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5H2S + 3Mg(NO3)2 → 2SO2 + 3N2O3 + 3MgS + 5H2O

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

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide5
Reducing
Reducing
Mg(NO3)2Magnesium nitrate3
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide2
Oxidized
N2O3Dinitrogen trioxide3
Reduced
MgSMagnesium sulfide3
H2OWater5

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and magnesium nitrate
ΔrG−457.1 kJ/mol
K1.20 × 1080
pK−80.08
5H2SGas + 3Mg(NO3)2Crystalline solid
2SO2Gas + 3N2O3Gas + 3MgSCrystalline solid + 5H2OLiquid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−334.6−457.1412.9192.80
per 1 mol of
−66.92−91.4282.5838.560
per 1 mol of
−111.5−152.4137.664.267
per 1 mol of
−167.3−228.6206.496.400
−111.5−152.4137.664.267
per 1 mol of
−111.5−152.4137.664.267
per 1 mol of
−66.92−91.4282.5838.560

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and magnesium nitrate
ΔrG−222.0 kJ/mol
K7.81 × 1038
pK−38.89
5H2SUn-ionized aqueous solution + 3Mg(NO3)2Ionized aqueous solution
2SO2Gas + 3N2O3Gas + 3MgSCrystalline solid + 5H2OLiquid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
33.6−222.0864
per 1 mol of
6.72−44.40173
per 1 mol of
11.2−74.00288
per 1 mol of
16.8−111.0432
11.2−74.00288
per 1 mol of
11.2−74.00288
per 1 mol of
6.72−44.40173

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and magnesium nitrate
ΔrG−223.0 kJ/mol
K1.17 × 1039
pK−39.07
5H2SUn-ionized aqueous solution + 3Mg(NO3)2Ionized aqueous solution
2SO2Un-ionized aqueous solution + 3N2O3Gas + 3MgSCrystalline solid + 5H2OLiquid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−18.7−223.0692
per 1 mol of
−3.74−44.60138
per 1 mol of
−6.23−74.33231
per 1 mol of
−9.35−111.5346
−6.23−74.33231
per 1 mol of
−6.23−74.33231
per 1 mol of
−3.74−44.60138

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
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]
Mg(NO3)2 (cr)-790.65[1]-589.4[1]164.0[1]141.92[1]
Mg(NO3)2 (ai)-881.57[1]-677.3[1]154.8[1]
Mg(NO3)2 (cr)
2 hydrate
-1409.2[1]
Mg(NO3)2 (cr)
6 hydrate
-2613.28[1]-2080.3[1]452[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
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]
N2O3 (l)50.29[1]
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[1]
MgS (cr)-346.0[1]-341.8[1]50.33[1]45.56[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. 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
    National Institute of Standards and Technology (NIST)