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10H2S + 6KNO3 → 4H2SO3 + 3SO2 + 3N2H4 + 3K2S

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Reaction of hydrogen sulfide and potassium nitrate
10H2SHydrogen sulfide + 6KNO3Potassium nitrate
⟶
4H2SO3Sulfurous acid + 3SO2Sulfur dioxide + 3N2H4Hydrazine + 3K2SPotassium sulfide

The reaction of hydrogen sulfide and potassium nitrate yields sulfurous acid, sulfur dioxide, hydrazine, and potassium sulfide (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 potassium nitrate
10H2SHydrogen sulfide + 6KNO3Potassium nitrate
⟶
4H2SO3Sulfurous acid + 3SO2Sulfur dioxide + 3N2H4Hydrazine + 3K2SPotassium sulfide

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 potassium nitrate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide10
Reducing
Reducing
KNO3Potassium nitrate6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2SO3Sulfurous acid4
Oxidized
–
SO2Sulfur dioxide3
Oxidized
–
N2H4Hydrazine3
Reduced
–
K2SPotassium sulfide3
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and potassium nitrate
◆
ΔrG−1464.1 kJ/mol
K3.16 × 10256
pK−256.50
10H2SUn-ionized aqueous solution + 6KNO3Ionized aqueous solution
⟶
4H2SO3Un-ionized aqueous solution + 3SO2Gas + 3N2H4Un-ionized aqueous solution + 3K2SIonized aqueous solution
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
−1481.9−1464.1−45–
per 1 mol of
−148.19−146.41−4.5–
per 1 mol of
−246.98−244.02−7.5–
per 1 mol of
−370.48−366.02−11–
per 1 mol of
−493.97−488.03−15–
per 1 mol of
−493.97−488.03−15–
per 1 mol of
−493.97−488.03−15–

Changes in standard condition (2)

Reaction of hydrogen sulfide and potassium nitrate
◆
ΔrG−1465.6 kJ/mol
K5.78 × 10256
pK−256.76
10H2SUn-ionized aqueous solution + 6KNO3Ionized aqueous solution
⟶
4H2SO3Un-ionized aqueous solution + 3SO2Un-ionized aqueous solution + 3N2H4Un-ionized aqueous solution + 3K2SIonized aqueous solution
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
−1560.3−1465.6−304–
per 1 mol of
−156.03−146.56−30.4–
per 1 mol of
−260.05−244.27−50.7–
per 1 mol of
−390.07−366.40−76.0–
per 1 mol of
−520.10−488.53−101–
per 1 mol of
−520.10−488.53−101–
per 1 mol of
−520.10−488.53−101–

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]–
KNO3 (cr)-494.63[1]-394.86[1]133.05[1]96.40[1]
KNO3 (ai)-459.74[1]-394.53[1]248.9[1]-64.9[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
H2SO3 (ao)-608.81[1]-537.81[1]232.2[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]–
N2H4 (l)50.63[1]149.34[1]121.21[1]98.87[1]
N2H4 (g)95.40[1]159.35[1]238.47[1]49.58[1]
N2H4 (ao)34.31[1]128.1[1]138[1]–
K2S (cr)-380.7[1]-364.0[1]105[1]–
K2S (ai)-471.5[1]-480.7[1]190.4[1]–
K2S (cr)
2 hydrate
-975.3[1]–––
K2S (cr)
5 hydrate
-1871.5[1]–––
* (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas, (cr):Crystalline solid, (ai):Ionized aqueous solution

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)