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16NO + 9Co(OH)2 🔥→ 5Co(NO3)2 + 6NH3 + 4CoO

16NO + 9Co(OH)₂ 🔥→ 5Co(NO₃)₂ + 6NH₃ + 4CoO

Last updated: June 13, 2022

Reaction of nitrogen monoxide and cobalt(II) hydroxide: 16NONitrogen monoxide + 9Co(OH)₂Cobalt(II) hydroxide
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5Co(NO₃)₂Cobalt(II) nitrate + 6NH₃Ammonia + 4CoOCobalt(II) oxide

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

Reaction of self redoxing species and base

Table of contents

Reaction data

Chemical equation

Reaction of nitrogen monoxide and cobalt(II) hydroxide: 16NONitrogen monoxide + 9Co(OH)₂Cobalt(II) hydroxide
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5Co(NO₃)₂Cobalt(II) nitrate + 6NH₃Ammonia + 4CoOCobalt(II) oxide

General equation

Reaction of self redoxing species and base: Self-redoxing speciesSelf redox agent + BaseNon-redox agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of nitrogen monoxide and cobalt(II) hydroxide

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NO	Nitrogen monoxide	16	–	Self redoxing
Co(OH)₂	Cobalt(II) hydroxide	9	–	Base

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Co(NO₃)₂	Cobalt(II) nitrate	5	Oxidized	–
NH₃	Ammonia	6	Reduced	–
CoO	Cobalt(II) oxide	4	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of nitrogen monoxide and cobalt(II) hydroxide: 16NOGas + 9Co(OH)₂Crystalline solidblue, precipitated
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5Co(NO₃)₂Crystalline solid + 6NH₃Gas + 4CoOCrystalline 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	–	–	–	–
per 1 mol of Nitrogen monoxide	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–
per 1 mol of Cobalt(II) nitrate	–	–	–	–
per 1 mol of Ammonia	–	–	–	–
per 1 mol of Cobalt(II) oxide	–	–	–	–

Changes in standard condition (2)

Reaction of nitrogen monoxide and cobalt(II) hydroxide: 16NOGas + 9Co(OH)₂Crystalline solidpink, precipitated
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5Co(NO₃)₂Crystalline solid + 6NH₃Gas + 4CoOCrystalline 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	82.4	–	–	–
per 1 mol of Nitrogen monoxide	5.15	–	–	–
per 1 mol of Cobalt(II) hydroxide	9.16	–	–	–
per 1 mol of Cobalt(II) nitrate	16.5	–	–	–
per 1 mol of Ammonia	13.7	–	–	–
per 1 mol of Cobalt(II) oxide	20.6	–	–	–

Changes in standard condition (3)

Reaction of nitrogen monoxide and cobalt(II) hydroxide: 16NOGas + 9Co(OH)₂Crystalline solidpink, precipitated, aged
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5Co(NO₃)₂Crystalline solid + 6NH₃Gas + 4CoOCrystalline 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	–	–	–	–
per 1 mol of Nitrogen monoxide	–	–	–	–
per 1 mol of Cobalt(II) hydroxide	–	–	–	–
per 1 mol of Cobalt(II) nitrate	–	–	–	–
per 1 mol of Ammonia	–	–	–	–
per 1 mol of Cobalt(II) oxide	–	–	–	–

Changes in aqueous solution (1)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 70.5 kJ/mol K 0.45 × 10⁻¹² pK 12.35: 16NOGas + 9Co(OH)₂Un-ionized aqueous solution
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5Co(NO₃)₂Ionized aqueous solution + 6NH₃Gas + 4CoOCrystalline 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	–	70.5	–	–
per 1 mol of Nitrogen monoxide	–	4.41	–	–
per 1 mol of Cobalt(II) hydroxide	–	7.83	–	–
per 1 mol of Cobalt(II) nitrate	–	14.1	–	–
per 1 mol of Ammonia	–	11.8	–	–
per 1 mol of Cobalt(II) oxide	–	17.6	–	–

Changes in aqueous solution (2)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 10.2 kJ/mol K 0.16 × 10⁻¹ pK 1.79: 16NOGas + 9Co(OH)₂Un-ionized aqueous solution
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⟶
5Co(NO₃)₂Ionized aqueous solution + 6NH₃Un-ionized aqueous solution + 4CoOCrystalline 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	–	10.2	–	–
per 1 mol of Nitrogen monoxide	–	0.637	–	–
per 1 mol of Cobalt(II) hydroxide	–	1.13	–	–
per 1 mol of Cobalt(II) nitrate	–	2.04	–	–
per 1 mol of Ammonia	–	1.70	–	–
per 1 mol of Cobalt(II) oxide	–	2.55	–	–

Changes in aqueous solution (3)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 326.1 kJ/mol K 0.74 × 10⁻⁵⁷ pK 57.13: 16NOGas + 9Co(OH)₂Crystalline solidblue, precipitated
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5Co(NO₃)₂Ionized aqueous solution + 6NH₃Gas + 4CoOCrystalline 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	–	326.1	–	–
per 1 mol of Nitrogen monoxide	–	20.38	–	–
per 1 mol of Cobalt(II) hydroxide	–	36.23	–	–
per 1 mol of Cobalt(II) nitrate	–	65.22	–	–
per 1 mol of Ammonia	–	54.35	–	–
per 1 mol of Cobalt(II) oxide	–	81.53	–	–

Changes in aqueous solution (4)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 265.8 kJ/mol K 0.27 × 10⁻⁴⁶ pK 46.57: 16NOGas + 9Co(OH)₂Crystalline solidblue, precipitated
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⟶
5Co(NO₃)₂Ionized aqueous solution + 6NH₃Un-ionized aqueous solution + 4CoOCrystalline 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	–	–
per 1 mol of Nitrogen monoxide	–	16.61	–	–
per 1 mol of Cobalt(II) hydroxide	–	29.53	–	–
per 1 mol of Cobalt(II) nitrate	–	53.16	–	–
per 1 mol of Ammonia	–	44.30	–	–
per 1 mol of Cobalt(II) oxide	–	66.45	–	–

Changes in aqueous solution (5)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 363.9 kJ/mol K 0.18 × 10⁻⁶³ pK 63.75: 16NOGas + 9Co(OH)₂Crystalline solidpink, precipitated
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⟶
5Co(NO₃)₂Ionized aqueous solution + 6NH₃Gas + 4CoOCrystalline 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	−179.1	363.9	−1817	–
per 1 mol of Nitrogen monoxide	−11.19	22.74	−113.6	–
per 1 mol of Cobalt(II) hydroxide	−19.90	40.43	−201.9	–
per 1 mol of Cobalt(II) nitrate	−35.82	72.78	−363.4	–
per 1 mol of Ammonia	−29.85	60.65	−302.8	–
per 1 mol of Cobalt(II) oxide	−44.77	90.97	−454.3	–

Changes in aqueous solution (6)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 303.6 kJ/mol K 0.65 × 10⁻⁵³ pK 53.19: 16NOGas + 9Co(OH)₂Crystalline solidpink, precipitated
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⟶
5Co(NO₃)₂Ionized aqueous solution + 6NH₃Un-ionized aqueous solution + 4CoOCrystalline 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	−384.2	303.6	−2303	–
per 1 mol of Nitrogen monoxide	−24.01	18.98	−143.9	–
per 1 mol of Cobalt(II) hydroxide	−42.69	33.73	−255.9	–
per 1 mol of Cobalt(II) nitrate	−76.84	60.72	−460.6	–
per 1 mol of Ammonia	−64.03	50.60	−383.8	–
per 1 mol of Cobalt(II) oxide	−96.05	75.90	−575.8	–

Changes in aqueous solution (7)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 398.1 kJ/mol K 0.18 × 10⁻⁶⁹ pK 69.74: 16NOGas + 9Co(OH)₂Crystalline solidpink, precipitated, aged
🔥
⟶
5Co(NO₃)₂Ionized aqueous solution + 6NH₃Gas + 4CoOCrystalline 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	–	398.1	–	–
per 1 mol of Nitrogen monoxide	–	24.88	–	–
per 1 mol of Cobalt(II) hydroxide	–	44.23	–	–
per 1 mol of Cobalt(II) nitrate	–	79.62	–	–
per 1 mol of Ammonia	–	66.35	–	–
per 1 mol of Cobalt(II) oxide	–	99.53	–	–

Changes in aqueous solution (8)

Reaction of nitrogen monoxide and cobalt(II) hydroxide ◆ Δ_rG 337.8 kJ/mol K 0.66 × 10⁻⁵⁹ pK 59.18: 16NOGas + 9Co(OH)₂Crystalline solidpink, precipitated, aged
🔥
⟶
5Co(NO₃)₂Ionized aqueous solution + 6NH₃Un-ionized aqueous solution + 4CoOCrystalline 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	–	337.8	–	–
per 1 mol of Nitrogen monoxide	–	21.11	–	–
per 1 mol of Cobalt(II) hydroxide	–	37.53	–	–
per 1 mol of Cobalt(II) nitrate	–	67.56	–	–
per 1 mol of Ammonia	–	56.30	–	–
per 1 mol of Cobalt(II) oxide	–	84.45	–	–

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
NO (g)	90.25^[1]	86.55^[1]	210.761^[1]	29.844^[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]	–	–

* (g):Gas, (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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
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]
NH₃ (g)	-46.11^[1]	-16.45^[1]	192.45^[1]	35.06^[1]
NH₃ (ao)	-80.29^[1]	-26.50^[1]	111.3^[1]	–
CoO (cr)	-237.94^[1]	-214.20^[1]	52.97^[1]	55.23^[1]

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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	70.5 kJ/mol
K	0.45 × 10⁻¹²
pK	12.35

Δ_rG	10.2 kJ/mol
K	0.16 × 10⁻¹
pK	1.79

Δ_rG	326.1 kJ/mol
K	0.74 × 10⁻⁵⁷
pK	57.13

Δ_rG	265.8 kJ/mol
K	0.27 × 10⁻⁴⁶
pK	46.57

16NO + 9Co(OH)2 🔥→ 5Co(NO3)2 + 6NH3 + 4CoO

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

16NO + 9Co(OH)₂ 🔥→ 5Co(NO₃)₂ + 6NH₃ + 4CoO