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Chemical reactions
H2S + 2AgNO3 → SO2 + 2Ag + N2O3 + H2O

H₂S + 2AgNO₃ → SO₂ + 2Ag + N₂O₃ + H₂O

Last updated: June 13, 2022

Reaction of hydrogen sulfide and silver(I) nitrate: H₂SHydrogen sulfide + 2AgNO₃Silver(I) nitrate
⟶
SO₂Sulfur dioxide + 2AgSilver + N₂O₃Dinitrogen trioxide + H₂OWater

The reaction of hydrogen sulfide and silver(I) nitrate yields sulfur dioxide, silver, dinitrogen trioxide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Reaction of reducing species and oxidizing species

Table of contents

Reaction data

Chemical equation

Reaction of hydrogen sulfide and silver(I) nitrate: H₂SHydrogen sulfide + 2AgNO₃Silver(I) nitrate
⟶
SO₂Sulfur dioxide + 2AgSilver + N₂O₃Dinitrogen trioxide + H₂OWater

General equation

Reaction of reducing species and oxidizing species: Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen sulfide and silver(I) nitrate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
H₂S	Hydrogen sulfide	1	Reducing	Reducing
AgNO₃	Silver(I) nitrate	2	Oxidizing	Oxidizing

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
SO₂	Sulfur dioxide	1	Oxidized	–
Ag	Silver	2	Reduced	–
N₂O₃	Dinitrogen trioxide	1	Reduced	–
H₂O	Water	1	–	–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and silver(I) nitrate ◆ Δ_rG −297.48 kJ/mol K 1.31 × 10⁵² pK −52.12: H₂SGas + 2AgNO₃Crystalline solid
⟶
SO₂Gas + 2AgCrystalline solid + N₂O₃Gas + H₂OLiquid

	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	−229.53	−297.48	227.88	11.14
per 1 mol of Hydrogen sulfide	−229.53	−297.48	227.88	11.14
per 1 mol of Silver(I) nitrate	−114.77	−148.74	113.94	5.570
per 1 mol of Sulfur dioxide	−229.53	−297.48	227.88	11.14
per 1 mol of Silver	−114.77	−148.74	113.94	5.570
per 1 mol of Dinitrogen trioxide	−229.53	−297.48	227.88	11.14
per 1 mol of Water	−229.53	−297.48	227.88	11.14

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and silver(I) nitrate ◆ Δ_rG −301.71 kJ/mol K 7.20 × 10⁵² pK −52.86: H₂SUn-ionized aqueous solution + 2AgNO₃Ionized aqueous solution
⟶
SO₂Gas + 2AgCrystalline solid + N₂O₃Gas + H₂OLiquid

	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	−255.6	−301.71	156	–
per 1 mol of Hydrogen sulfide	−255.6	−301.71	156	–
per 1 mol of Silver(I) nitrate	−127.8	−150.85	78.0	–
per 1 mol of Sulfur dioxide	−255.6	−301.71	156	–
per 1 mol of Silver	−127.8	−150.85	78.0	–
per 1 mol of Dinitrogen trioxide	−255.6	−301.71	156	–
per 1 mol of Water	−255.6	−301.71	156	–

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and silver(I) nitrate ◆ Δ_rG −302.20 kJ/mol K 8.77 × 10⁵² pK −52.94: H₂SUn-ionized aqueous solution + 2AgNO₃Ionized aqueous solution
⟶
SO₂Un-ionized aqueous solution + 2AgCrystalline solid + N₂O₃Gas + H₂OLiquid

	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	−281.8	−302.20	70	–
per 1 mol of Hydrogen sulfide	−281.8	−302.20	70	–
per 1 mol of Silver(I) nitrate	−140.9	−151.10	35	–
per 1 mol of Sulfur dioxide	−281.8	−302.20	70	–
per 1 mol of Silver	−140.9	−151.10	35	–
per 1 mol of Dinitrogen trioxide	−281.8	−302.20	70	–
per 1 mol of Water	−281.8	−302.20	70	–

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and silver(I) nitrate ◆ Δ_rG −305.05 kJ/mol K 2.77 × 10⁵³ pK −53.44: H₂SUn-ionized aqueous solution + 2AgNO₃Un-ionized aqueous solution
⟶
SO₂Gas + 2AgCrystalline solid + N₂O₃Gas + H₂OLiquid

	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	–	−305.05	–	–
per 1 mol of Hydrogen sulfide	–	−305.05	–	–
per 1 mol of Silver(I) nitrate	–	−152.53	–	–
per 1 mol of Sulfur dioxide	–	−305.05	–	–
per 1 mol of Silver	–	−152.53	–	–
per 1 mol of Dinitrogen trioxide	–	−305.05	–	–
per 1 mol of Water	–	−305.05	–	–

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and silver(I) nitrate ◆ Δ_rG −305.54 kJ/mol K 3.38 × 10⁵³ pK −53.53: H₂SUn-ionized aqueous solution + 2AgNO₃Un-ionized aqueous solution
⟶
SO₂Un-ionized aqueous solution + 2AgCrystalline solid + N₂O₃Gas + H₂OLiquid

	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	–	−305.54	–	–
per 1 mol of Hydrogen sulfide	–	−305.54	–	–
per 1 mol of Silver(I) nitrate	–	−152.77	–	–
per 1 mol of Sulfur dioxide	–	−305.54	–	–
per 1 mol of Silver	–	−152.77	–	–
per 1 mol of Dinitrogen trioxide	–	−305.54	–	–
per 1 mol of Water	–	−305.54	–	–

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
H₂S (g)	-20.63^[1]	-33.56^[1]	205.79^[1]	34.23^[1]
H₂S (ao)	-39.7^[1]	-27.83^[1]	121^[1]	–
AgNO₃ (cr)	-124.39^[1]	-33.41^[1]	140.92^[1]	93.05^[1]
AgNO₃ (ai)	-101.80^[1]	-34.16^[1]	219.2^[1]	-64.9^[1]
AgNO₃ (ao)	–	-32.49^[1]	–	–

* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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
SO₂ (l)	-320.5^[1]	–	–	–
SO₂ (g)	-296.830^[1]	-300.194^[1]	248.22^[1]	39.87^[1]
SO₂ (ao)	-322.980^[1]	-300.676^[1]	161.9^[1]	–
Ag (cr)	0^[1]	0^[1]	42.55^[1]	25.351^[1]
Ag (g)	284.55^[1]	245.65^[1]	172.997^[1]	20.786^[1]
N₂O₃ (l)	50.29^[1]	–	–	–
N₂O₃ (g)	83.72^[1]	139.46^[1]	312.28^[1]	65.61^[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]

* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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	−297.48 kJ/mol
K	1.31 × 10⁵²
pK	−52.12

Δ_rG	−301.71 kJ/mol
K	7.20 × 10⁵²
pK	−52.86

Δ_rG	−302.20 kJ/mol
K	8.77 × 10⁵²
pK	−52.94

Δ_rG	−305.05 kJ/mol
K	2.77 × 10⁵³
pK	−53.44

H2S + 2AgNO3 → SO2 + 2Ag + N2O3 + H2O

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition

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

H₂S + 2AgNO₃ → SO₂ + 2Ag + N₂O₃ + H₂O