen monoxide	–	205.6	–	–
per 1 mol of Ozone	–	411.1	–	–

Changes in aqueous solution (5)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 396.0 kJ/mol K 0.42 × 10⁻⁶⁹ pK 69.38: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Crystalline solidpink, precipitated + 2NO↑Gas + O₃↑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	542.1	396.0	490	–
per 1 mol of Cobalt(II) nitrate	542.1	396.0	490	–
per 1 mol of Water	542.1	396.0	490	–
per 1 mol of Cobalt(II) hydroxide	542.1	396.0	490	–
per 1 mol of Nitrogen monoxide	271.1	198.0	245	–
per 1 mol of Ozone	542.1	396.0	490	–

Changes in aqueous solution (6)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 406.9 kJ/mol K 0.52 × 10⁻⁷¹ pK 71.29: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Crystalline solidpink, precipitated + 2NO↑Gas + O₃↑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	525.3	406.9	397	–
per 1 mol of Cobalt(II) nitrate	525.3	406.9	397	–
per 1 mol of Water	525.3	406.9	397	–
per 1 mol of Cobalt(II) hydroxide	525.3	406.9	397	–
per 1 mol of Nitrogen monoxide	262.6	203.4	199	–
per 1 mol of Ozone	525.3	406.9	397	–

Changes in aqueous solution (7)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 392.2 kJ/mol K 0.19 × 10⁻⁶⁸ pK 68.71: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Crystalline solidpink, precipitated, aged + 2NO↑Gas + O₃↑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	–	392.2	–	–
per 1 mol of Cobalt(II) nitrate	–	392.2	–	–
per 1 mol of Water	–	392.2	–	–
per 1 mol of Cobalt(II) hydroxide	–	392.2	–	–
per 1 mol of Nitrogen monoxide	–	196.1	–	–
per 1 mol of Ozone	–	392.2	–	–

Changes in aqueous solution (8)

Electrolysis of aqueous cobalt(II) nitrate with water as non-redox agent ◆ Δ_rG 403.1 kJ/mol K 0.24 × 10⁻⁷⁰ pK 70.62: Co(NO₃)₂Ionized aqueous solution + H₂OLiquid
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Co(OH)₂Crystalline solidpink, precipitated, aged + 2NO↑Gas + O₃↑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	–	403.1	–	–
per 1 mol of Cobalt(II) nitrate	–	403.1	–	–
per 1 mol of Water	–	403.1	–	–
per 1 mol of Cobalt(II) hydroxide	–	403.1	–	–
per 1 mol of Nitrogen monoxide	–	201.6	–	–
per 1 mol of Ozone	–	403.1	–	–

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
Co(NO₃)₂ (cr)	-420.5^[1]	–	–	–
Co(NO₃)₂ (ai)	-472.8^[1]	-276.9^[1]	180^[1]	–
Co(NO₃)₂ (cr) 2 hydrate	-1021.7^[1]	–	–	–
Co(NO₃)₂ (cr) 3 hydrate	-1325.9^[1]	–	–	–
Co(NO₃)₂ (cr) 4 hydrate	-1630.5^[1]	–	–	–
Co(NO₃)₂ (cr) 6 hydrate	-2211.20^[1]	–	–	452^[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, (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
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]	–	–
NO (g)	90.25^[1]	86.55^[1]	210.761^[1]	29.844^[1]
O₃ (g)	142.7^[1]	163.2^[1]	238.93^[1]	39.20^[1]
O₃ (ao)	125.9^[1]	174.1^[1]	146^[1]	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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	428.6 kJ/mol
K	0.82 × 10⁻⁷⁵
pK	75.09

Δ_rG	439.5 kJ/mol
K	0.10 × 10⁻⁷⁶
pK	77.00

Δ_rG	400.2 kJ/mol
K	0.77 × 10⁻⁷⁰
pK	70.11

Δ_rG	411.1 kJ/mol
K	0.95 × 10⁻⁷²
pK	72.02

Co(NO3)2 + H2O 💧⚡→ Co(OH)2 + 2NO↑ + O3↑

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

Co(NO₃)₂ + H₂O 💧⚡→ Co(OH)₂ + 2NO↑ + O₃↑