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4KHS + 10HNO3 → 4KNO3 + H2SO3 + 3SO2↑ + 3NH4NO3

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Reaction of potassium hydrogensulfide and nitric acid
4KHSPotassium hydrogensulfide + 10HNO3Nitric acid
⟶
4KNO3Potassium nitrate + H2SO3Sulfurous acid + 3SO2↑Sulfur dioxide + 3NH4NO3Ammonium nitrate

The reaction of potassium hydrogensulfide and nitric acid yields potassium nitrate, sulfurous acid, sulfur dioxide, and ammonium nitrate (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 potassium hydrogensulfide and nitric acid
4KHSPotassium hydrogensulfide + 10HNO3Nitric acid
⟶
4KNO3Potassium nitrate + H2SO3Sulfurous acid + 3SO2↑Sulfur dioxide + 3NH4NO3Ammonium nitrate

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 potassium hydrogensulfide and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KHSPotassium hydrogensulfide4
Reducing
Reducing
HNO3Nitric acid10
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
KNO3Potassium nitrate4
–
–
H2SO3Sulfurous acid1
Oxidized
–
SO2Sulfur dioxide3
Oxidized
–
NH4NO3Ammonium nitrate3
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium hydrogensulfide and nitric acid
◆
ΔrG−1390.93 kJ/mol
K4.79 × 10243
pK−243.68
4KHSIonized aqueous solution + 10HNO3Ionized aqueous solution
⟶
4KNO3Ionized aqueous solution + H2SO3Un-ionized aqueous solution + 3SO2↑Gas + 3NH4NO3Ionized 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
−1204.7−1390.93626.7–
−301.18−347.733156.7–
per 1 mol of
−120.47−139.09362.67–
per 1 mol of
−301.18−347.733156.7–
per 1 mol of
−1204.7−1390.93626.7–
per 1 mol of
−401.57−463.643208.9–
per 1 mol of
−401.57−463.643208.9–

Changes in standard condition (2)

Reaction of potassium hydrogensulfide and nitric acid
◆
ΔrG−1392.38 kJ/mol
K8.60 × 10243
pK−243.93
4KHSIonized aqueous solution + 10HNO3Ionized aqueous solution
⟶
4KNO3Ionized aqueous solution + H2SO3Un-ionized aqueous solution + 3SO2↑Un-ionized aqueous solution + 3NH4NO3Ionized 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
−1283.1−1392.38367.7–
−320.77−348.09591.92–
per 1 mol of
−128.31−139.23836.77–
per 1 mol of
−320.77−348.09591.92–
per 1 mol of
−1283.1−1392.38367.7–
per 1 mol of
−427.70−464.127122.6–
per 1 mol of
−427.70−464.127122.6–

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
KHS (cr)-265.10[1]––75.31[1]
KHS (ai)-269.9[1]-271.19[1]165.3[1]–
KHS (cr)
0.25 hydrate
-337.2[1]–––
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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
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]
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]–
NH4NO3 (cr)-365.56[1]-183.87[1]151.08[1]139.3[1]
NH4NO3 (ai)-339.87[1]-190.56[1]259.8[1]-6.7[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas

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)