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4H2S + Mg(NO3)2 → 3S + 2NO + MgS + 4H2O

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Reaction of hydrogen sulfide and magnesium nitrate
4H2SHydrogen sulfide + Mg(NO3)2Magnesium nitrate
⟶
3SSulfur + 2NONitrogen monoxide + MgSMagnesium sulfide + 4H2OWater

The reaction of hydrogen sulfide and magnesium nitrate yields sulfur, nitrogen monoxide, 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

Reaction of hydrogen sulfide and magnesium nitrate
4H2SHydrogen sulfide + Mg(NO3)2Magnesium nitrate
⟶
3SSulfur + 2NONitrogen monoxide + MgSMagnesium sulfide + 4H2OWater

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 magnesium nitrate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide4
Reducing
Reducing
Mg(NO3)2Magnesium nitrate1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur3
Oxidized
–
NONitrogen monoxide2
Reduced
–
MgSMagnesium sulfide1
–
–
H2OWater4
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and magnesium nitrate
◆
ΔrG−393.6 kJ/mol
K9.03 × 1068
pK−68.96
4H2SGas + Mg(NO3)2Crystalline solid
⟶
3SCrystalline solidrhombic + 2NOGas + MgSCrystalline solid + 4H2OLiquid
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
−435.7−393.6−140.3195.49
per 1 mol of
−108.9−98.40−35.0848.873
per 1 mol of
−435.7−393.6−140.3195.49
per 1 mol of
−145.2−131.2−46.7765.163
per 1 mol of
−217.8−196.8−70.1597.745
per 1 mol of
−435.7−393.6−140.3195.49
per 1 mol of
−108.9−98.40−35.0848.873

Changes in standard condition (2)

Reaction of hydrogen sulfide and magnesium nitrate
4H2SGas + Mg(NO3)2Crystalline solid
⟶
3SCrystalline solidmonoclinic + 2NOGas + MgSCrystalline solid + 4H2OLiquid
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
−434.7–––
per 1 mol of
−108.7–––
per 1 mol of
−434.7–––
per 1 mol of
−144.9–––
per 1 mol of
−217.3–––
per 1 mol of
−434.7–––
per 1 mol of
−108.7–––

Changes in aqueous solution

Reaction of hydrogen sulfide and magnesium nitrate
◆
ΔrG−328.6 kJ/mol
K3.70 × 1057
pK−57.57
4H2SUn-ionized aqueous solution + Mg(NO3)2Ionized aqueous solution
⟶
3SCrystalline solidrhombic + 2NOGas + MgSCrystalline solid + 4H2OLiquid
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
−268.5−328.6208–
per 1 mol of
−67.13−82.1552.0–
per 1 mol of
−268.5−328.6208–
per 1 mol of
−89.50−109.569.3–
per 1 mol of
−134.3−164.3104–
per 1 mol of
−268.5−328.6208–
per 1 mol of
−67.13−82.1552.0–

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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
NO (g)90.25[1]86.55[1]210.761[1]29.844[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]
* (cr):Crystalline solid, (g):Gas, (l):Liquid

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)