You-iggy
  1. Home
  2. Chemical reactions
  3. 8KHS + 2HNO3 → 4K2S + 3SO2↑ + (NH4)2S + H2↑

8KHS + 2HNO3 → 4K2S + 3SO2↑ + (NH4)2S + H2↑

Last updated:
Reaction of potassium hydrogensulfide and nitric acid
8KHSPotassium hydrogensulfide + 2HNO3Nitric acid
⟶
4K2SPotassium sulfide + 3SO2↑Sulfur dioxide + (NH4)2SAmmonium sulfide + H2↑Hydrogen

The reaction of potassium hydrogensulfide and nitric acid yields potassium sulfide, sulfur dioxide, ammonium sulfide, and hydrogen (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
8KHSPotassium hydrogensulfide + 2HNO3Nitric acid
⟶
4K2SPotassium sulfide + 3SO2↑Sulfur dioxide + (NH4)2SAmmonium sulfide + H2↑Hydrogen

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 hydrogensulfide8
Reducing
Reducing
HNO3Nitric acid2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SPotassium sulfide4
–
–
SO2Sulfur dioxide3
Oxidized
–
(NH4)2SAmmonium sulfide1
Reduced
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of potassium hydrogensulfide and nitric acid
◆
ΔrG−504.0 kJ/mol
K1.98 × 1088
pK−88.30
8KHSIonized aqueous solution + 2HNO3Ionized aqueous solution
⟶
4K2SIonized aqueous solution + 3SO2↑Gas + (NH4)2SIonized aqueous solution + H2↑Gas
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
−434.4−504.0233.8–
−54.30−63.0029.23–
per 1 mol of
−217.2−252.0116.9–
per 1 mol of
−108.6−126.058.45–
per 1 mol of
−144.8−168.077.93–
per 1 mol of
−434.4−504.0233.8–
per 1 mol of
−434.4−504.0233.8–

Changes in aqueous solution (2)

Reaction of potassium hydrogensulfide and nitric acid
◆
ΔrG−486.4 kJ/mol
K1.64 × 1085
pK−85.21
8KHSIonized aqueous solution + 2HNO3Ionized aqueous solution
⟶
4K2SIonized aqueous solution + 3SO2↑Gas + (NH4)2SIonized aqueous solution + H2↑Un-ionized 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
−438.6−486.4680–
−54.83−60.8085.0–
per 1 mol of
−219.3−243.2340–
per 1 mol of
−109.7−121.6170–
per 1 mol of
−146.2−162.1227–
per 1 mol of
−438.6−486.4680–
per 1 mol of
−438.6−486.4680–

Changes in aqueous solution (3)

Reaction of potassium hydrogensulfide and nitric acid
◆
ΔrG−505.4 kJ/mol
K3.49 × 1088
pK−88.54
8KHSIonized aqueous solution + 2HNO3Ionized aqueous solution
⟶
4K2SIonized aqueous solution + 3SO2↑Un-ionized aqueous solution + (NH4)2SIonized aqueous solution + H2↑Gas
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
−512.8−505.4−25.1–
−64.10−63.17−3.14–
per 1 mol of
−256.4−252.7−12.6–
per 1 mol of
−128.2−126.3−6.28–
per 1 mol of
−170.9−168.5−8.37–
per 1 mol of
−512.8−505.4−25.1–
per 1 mol of
−512.8−505.4−25.1–

Changes in aqueous solution (4)

Reaction of potassium hydrogensulfide and nitric acid
◆
ΔrG−487.8 kJ/mol
K2.88 × 1085
pK−85.46
8KHSIonized aqueous solution + 2HNO3Ionized aqueous solution
⟶
4K2SIonized aqueous solution + 3SO2↑Un-ionized aqueous solution + (NH4)2SIonized aqueous solution + H2↑Un-ionized 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
−517.0−487.8421–
−64.63−60.9852.6–
per 1 mol of
−258.5−243.9211–
per 1 mol of
−129.3−122.0105–
per 1 mol of
−172.3−162.6140–
per 1 mol of
−517.0−487.8421–
per 1 mol of
−517.0−487.8421–

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
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]–––
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]–
(NH4)2S (ai)-231.8[1]-72.6[1]212.1[1]–
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (ao):Un-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)