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10NaCl + Zn(NO3)2 + 6H2O 🔥→ 10NaOH + 5Cl2↑ + N2↑ + Zn(OH)2

10NaCl + Zn(NO₃)₂ + 6H₂O 🔥→ 10NaOH + 5Cl₂↑ + N₂↑ + Zn(OH)₂

Last updated: May 12, 2022

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClSodium chloride + Zn(NO₃)₂Zinc nitrate + 6H₂OWater
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10NaOHSodium hydroxide + 5Cl₂↑Chlorine + N₂↑Nitrogen + Zn(OH)₂Zinc hydroxide

The reaction of sodium chloride, zinc nitrate, and water yields sodium hydroxide, chlorine, nitrogen, and zinc 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 zinc nitrate under neutral condition: 10NaClSodium chloride + Zn(NO₃)₂Zinc nitrate + 6H₂OWater
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10NaOHSodium hydroxide + 5Cl₂↑Chlorine + N₂↑Nitrogen + Zn(OH)₂Zinc 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 zinc nitrate under neutral condition

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
NaCl	Sodium chloride	10	Reducing	Hardly oxidizable
Zn(NO₃)₂	Zinc nitrate	1	Oxidizing	Oxidizing
H₂O	Water	6	–	Water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
NaOH	Sodium hydroxide	10	–	–
Cl₂	Chlorine	5	Oxidized	–
N₂	Nitrogen	1	Reduced	–
Zn(OH)₂	Zinc hydroxide	1	–	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClCrystalline solid + Zn(NO₃)₂Crystalline solid + 6H₂OLiquid
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10NaOHCrystalline solid + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidγ

	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 Sodium chloride	–	–	–	–
per 1 mol of Zinc nitrate	–	–	–	–
per 1 mol of Water	–	–	–	–
per 1 mol of Sodium hydroxide	–	–	–	–
per 1 mol of Chlorine	–	–	–	–
per 1 mol of Nitrogen	–	–	–	–
per 1 mol of Zinc hydroxide	–	–	–	–

Changes in standard condition (2)

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClCrystalline solid + Zn(NO₃)₂Crystalline solid + 6H₂OLiquid
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10NaOHCrystalline solid + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidβ

	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	1412.2	–	–	–
per 1 mol of Sodium chloride	141.22	–	–	–
per 1 mol of Zinc nitrate	1412.2	–	–	–
per 1 mol of Water	235.37	–	–	–
per 1 mol of Sodium hydroxide	141.22	–	–	–
per 1 mol of Chlorine	282.44	–	–	–
per 1 mol of Nitrogen	1412.2	–	–	–
per 1 mol of Zinc hydroxide	1412.2	–	–	–

Changes in standard condition (3)

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClCrystalline solid + Zn(NO₃)₂Crystalline solid + 6H₂OLiquid
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10NaOHCrystalline solid + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidε

	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	1410.9	–	–	–
per 1 mol of Sodium chloride	141.09	–	–	–
per 1 mol of Zinc nitrate	1410.9	–	–	–
per 1 mol of Water	235.15	–	–	–
per 1 mol of Sodium hydroxide	141.09	–	–	–
per 1 mol of Chlorine	282.18	–	–	–
per 1 mol of Nitrogen	1410.9	–	–	–
per 1 mol of Zinc hydroxide	1410.9	–	–	–

Changes in standard condition (4)

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClCrystalline solid + Zn(NO₃)₂Crystalline solid + 6H₂OLiquid
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10NaOHCrystalline solid + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidprecipitated

	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	1411.9	–	–	–
per 1 mol of Sodium chloride	141.19	–	–	–
per 1 mol of Zinc nitrate	1411.9	–	–	–
per 1 mol of Water	235.32	–	–	–
per 1 mol of Sodium hydroxide	141.19	–	–	–
per 1 mol of Chlorine	282.38	–	–	–
per 1 mol of Nitrogen	1411.9	–	–	–
per 1 mol of Zinc hydroxide	1411.9	–	–	–

Changes in aqueous solution (1)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 1009.44 kJ/mol K 0.14 × 10⁻¹⁷⁶ pK 176.85: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Gas + N₂↑Gas + Zn(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	–	1009.44	–	–
per 1 mol of Sodium chloride	–	100.944	–	–
per 1 mol of Zinc nitrate	–	1009.44	–	–
per 1 mol of Water	–	168.240	–	–
per 1 mol of Sodium hydroxide	–	100.944	–	–
per 1 mol of Chlorine	–	201.888	–	–
per 1 mol of Nitrogen	–	1009.44	–	–
per 1 mol of Zinc hydroxide	–	1009.44	–	–

Changes in aqueous solution (2)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 978.36 kJ/mol K 0.40 × 10⁻¹⁷¹ pK 171.40: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidγ

	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	–	978.36	–	–
per 1 mol of Sodium chloride	–	97.836	–	–
per 1 mol of Zinc nitrate	–	978.36	–	–
per 1 mol of Water	–	163.06	–	–
per 1 mol of Sodium hydroxide	–	97.836	–	–
per 1 mol of Chlorine	–	195.67	–	–
per 1 mol of Nitrogen	–	978.36	–	–
per 1 mol of Zinc hydroxide	–	978.36	–	–

Changes in aqueous solution (3)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 978.65 kJ/mol K 0.35 × 10⁻¹⁷¹ pK 171.45: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidβ

	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	1013.24	978.65	114.0	–
per 1 mol of Sodium chloride	101.324	97.865	11.40	–
per 1 mol of Zinc nitrate	1013.24	978.65	114.0	–
per 1 mol of Water	168.873	163.11	19.00	–
per 1 mol of Sodium hydroxide	101.324	97.865	11.40	–
per 1 mol of Chlorine	202.648	195.73	22.80	–
per 1 mol of Nitrogen	1013.24	978.65	114.0	–
per 1 mol of Zinc hydroxide	1013.24	978.65	114.0	–

Changes in aqueous solution (4)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 977.10 kJ/mol K 0.66 × 10⁻¹⁷¹ pK 171.18: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidε

	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	1011.90	977.10	114.4	−176
per 1 mol of Sodium chloride	101.190	97.710	11.44	−17.6
per 1 mol of Zinc nitrate	1011.90	977.10	114.4	−176
per 1 mol of Water	168.650	162.85	19.07	−29.3
per 1 mol of Sodium hydroxide	101.190	97.710	11.44	−17.6
per 1 mol of Chlorine	202.380	195.42	22.88	−35.2
per 1 mol of Nitrogen	1011.90	977.10	114.4	−176
per 1 mol of Zinc hydroxide	1011.90	977.10	114.4	−176

Changes in aqueous solution (5)

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Gas + N₂↑Gas + Zn(OH)₂Crystalline solidprecipitated

	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	1013.0	–	–	–
per 1 mol of Sodium chloride	101.30	–	–	–
per 1 mol of Zinc nitrate	1013.0	–	–	–
per 1 mol of Water	168.83	–	–	–
per 1 mol of Sodium hydroxide	101.30	–	–	–
per 1 mol of Chlorine	202.60	–	–	–
per 1 mol of Nitrogen	1013.0	–	–	–
per 1 mol of Zinc hydroxide	1013.0	–	–	–

Changes in aqueous solution (6)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 1044.14 kJ/mol K 0.12 × 10⁻¹⁸² pK 182.93: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Un-ionized aqueous solution + N₂↑Gas + Zn(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	–	1044.14	–	–
per 1 mol of Sodium chloride	–	104.414	–	–
per 1 mol of Zinc nitrate	–	1044.14	–	–
per 1 mol of Water	–	174.023	–	–
per 1 mol of Sodium hydroxide	–	104.414	–	–
per 1 mol of Chlorine	–	208.828	–	–
per 1 mol of Nitrogen	–	1044.14	–	–
per 1 mol of Zinc hydroxide	–	1044.14	–	–

Changes in aqueous solution (7)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 1013.06 kJ/mol K 0.33 × 10⁻¹⁷⁷ pK 177.48: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Un-ionized aqueous solution + N₂↑Gas + Zn(OH)₂Crystalline solidγ

	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	–	1013.06	–	–
per 1 mol of Sodium chloride	–	101.306	–	–
per 1 mol of Zinc nitrate	–	1013.06	–	–
per 1 mol of Water	–	168.843	–	–
per 1 mol of Sodium hydroxide	–	101.306	–	–
per 1 mol of Chlorine	–	202.612	–	–
per 1 mol of Nitrogen	–	1013.06	–	–
per 1 mol of Zinc hydroxide	–	1013.06	–	–

Changes in aqueous solution (8)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 1013.35 kJ/mol K 0.29 × 10⁻¹⁷⁷ pK 177.53: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Un-ionized aqueous solution + N₂↑Gas + Zn(OH)₂Crystalline solidβ

	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	896.2	1013.35	−396	–
per 1 mol of Sodium chloride	89.62	101.335	−39.6	–
per 1 mol of Zinc nitrate	896.2	1013.35	−396	–
per 1 mol of Water	149.4	168.892	−66.0	–
per 1 mol of Sodium hydroxide	89.62	101.335	−39.6	–
per 1 mol of Chlorine	179.2	202.670	−79.2	–
per 1 mol of Nitrogen	896.2	1013.35	−396	–
per 1 mol of Zinc hydroxide	896.2	1013.35	−396	–

Changes in aqueous solution (9)

Reaction of sodium chloride and zinc nitrate under neutral condition ◆ Δ_rG 1011.80 kJ/mol K 0.55 × 10⁻¹⁷⁷ pK 177.26: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Un-ionized aqueous solution + N₂↑Gas + Zn(OH)₂Crystalline solidε

	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	894.9	1011.80	−396	–
per 1 mol of Sodium chloride	89.49	101.180	−39.6	–
per 1 mol of Zinc nitrate	894.9	1011.80	−396	–
per 1 mol of Water	149.2	168.633	−66.0	–
per 1 mol of Sodium hydroxide	89.49	101.180	−39.6	–
per 1 mol of Chlorine	179.0	202.360	−79.2	–
per 1 mol of Nitrogen	894.9	1011.80	−396	–
per 1 mol of Zinc hydroxide	894.9	1011.80	−396	–

Changes in aqueous solution (10)

Reaction of sodium chloride and zinc nitrate under neutral condition: 10NaClIonized aqueous solution + Zn(NO₃)₂Ionized aqueous solution + 6H₂OLiquid
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10NaOHIonized aqueous solution + 5Cl₂↑Un-ionized aqueous solution + N₂↑Gas + Zn(OH)₂Crystalline solidprecipitated

	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	895.9	–	–	–
per 1 mol of Sodium chloride	89.59	–	–	–
per 1 mol of Zinc nitrate	895.9	–	–	–
per 1 mol of Water	149.3	–	–	–
per 1 mol of Sodium hydroxide	89.59	–	–	–
per 1 mol of Chlorine	179.2	–	–	–
per 1 mol of Nitrogen	895.9	–	–	–
per 1 mol of Zinc hydroxide	895.9	–	–	–

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]
Zn(NO₃)₂ (cr)	-483.7^[1]	–	–	–
Zn(NO₃)₂ (ai)	-568.61^[1]	-369.57^[1]	180.7^[1]	-126^[1]
Zn(NO₃)₂ (cr) 1 hydrate	-805.0^[1]	–	–	–
Zn(NO₃)₂ (cr) 2 hydrate	-1110.27^[1]	–	–	–
Zn(NO₃)₂ (cr) 4 hydrate	-1699.12^[1]	–	–	–
Zn(NO₃)₂ (cr) 6 hydrate	-2306.64^[1]	-1772.71^[1]	456.9^[1]	323.0^[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]	–
N₂ (g)	0^[1]	0^[1]	191.61^[1]	29.125^[1]
Zn(OH)₂ (cr) γ	–	-553.81^[1]	–	–
Zn(OH)₂ (cr) β	-641.91^[1]	-553.52^[1]	81.2^[1]	–
Zn(OH)₂ (cr) ε	-643.25^[1]	-555.07^[1]	81.6^[1]	72.4^[1]
Zn(OH)₂ (cr) precipitated	-642.2^[1]	–	–	–
Zn(OH)₂ (ai)	-613.88^[1]	-461.56^[1]	-133.5^[1]	-251^[1]
Zn(OH)₂ (ao)	–	-522.73^[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	1009.44 kJ/mol
K	0.14 × 10⁻¹⁷⁶
pK	176.85

Δ_rG	978.36 kJ/mol
K	0.40 × 10⁻¹⁷¹
pK	171.40

Δ_rG	978.65 kJ/mol
K	0.35 × 10⁻¹⁷¹
pK	171.45

Δ_rG	977.10 kJ/mol
K	0.66 × 10⁻¹⁷¹
pK	171.18

10NaCl + Zn(NO3)2 + 6H2O 🔥→ 10NaOH + 5Cl2↑ + N2↑ + Zn(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 standard condition (4)

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)

Changes in aqueous solution (9)

Changes in aqueous solution (10)

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

10NaCl + Zn(NO₃)₂ + 6H₂O 🔥→ 10NaOH + 5Cl₂↑ + N₂↑ + Zn(OH)₂